Endothermic reactions are a fascinating and crucial aspect of chemistry, where the system absorbs heat from its surroundings, leading to a decrease in temperature. These reactions are in stark contrast to exothermic reactions, which release heat and cause an increase in temperature. Understanding the intricacies of endothermic reactions is essential for science students, as it … Read more
The Mannich reaction is a powerful three-component condensation reaction that involves an enolizable carbonyl compound, a primary or secondary amine, and a non-enolizable aldehyde. This reaction proceeds through the formation of an iminium ion intermediate, which then reacts with the enol form of the carbonyl compound to produce a β-amino carbonyl compound known as a … Read more
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In this article, “synthesis reaction example”, different types of synthesis (Williamson synthesis, balanced synthesis and peptide synthesis) example with detailed explanations are discusses briefly.
Synthesis reaction is one type of chemical reaction in which two different atoms involve in the reaction, react with each other to form a totally different molecular compound. In most of the synthesis reaction, energy is released from the reaction medium and known as exothermic reaction.
Synthesis Reaction
Example of Williamson Synthesis
Synthesis of ethyl methyl ether
Williamson synthesis process is the best method to synthesis ethyl methyl ether (CH3-O- CH2CH3). This reaction proceeds through SN2 pathway. To obtain ethyl methyl ether as the synthesized product, sodium methoxide (CH3ONa) and ethyl chloride (C2H5Cl) reacts with each other. Sodium methoxide acts as nucleophile and attacks the electrophilic centre of ethyl chloride to eliminate the leaving group (Cl–). Ethyl methyl ether is obtained as the Williamson synthesized product.
Synthesis of Ethyl Methyl Ether
Synthesis of anisole
This ether can also be synthesized by Williamson ether synthesis. To obtain anisole, sodium phenoxide (C5H5ONa) will react with methyl iodide (CH3I) and sodium phenoxide (nucleophile) attacks the electrophilic centre of methyl iodide. Iodide (I–) will be eliminated as it is a good leaving group and anisole is formed.
To proceed this reaction, hydroxyl group should be inserted at the 2 position of naphthalene group and reacts with bromoethane. The reaction medium should be basis. Thus, sodium hydride (NaH) is used. Nucleophilic oxygen atom of OH group in naphthalene attacks the CH2 centre of CH3CH2Br and Br– is eliminated as the leaving group.
Synthesis of 2-ethoxynaphthalene
Synthesis of Phenyl Propyl Ether
To synthesis phenyl propyl ether the reactants that are chosen are phenol, sodium metal and n-propyl bromide. Solvent that is used in this synthesis reaction is a polar aprotic solvent. The first step is to react phenol with sodium to form sodium phenoxide (active nucleophile). This nucleophile reacts with n-propyl bromide (electrophile) to synthesize phenyl propyl ether after elimination of bromide ion.
William synthesis pathway is followed for the formation of benzyl-tertbutyl ether. Sodium tert-butoxide and benzyl bromide is taken as the reactants. O– ion from sodium tert-butoxide attacks the electron deficient centre of benzyl bromide Br– is eliminated as the leaving group to form the desired product.
Synthesis of benzyl tert-butyl ether
Synthesis of tert-butyl methyl ether
This synthesis process almost similar to the synthesis of benzyl tert-butyl ether. One of the reactants is also same, sodium tert-butoxide and the another reactant is methyl bromide (CH3Br). Tertiary sodium tert butoxide reacts as nucleophile and attacks the methyl carbon center to eliminate bromide ion.
In this process of synthesis of ethoxy benzene, Williamson synthesis process is followed. Sodium ethoxide reacts with phenyl bromide to form ethoxy benzene. O– attacks the electrophilic centre of phenyl bromide and ethoxy benzene is obtained.
Synthesis of Ethoxy benzene
Synthesis of Cyclopentyl methyl ether
In this Williamson ether synthesis, cyclopentanol and methyl bromide is reacted with each other in a basic medium. In presence of base, hydrogen in O-H bond is eliminated and O– attacks the methyl bromide to form the cyclopentyl methyl ether.
Synthesis of cyclepentyl methyl ether
Example of Balanced Synthesis
Synthesis of Water
Hydrogen and oxygen-these two gases are the two main reactants of this synthesis. Water molecule that is formed is also in gaseous state. Two molecules of hydrogen react with one molecule of oxygen to form water molecule. Dissociation of water is taken place by passing electric through water.
Carbon dioxide is synthesized during the different decay process of various different material and fermentation of sugars. It can be produced by combustion process of wood or other organic materials. Another procedure is to react metal carbonates with dilute acid for the formation of water. For example, carbon dioxide can be synthesized by the reaction between sodium carbonate with dilute HCl.
Synthesis of Ammonia
Haber-Bosch process is the most well known process to synthesize ammonia. High pressure and high temperature is the two most important driving force of ammonia production. It is an exothermic process (del H= -91.8 KJ/mol). Ammonia is widely used as fertilizer.
Aluminium hydroxide is the main reactant for the formation of aluminium oxide. Solid Al(OH)3 is decomposed over 11000C and form aluminium oxide (Al2O3). Besides that aluminium is oxidized in presence of oxygen to form aluminium oxide.
2Al(OH)3 = (Al2O3) + 3H2O
4Al (s) + 3O2 (g)= 2Al2O3
Synthesis of Iron Sulfide
Iron after reaction with sulfur forms iron sulfide (pyrrhotite) in presence of heat energy. Iron sulphide (FeS) has totally different physical and chemical properties with respect to two reactants, iron and sulphur. The ratio of iron with sulphur is 1:1. Equal amount of iron is reacted with equal amount of sulphur to form iron sulphide.
Fe + S = FeS
Synthesis of Potassium Chloride
Potassium chloride is basically an ionic salt. It can be synthesized by the reaction bases of potassium like potassium hydroxide (KOH) with strong acid, hydrochloric acid. In this synthesis reaction, strong acid (HCl) is completely neutralized by strong base (KOH). Water is also produced along with the KCl.
KOH (aq) + HCl (aq) = KCl (s) + H2O (liq)
Formation of Rust
Rust is reddish brown iron oxide formed by reacting iron with oxygen. Water or air takes part in this synthesis reaction as catalyst. Chemical formula of rust is Fe2O3.Nh2O and iron oxide hydroxide (FeO (OH),Fe(OH)3).
Fe(OH)2 = FeO + H2O
Fe(OH)3 = FeO(OH) + H2O
2FeO(OH) = Fe2O3 +H2O
Synthesis of Calcium Carbonate
In this synthesis reaction, calcium oxide (CaO) and carbon dioxide is reacted to form calcium carbonate. At first step, calcium hydroxide is prepared by the reaction between calcium oxide with water. After that Ca(OH)2 is reacted with carbon dioxide and as a product calcium carbonate is obtained.
CaO +H2O = Ca(OH)2
Ca(OH)2 +CO2 = CaCO3 +H2O
Synthesis of Zinc Oxide
High temperature is one of the most important driving forces. Zinc vapour is reacted with air (oxygen) at 9100 C. It is mainly an oxidation process and ZnO is produced.
Example of Peptide Synthesis
Synthesis of dipeptide (Gly–Ala)
To synthesis of a dipeptide the following steps should be followed-
At first alpha amino group of glycine should be blocked by tert-butyloxycarbonylchloride.
After giving the protection to alpha amino acid of glycine, alanine will react with the previously formed compound.
Then the tert-butyloxycarbonylchloride group is eliminated by reacting with dilute acid and dipeptide (ala-gly) is obtained as the final product.
Synthesis of Gly-Ala
Solid Phase Peptide Synthesis
This synthesis procedure is known as Merrifield synthesis discovered by scientist R.Bruce Merrifield. In this peptide synthesis procedure, homogenous solution is not used for deprotection. This deprotection is carried out at the surface of an insoluble polymer or any solid support.
The carboxyl terminal amino acid is covalently linked with the Merrifield Resin and the length of the peptide chain is increased. Reagents are used to remove the resin with the soluble by products from the peptide chain and at the end desired peptide chain is obtained.
In this article, “is oxidation a redox reaction” basic similarities, differences and comparison between oxidation and redox reaction with detailed explanations are discussed briefly.
In redox reaction, oxidation and reduction must be taken place simultaneously. Exchange of electrons is the basic requirement of any redox reaction. But in oxidation reaction, one reactant is oxidized in presence of oxygen or any oxidizing agent to obtain the oxidized product.
Let discuss some frequently asked questions with answers on these two reactions below.
How is oxidation a redox reaction?
Redox reaction is comprised of two different half reactions that occurs together in a single redox reaction-
Oxidation half reaction
Reduction half reaction.
Exchanging of electrons between two reactants is the most important criteria to be fulfilled in a redox reaction. These two reactants are basically oxidized and reduced with the help of another reactant simultaneously. In the reduction half equation, reactants must gain electron(s) and in oxidation half reaction, reactant must lose electron(s) to obtain respective product. Number of electrons gained or lost during the redox reaction should be balanced properly to get the correct balanced redox equation.
Oxidation reaction basically signifies lose of electron by any reactant in presence of oxidizing agent. Oxidation number of that reactant is also increased by reacting with oxygen. Loss of hydrogen from any substance is also an example of oxidation reaction.
Redox reaction known as oxidation-reduction reaction. A redox reaction can be separated into two half reaction i.e oxidation and reduction half reaction. So, oxidation reaction must be involved in redox reaction.
In oxidation reaction, reactants react with oxygen and oxidation number of that particular species is increased in product than the reactant. With that the oxidation number of oxygen or any other oxidizing reagent by which the substance is oxidized is decreased in product. Thus, only oxidation can not take place separately in any reaction.
In redox reaction generally two reactants are present. Electrons are exchanged or transferred from one reactant to another and one oxidized with one reduced species are obtained as product.
In this above example, oxidation number of Fe in Fe2O3 is +3 which is changed to 0 in product side. Thus, this the reduction half reaction and oxidation number of carbon is +2 in CO but it is changed to +4 in CO2. So, it is the part of oxidation half reaction.
Let balance the above equation-
Change of oxidation number for oxidation half reaction and reduction half reaction is 2 and 3 respectively. Thus, net balanced equation is-
Fe2O3 +3CO → 2Fe + 3CO2
What happens in a redox reaction?
Redox reaction is nothing but the electron transfer between two substances. One reactant is oxidized and another reactant is reduced due to exchanging of electrons. In oxidation process, reactant loses its electrons while in reduction, reactant gains electrons in a single redox reaction.
In this above example, Zn is oxidized to Zn2+ and lost two electrons and the oxidizing agent is H+. So, the oxidation half reaction is: Zn (s) → Zn2+ (aq). Similarly, H+ is reduced to H2 by accepting two electrons with the help of Zn. Thus,Zn acts as reducing agent and H+ acts an oxidizing agent. Reduction half equation will be 2H+ (aq) → H2 (g)
Oxidation reaction is nothing but the increasing of oxidation number or loosing of one or more than one electron. Oxidation state is increased in the time of oxidation.
It is not always fixed that oxidation can only take place in presence of oxygen, any other oxidizing agent can participate in oxidation reaction. The purpose of adding of oxygen or oxidizing agent is to accept the electrons which are donated by the reactant to obtain the oxidized product. Reverse reaction of oxidation is reduction which is nothing but the gaining of electrons.
Relationship between Redox Reactions and Oxidation Reaction
In a redox reaction, reduction and oxidation take place at the same time. Oxidizing agent (oxidizes other chemical species) accepts electrons from reducing agent (reduces other one) to be reduced. Basically, it is an electron transfer reaction. Oxidized species lose electrons and reduced species gains electron in redox reaction, Thus, redox reaction can be divided into two parts- oxidation and reduction half reaction.
The process, oxidation must be present in a redox reaction.
In this above example, Ce4+ is reduced to Ce3+ and Fe2+ is oxidized to Fe2+ is oxidized to Fe3+. The above reaction is an example of redox reaction as both oxidation and reduction are involved in this reaction through transferring of electrons between two reactants.
The body of this research would be represented with the broadened examples of Oxidation reaction that are happened naturally as well as chemically.
Oxidation Reaction example holds different types of reactions those are listed below:
OXIDATION REACTION
During chemical reaction if the reactant or the reactants loses on or more than one electron from the atoms then that chemical reaction is called Oxidation reaction. This is the fundamental concept of oxidation.
A historical overview of the oxidation reaction can be presented here also that is the addition of oxygen molecule with the reactants and formation of new type of compounds. Those compounds can be called as oxides.
Basically, this type of reaction happens with the metals when they form oxides in their oxidation states by gaining oxygen molecule. Now, oxidation state refers to the states where the metals require electrons for being more stable and achieve octets.
These kinds of oxide formation could be taken as an example of oxidation reaction. There are more examples can e referred in this research broadly to make deep understanding about the process and concept of oxidation reaction.
Rust
Rusting is referred as the best oxidation reaction example. In this reaction, the Iron metals (Fe) are noticed to be oxidised by the touch of moist air if the materials made of iron are kept openly in the nature. This happens due to the chemical reaction between Fe, oxygen and water present in the air.
Oxygen molecule gets added with the openly kept Fe metals and oxidise it into Ferric oxide (hydrated) that is the hydrated iron. However, this process has been identified to be happened very naturally without any external addition of elements. This is why it is considered to the most natural oxidation reaction in the nature.
The fundamental and historical concept of oxidation reaction which has been shortly described above creates high support for explanation of rusting as an oxidation reaction.
Chemical equation of this reaction is given below:
4Fe + 3O2 + 6H2O = 4Fe(OH)3
This reaction can accompanied as an example of a rusting with the presentation of certain amount of molecules but most of the time this reaction is noticed to be happened in general way. In that case the number of water molecule in the ferric oxide cannot be defined with exact proportion. Then the rust or the product is expressed as Fe2O3. n(H2O).
In a very natural context oxidation happens regularly at each and every moment in animal world by the process of respiration. Breathing is considered to the most important factor for animal and for them as they are completely dependent on Oxygen. Therefore, oxygen consumption is the foremost part of breathing or respiration.
Basically, respiration is the combination of reduction and oxidation both the processes which is called redox reaction (reduction reaction is absolutely opposite reaction of oxidation reaction). The oxidation part is quite dominating in this process.
Oxidation happens in respiration when the oxygen molecule from air is inhaled by the animals and the absorbed oxygen molecule oxidises the food particles to extract energy from them.
Several metabolic processes happen in the body while proceeding through respiration. And those happen by following the principles of oxidation reactions. The products come from those reactions are quite effective in animal body to keep the internal processes very active and healthy.
However, based on the electronic concept it can be said that both the loss and gain of electron happen in the respiration process. Therefore, oxidation plays a huge role to conduct this natural process.
Example of chemical equation of respiration is given below:
In the above equation it is clear that Glucose is losing electron and producing carbon Dioxide. This is considered as a specific proof of oxidation reaction.
Electrochemical reactions
Electrochemical reactions are best to be mentioned as the effective examples of oxidation reactions. These reactions are considered to be perfect as these maintain the electronic principles of oxidation reaction. It can be represented with the description of a reaction between copper and silver ion.
When a copper wire dipped into a solution that contains silver ions, copper leaves elections and silver ions adopt those electron. Leaving the electron is the main principle of following oxidation reaction.
Equation of the above reaction:
Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s)
The above example is taken as the most effective example of oxidation reaction as it is responsible for clarifying the core concept of oxidation reaction in an easy way. The understandings are very reliable to support the idea oxidation reaction.
Combustion
In a very language it can be said that combustion is the chemical term of burning process. In presence of oxygen gas when organic compounds burn and produce carbon Dioxide and water then that process is called combustion.
Any kind of organic compound can burn in presence of oxygen. Rather it can be accompanied that oxygen is the main substance which influence the process of combustion or burning. Therefore, it is quite justified that combustion is one of the perfect example of oxidation reaction.
Combustion as an oxidation reaction example from Wikimedia
A simplest example of combustion reaction can be taken under consideration that is, the reaction between gaseous methane and oxygen gas gives out water and Carbon Dioxide molecule.
Chemical equation of the reaction:
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
One matter should be understood in this case that is all combustion reactions are complete example of oxidation reaction but all oxidation reaction do not stand for combustion reaction.
Oxide formation
Generally the metals lose election and combine with oxygen and form metal oxides (MO). This is the fundamental concept of oxide formation. Here the example of formation of magnesium oxide (MgO) can be referred as the basic and simplest example of oxidation.
Mg loses 2 election and use to be oxidised and oxygen gas takes those two free electrons and get reduced. The reduction of oxygen gas completely depends on the ability of Mg in losing the electrons. Therefore, oxidation gets more priority in this reaction and makes an effective example of the core principle of the reaction.
Chemical equation of the above exaction:
2 Mg + O2 → 2 [Mg2+][O2-]
Or
2 Mg (s) + O2 (g) → 2 MgO (s)
Loss of hydrogen
This concept holds exactly the opposite definition of the oxidation reaction which is defined in terms of oxygen. The hydrogen related definition of the oxidation reaction is also one kind of historic definition which supports the concept of losing hydrogen from a compound. This loss of hydrogen is also an oxidation reaction example.
Photosynthesis is also a combination of oxidation and reduction reaction. As this is a lengthy process it holds both type of reaction. Therefore, it cannot be considers as the completely oxidation process.
In photosynthesis a vital part of reaction poses the principle of oxidation when the water molecules get oxidised and produce molecular oxygen. This part cannot be ignored because that produced oxygen a huge biological impact in the nature.
Oxidation reaction in photosynthesis from Wikimedia
This oxidation process is considered to the part of biochemical world which holds great significance in living world.
Frequently Asked Questions (FAQs)
Question 1: Are oxidation and reduction reactions dependent on each other?
Answer: In the combination of Redox reaction Reduction definitely depends on oxidation reaction simultaneously oxidation also depends on reduction as when reduction (gaining the free electrons) happens, oxidation (generating free electrons) must take place to support to the reduction reaction.
Question 2: How do oxides occur from metal molecules?
Answer: Oxide formation takes place in the metals by losing electron, metals actually loses electron for filling octet state and get stabilised. When oxygen gas receives the free electrons and combines with the metals and forms metal oxides.
Question 3: What is the best example of oxidation reaction and why?
Answer: Electrochemical reactions are the best example of oxidation reaction. These reactions describe the methods of oxidation reaction that the loss of electron from atoms very precisely by following all the core principles of the reaction.
Question 4: How does rusting support the concept of oxidation reaction?
Answer: Rusting shows huge support to the concept of oxidation reaction. It is completely happens through the presence of oxygen gas. Without reacting with oxygen, iron metal would not achieve its oxide form. It is also an example of oxide formation.
Question 5: Can we consider all oxidation reaction as combustion reaction?
Answers: All oxidation reaction cannot be conspired as combustion. Combustion is the concept of burning process of organic compound sin presence of oxygen gas but oxidation dies not takes place to influence burning always. Oxidation can happen in low or moderate temperature as well. Therefore, all oxidation reaction does not stand for combustion reaction.
An exergonic reaction example is cellular respiration, where glucose (C6H12O6) combines with oxygen (O2) to produce carbon dioxide (CO2), water (H2O), and energy. It releases approximately 686 kilocalories per mole of glucose, illustrating a high-energy yield and entropy increase, characteristic of exergonic reactions.Exergonic reaction example has been listed below:
Exergonic Reaction
Exergonic reaction refers to the idea of chemical reaction which releases a certain amount of negative energy. This reaction comes under the chemical thermodynamics part of chemistry. It is highly conserved with the concept of realising free energies once the reaction is done. The net amount of free energy release indicates that the process is quite spontaneous and happens in a closed system.
However, one condition can be found in this type of chemical reaction that is the initial and final temperature of the system would be same. Generally in a constant temperature a certain amount of Gibbs free energy or Helmholtz energy is required for proceeding with any chemical reaction process.
One of the most important factors that should be understood that is the exergonic reactions do not need energy from outside. Constant temperature is the only criterion for getting the outcomes as the product and the free energies. There are various examples that can be described from in the thermodynamics context of the study.
Cellular Respiration
This is one of the most relevant examples of exergonic reaction which biologically happens in human body. This is basically the chemical reaction which follows the pathway of exergonic reaction. The main reactants in this process are Carbon Dioxide, water, Glucose and oxygen. These are considered as the main substances which react with each other. As a result free energy molecules are released from this reaction simultaneously with the products.
Basically, Cellular respiration involves in the process of extracting free energy molecules on the form of ATP (Adenosine Tri Phosphate) in the human body which stores energy in the cellular organ Mitochondria. Not only in human body can it be happened in every living being. Most of the chemical reaction regarding Cellular respiration process happens in Mitochondria.
All the way it produces energies or calories in constant and normal body temperature without consuming extra heat or energy from the outside so it is considered as the most relevant example of the exergonic reaction. It happens completely by based on the chemical pathway that shows by the exergonic reactions. All the principles of this reaction can be seen as engaged in the cellular respiration process. This internal chemical process is biologically supported and it can be expressed with chemical formula as well.
Chemical Reaction: C6H12O6 +6O2 = 6CO2 + 6H2O + Energy (36-38 molecules of ATP)
The net amount of 36 to 38 ATP are formed and stored in the mitochondria, the actual products in this chemical reaction are water and Carbon Dioxide. These products are released by human being from the body as well. The energy it produces is stored for future use in the body in case of doing any kind of physical work. Nevertheless, this example can be considered as the simplest example of exergonic reaction which is happening each and every moment in the animal body.
Glycolysis
Glycolysis is also considered as a strong and exact example of exergonic reaction. This process is also simple one but in this one the present of catalyst is quite highlighted anyway. The overall process maintains the thermodynamic concept of exergonic reaction.
In this process some energy has been released with the products after a chemical reaction happens between several chemical components. This reaction is a lengthy one which possesses more than two steps. Therefore, the present of catalyst is required here.
It can be seen that the Phosphofructokinase, Hexokinase and pyruvate kinase are the most important three catalysts which positively provides driving force to the chemical reaction. However, Pyruvate and ATP are the final product comes from the breakage of glucose in present of mentioned catalysts.
The release of free energy molecules in a constant temperature proves that these chemical reactions also follow the pathway of exergonic reaction. Though the stored ATP in living beings helps to break the glucose in this process, the formation of extensive amount of free energy makes this process powerful for considering it as an exergonic reaction.
The breakdown of fatty acid is another biochemical reaction which integrates the idea of exergonic reaction. This process is highly spontaneous and the breakdown of fatty acid releases a certain amount of energy. This is also supported by the biological facts in the human body.
The presence of enzymes boosts up these reactions and makes it grow rapidly in body by producing a large amount of heat and energy. This catabolism of fatty acid also happens in normal body temperature. Therefore,. The temperature is considered as constant in this case as well. Fatty acids are large molecules.
It is very natural that in the breaking process of these molecules gives out a large amount of energy in the place of reaction. The enzymes work here as the valuable catalysts of this reaction. The long chains in fatty acids store the wholesome energy which gets released by the influence of the enzymes. The long chains of fatty acid break sin small chunks of the energy.
It stores more energy than the glucose or sugar molecules. This process spontaneously creates high energy in the body accordingly it releases Carbon Dioxide just as the cellular respiration process. Normally this process happens in the outer membrane of Mitochondria. Catabolism refers to the breakdown process. Therefore, it can be considered as the exergonic reaction. The thermodynamic expression is highlighted in its chemical formula.
Chemical reaction: fatty acid and Coenzyme A reacts in presence of AMP and PPi (forms from ATP breakdown) and gives Fatty acyl coenzyme A and water. The product contains the energy.
Combustion of Propane
This entirely is taken as a chemical example of exergonic reaction without any influence of biological aspects. This reaction can be a practical example by preceding it in artificial way. In the case of chemical reactions this process can be represented as the example of exergonic reaction by creating the environment suitable for exergonic reaction.
In a constant temperature and constant enthalpy Propane molecule reacts with oxygen and breaks into water and Carbon Dioxide and gives out certain amount of energy.
Chemical reaction: 5O2 + C3H8 = 4H2O + 3CO2 + energy
Frequently Asked Questions (FAQ)
Question 1: Can fatty acid metabolism be considered as an exergonic reaction?
Answer:-Fatty acid metabolism requires energy to provide from outside. Therefore, it can be said that this reaction consumes energy does not give out free energy molecules. This is also a chemical reaction but opposite of exergonic reaction. Fatty acid metabolism refers to the synthesis of fatty acid so it cannot be considered as an exergonic reaction.
Question 2: What is the fundamental condition for preceding an exergonic reaction and explain why that condition should be applied in this reaction?
Answer:- The fundamental condition is the constant temperature of the place where the reaction would be proceeded.
This is the fundamental condition as the exergonic reaction does not consume heat from outsides. Therefore, there is no need of changing the temperature of the reaction anyway.
Question 3: Why cellular respiration is highly considered as an example of exergonic reaction?
Answer:-Cellular respiration is considers as the most relevant example of exergonic reaction as it totally works under the fundamental chemical thermodynamic conditions of an exergonic reaction. It happens under constant temperature and enthalpy. It releases free energy that is the negative change in enthalpy happens in cellular respiration.
Question 4: What is the main product obtained from glycolysis process?
Answer:-Pyruvate is the main product that is obtained from Glycolysis process.
Question 5: Why fatty acids are appraised as the great storage of energy?
Answer:-Fatty Acid is a long chain of protein molecules it can be considered as the polymer of protein. Therefore, when it breaks being influenced by the work of enzymes a huge amount of energy released with the products.
Question 5: Give an example of pure chemical exergonic reaction, which can be happened artificially.
Answer:- Combustion of Propane is an example of exergonic reaction which produce negative enthalpy under artificially made circumstances for an exergonic reaction.
In this article, “how to balance redox reaction” different types of balancing method of redox reactions are discussed briefly.
Redox reaction is basically an electron transfer reaction. Electrons are donated by reducing agent to oxidizing agent to drive a redox reaction towards forward direction. Balancing of a redox reaction is essential to determine the number of electrons involved in the redox reaction.
Some frequently asked questions with answers on how to balance the redox reaction is described in this article.
How to balance a redox reaction in basic medium?
To balance any redox reaction in basic medium, these following steps must be maintained.
Oxidation and reduction half reaction will be determined at the very first step.
How to balance redox reaction by half reaction method?
Another method of balancing redox reaction is “half reaction method” or “half equation method”. Any redox reaction consists of two half reaction, oxidation and reduction half reaction. Research says that it is better and suitable method than oxidation number method of balancing redox reaction.
In the half reaction, atoms are balanced separately and after the balancing of all the participating atoms net balanced redox reaction is developed by adding the two half reactions. Not only the atoms, the electrons involved in redox reaction should be balanced before developing the net balanced equation.
Let’s take an example to clear the balancing method.
Fe2+ (aq) + Cr2O72- (aq) → Fe3+ (aq)+ Cr3+ (aq)
Oxidation half reaction: Fe2+→ Fe3+ + e– ———1 no equation
How to balance redox reaction by oxidation number method?
One of the methods of balancing redox reaction is oxidation number change method. As we all know that redox reaction is none other than electron transfer reaction and oxidation number must be changed due to the electron transfer.
Let’s account an example to make it clear.
Fe2O3 (s) + CO (g) → Fe (s) + CO2 (g)
In the above example, Fe is reduced to its +3 oxidation state to 0 oxidation state and carbon is oxidized by Fe2O3 and change of oxidation state takes place is from +2 to +4.
Oxidation- Reduction Reaction
Thus, oxidation number increases for the oxidation half reaction is 2 and for reduction half reaction oxidation number is decreased by 3. Least common number (LCM) of these two numbers (2 and 3) is 6. So, oxidation and reduction half reaction are multiplied by 3 and 2 respectively to balance the equation.
Oxidation number of nitrogen is decreased from +5 to +2 and increase of oxidation state of As is +2. The increase of oxidation number must be equal to the decrease of oxidation number.
These two integers are used as coefficients of the redox reaction and placed in front of the substances.
How to balance a redox reaction with only one reactant?
Formation of more than one product from one reactant in redox reaction is called disproportionation reaction. The one reactant is oxidized and reduced simultaneously.
These following steps should be followed to balance any disproportionation reaction-
The oxidation number of both the reactant and products should be determined.
Identify the atoms for which oxidation numbers are changed from reactant to product.
At the end integers are placed as coefficients before the substances to balance the redox reaction.
Let’s take an example to make it clear.
2CuCl → CuCl2+ Cu.
CuCl is only one reactant in this redox reaction. It is oxidized to CuCl2 and reduced to molecular Cu at a time. Oxidation number is changed for oxidation is +1 and -1 for reduction respectively. Thus, the coefficients “2” is multiplied with reactant and Cu to balance this equation.
Balancing of electrons that are gained and lost during a redox reaction is very important part of a redox reaction. All the methods are used to balance the redox reaction (ion electron method, oxidation number method, half equation method) must involve the balancing of electrons step.
Reduction half reaction: Al3++ 3e–→ Al ———-2 no equation
(1 no equation × 3)——— 3Mg→3Mg2+ + 6e–
(2 no equation × 2)——— 2Al3++ 6e–→ 2Al
Net balanced equation: 3Mg + 2Al3+→3Mg2+ + 2Al
Relationship between redox reactions and oxidation reaction
In a redox reaction both the oxidation and reduction take place simultaneously in a single reaction. If one reactant is oxidized then other reaction must be reduced in that reaction. But in oxidation reaction any substance is only oxidized by oxygen or any other oxidizing agent.
For example-
Magnesium is oxidized in presence of oxygen and form magnesium oxide (MgO) as product. In this reaction only oxidation takes place not reduction in the same reaction. But for the following reaction- Ce4+ + Fe2+ → Ce3+ + Fe3+. Ce4+is reduced to Ce3+ and Fe2+ is oxidized to Fe3+ simultaneously. So it is a redox reaction.
Image by Compost Camel – Wikimedia Commons, Wikimedia Commons, Licensed under CC BY-SA 4.0.Image by Grogu60 – Wikimedia Commons, Wikimedia Commons, Licensed under CC BY-SA 4.0.Image by Cmglee – Wikimedia Commons, Wikimedia Commons, Licensed under CC BY-SA 4.0.
redox reactions, short for oxidation-reduction reactions, are fundamental chemical processes that involve the transfer of electrons between reactants. Understanding how to identify and calculate redox reactions is crucial in the fields of chemistry and biology. In this blog post, we will explore the basics of redox reactions, learn how to identify them, delve into the calculations involved, and explore their practical applications.
Understanding the Basics of Redox Reactions
Redox reactions occur when there is a transfer of electrons between two species. One species loses electrons (undergoes oxidation) while the other species gains electrons (undergoes reduction). This transfer of electrons is driven by a difference in the electronegativity of the atoms involved.
The oxidized species is known as the reducing agent because it donates electrons, while the reduced species is called the oxidizing agent because it accepts electrons. It’s important to note that redox reactions always involve both oxidation and reduction, hence the name.
Importance of Redox Reactions
redox reactions play a crucial role in various chemical and biological processes. They are involved in energy production, corrosion, synthesis of chemicals, and even the functioning of our own bodies. For instance, the process of oxidative phosphorylation, which occurs in our cells’ mitochondria, relies on redox reactions to produce ATP, the universal energy currency of cells.
Common Examples of Redox Reactions
Let’s take a look at some common examples of redox reactions:
Combustion: When a substance reacts with oxygen to produce heat and light, it is a redox reaction. For example, the burning of wood or the combustion of gasoline in a car engine.
Rusting: The process of rusting involves the oxidation of iron in the presence of oxygen and water. The iron loses electrons, forming iron(III) oxide (rust).
Photosynthesis: During photosynthesis, plants convert carbon dioxide and water into glucose and oxygen, with the help of sunlight. This process involves the reduction of carbon dioxide and the oxidation of water.
Identifying Redox Reactions
To identify a redox reaction, we need to recognize the substances that are undergoing oxidation and reduction. Here are a few key steps to help us identify redox reactions quickly:
Recognizing oxidation and reduction: Look for changes in oxidation states or the loss/gain of electrons. If an element’s oxidation state increases, it is being oxidized, while a decrease in oxidation state indicates reduction.
Determining the oxidation Number: The oxidation number is a concept used to determine the distribution of electrons in a compound or ion. It helps us identify the change in oxidation states during a redox reaction.
Identifying redox reactions Quickly: One effective method to identify redox reactions is by looking for the presence of certain elements or compounds known to undergo redox reactions. For example, hydrogen peroxide (H2O2) is a common oxidizing agent, while substances like sodium borohydride (NaBH4) are reducing agents.
Calculating Redox Reactions
Once we have identified a redox reaction, we can proceed with calculating it. Here’s how:
Finding the Half reactions: Split the redox reaction into two half-reactions, one representing oxidation and the other representing reduction. This helps in balancing the equation later on.
Balancing the redox Reaction: Balance the number of atoms on each side of the equation by adjusting coefficients. It’s essential to balance both mass and charge when dealing with redox reactions.
Calculating the Overall Redox Reaction: Combine the balanced half-reactions, ensuring that the number of electrons gained in reduction matches the number of electrons lost in oxidation.
Advanced Concepts in Redox Reactions
To deepen our understanding of redox reactions, let’s explore some advanced concepts:
Determining Spontaneity of redox Reactions: The spontaneity of a redox reaction can be determined using the concept of redox potential. If the redox potential is positive, the reaction is spontaneous, indicating a higher likelihood of occurring.
Finding the Coefficient of redox Reactions: The coefficients in a balanced redox reaction represent the relative number of moles of each species involved. These coefficients are crucial for stoichiometric calculations.
Understanding the Role of Electrons in redox reactions: Electrons are the carriers of charge in redox reactions. They travel from the reducing agent to the oxidizing agent, facilitating the transfer of energy.
Practical Applications of Redox Reactions
Redox reactions have practical applications in various domains. Let’s explore a few examples:
redox reactions in Everyday Life: The process of respiration in our bodies relies on redox reactions to convert glucose into energy. Additionally, the batteries we use daily, such as alkaline batteries and lithium-ion batteries, operate based on redox reactions.
Industrial Applications of Redox reactions: Redox reactions are crucial in industrial processes like metal extraction, electroplating, and wastewater treatment. They help remove harmful pollutants and convert them into less toxic substances.
redox reactions in Biological Systems: In the human body, redox reactions are involved in various biological processes, including metabolism, detoxification, and immune responses. However, excessive redox reactions can lead to oxidative stress, which can damage cells and contribute to diseases.
Chemical reactions play a crucial role in various natural and biochemical processes. These reactions involve the transformation of reactants into products, accompanied by energy changes. In this section, we will explore the concepts of energy absorption, non-spontaneous reactions, biochemical reactions, and the role of energy in these processes.
Photosynthesis is a vital process that occurs in plants, algae, and some bacteria. It involves the conversion of light energy into chemical energy, specifically in the form of ATP synthesis. We will delve into the details of photosynthesis, the energy input required, and the thermodynamics governing this process.
Metabolic processes encompass a range of chemical reactions that occur within living organisms. These processes involve the storage and utilization of energy for various cellular functions. We will discuss endothermic reactions, the role of Gibbs free energy, and how anabolic reactions require energy input.
Cellular respiration is the process by which cells convert organic molecules into usable energy, primarily in the form of ATP. We will explore the overall process of cellular respiration, the storage of energy in ATP, and the crucial role of enzyme catalysis in this energy-releasing process.
Activation energy is the energy required to initiate a chemical reaction. Bioenergetics focuses on the study of energy transfer and transformation in living organisms. We will examine the concept of activation energy, its significance in reactions, and how it relates to the broader field of bioenergetics.
Throughout this content, we will provide examples and explanations to illustrate the concepts of chemical reactions, energy absorption, endergonic and exergonic processes, and the role of energy in various biochemical reactions. By understanding these fundamental principles, we can gain insights into the intricate mechanisms that govern energy flow in living systems.
Endergonic reactions are chemical reactions that require an input of energy in order to proceed. Unlike exergonic reactions, which release energy, endergonic reactions absorb energy from their surroundings. These reactions are typically non-spontaneous and require an external source of energy to occur. One common example of an endergonic reaction is photosynthesis, where plants convert sunlight into chemical energy to produce glucose. Another example is the synthesis of ATP (adenosine triphosphate), the energy currency of cells, which requires the input of energy to form. Endergonic reactions play a crucial role in various biological processes, allowing organisms to store and utilize energy efficiently.
Key Takeaways
Reaction Example
Energy Requirement
Photosynthesis
Sunlight
ATP synthesis
Cellular energy
Protein synthesis
Amino acids
DNA replication
Nucleotides
Active transport
ATP
Muscle contraction
ATP
Endothermic reactions
Heat
Definition of an Endergonic Reaction
An endergonic reaction is a type of chemical reaction that requires an input of energy in order to proceed. Unlike exergonic reactions, which release energy, endergonic reactions absorb energy from their surroundings. These reactions are also known as non-spontaneous reactions because they do not occur naturally without an external energy input.
Endergonic reactions are essential for various biochemical processes in living organisms. For example, photosynthesis, the process by which plants convert sunlight into energy, is an endergonic reaction. During photosynthesis, energy from the sun is absorbed and used to synthesize glucose and other organic molecules. Another example is ATP synthesis, where energy is inputted to produce adenosine triphosphate (ATP), the primary energy currency of cells.
In terms of thermodynamics, endergonic reactions have a positive change in Gibbs free energy (∆G). This indicates that the reaction requires an input of energy to proceed. The energy input can come from various sources, such as light, heat, or chemical reactions. Endergonic reactions are often coupled with exergonic reactions, where the energy released from the exergonic reaction is used to drive the endergonic reaction.
Endergonic reactions play a crucial role in metabolic processes, including anabolic reactions that build complex molecules and cellular respiration that breaks down molecules to release energy. These reactions are vital for energy storage and utilization within cells.
To better understand the concept of endergonic reactions, let’s consider an example. Imagine a reaction where a molecule needs to be converted into its ion form. This conversion requires an input of energy to break the bonds and separate the charges. Without the energy input, the reaction would not occur spontaneously. However, by providing the necessary energy, the reaction can proceed, resulting in the formation of the ion.
Characteristics of Endergonic Reactions
Endergonic reactions are a type of chemical reactions that require an input of energy to proceed. These reactions are non-spontaneous, meaning they do not occur naturally without the addition of energy. Endergonic reactions play a crucial role in various biochemical processes, such as photosynthesis and ATP synthesis.
In an endergonic reaction, the energy input is greater than the energy release. This positive energy input is necessary to overcome the activation energy barrier and drive the reaction forward. The Gibbs free energy change (∆G) for endergonic reactions is positive, indicating that energy is absorbed during the process.
To better understand the characteristics of endergonic reactions, let’s take a closer look at some key aspects:
Energy Requirement
Endergonic reactions require an input of energy to proceed. This energy can come from various sources, such as light, heat, or the breakdown of other molecules. The energy input is necessary to provide the activation energy needed to initiate the reaction.
Reaction Coupling
In many biological systems, endergonic reactions are coupled with exergonic reactions to drive the overall process. This coupling allows the energy released from exergonic reactions to be used as an input for endergonic reactions. For example, in cellular respiration, the energy released from the breakdown of glucose in exergonic reactions is used to drive the endergonic synthesis of ATP.
Anabolic Reactions
Endergonic reactions are often involved in anabolic processes, which are responsible for building complex molecules from simpler ones. These reactions require an input of energy to form bonds and create new chemical structures. Anabolic reactions are essential for processes like protein synthesis and the formation of complex carbohydrates.
Energy Storage
Endergonic reactions also play a crucial role in energy storage. For example, during photosynthesis, plants use endergonic reactions to convert light energy into chemical energy in the form of glucose. This stored energy can be later released and utilized by the organism when needed.
Enzyme Catalysis
Enzymes play a vital role in facilitating endergonic reactions by lowering the activation energy required for the reaction to occur. Enzymes act as catalysts, increasing the rate of the reaction without being consumed in the process. They provide an alternative pathway for the reaction, making it easier for the energy input to drive the reaction forward.
Difference Between Endergonic and Exergonic Reactions
Endergonic and exergonic reactions are two types of chemical reactions that differ in terms of energy changes. Let’s explore the differences between these two reactions.
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Endergonic reactions are chemical reactions that require an input of energy to proceed. In these reactions, the products have a higher energy level than the reactants. This means that energy is absorbed or taken in during the reaction. Endergonic reactions are non-spontaneous and do not occur naturally without an external source of energy.
On the other hand, exergonic reactions are chemical reactions that release energy. In these reactions, the products have a lower energy level than the reactants. This means that energy is released or given off during the reaction. Exergonic reactions are spontaneous and occur naturally without the need for an external source of energy.
To better understand the difference between endergonic and exergonic reactions, let’s compare them in terms of energy input, energy release, and examples:
Energy Input:
Endergonic reactions require an input of energy to proceed.
Exergonic reactions do not require an input of energy to proceed.
Energy Release:
Endergonic reactions release a small amount of energy.
Exergonic reactions release a significant amount of energy.
Examples:
Endergonic reactions are commonly found in biochemical processes such as photosynthesis and ATP synthesis. These metabolic processes require an input of energy to build complex molecules and store energy.
Exergonic reactions are involved in processes like cellular respiration, where energy is released from the breakdown of complex molecules to produce ATP.
In terms of thermodynamics, endergonic reactions have a positive Gibbs free energy change (∆G > 0), indicating that they are not spontaneous. Exergonic reactions, on the other hand, have a negative Gibbs free energy change (∆G < 0), indicating that they are spontaneous.
It’s important to note that endergonic and exergonic reactions can be coupled together in living organisms. This means that the energy released from an exergonic reaction can be used to drive an endergonic reaction, allowing for energy transfer and utilization in various biological processes.
Factors Influencing Endergonic Reactions
Endergonic reactions are chemical reactions that require an input of energy to proceed. Unlike exergonic reactions that release energy, endergonic reactions are non-spontaneous and need an energy input to occur. These reactions play a crucial role in various biochemical processes such as photosynthesis, ATP synthesis, and other metabolic processes.
Several factors influence endergonic reactions, and understanding these factors is essential for comprehending the principles of thermodynamics and bioenergetics. Let’s explore some of the key factors that affect endergonic reactions:
Energy Input
Endergonic reactions require an input of energy to overcome the activation energy barrier and proceed. This energy input can come in various forms, such as heat, light, or the transfer of high-energy molecules like ATP. The amount of energy required for an endergonic reaction is typically positive, meaning that more energy is needed than is released during the reaction.
Reaction Coupling
In some cases, endergonic reactions can be driven forward by coupling them with exergonic reactions. By linking an exergonic reaction (which releases energy) with an endergonic reaction, the overall process becomes energetically favorable. This coupling allows the energy released from the exergonic reaction to be used as an input for the endergonic reaction, making it possible for the endergonic reaction to occur.
Enzyme Catalysis
Enzymes play a crucial role in facilitating endergonic reactions by lowering the activation energy required for the reaction to proceed. Enzymes are biological catalysts that speed up chemical reactions without being consumed in the process. By reducing the energy barrier, enzymes enable endergonic reactions to occur more readily, making them essential for various metabolic processes.
Chemical Equilibrium
Endergonic reactions can be influenced by the principle of chemical equilibrium. In a reversible endergonic reaction, the forward reaction requires an input of energy, while the reverse reaction releases energy. The position of the equilibrium can be shifted by altering the concentration of reactants or products, which can impact the occurrence and rate of endergonic reactions.
Potential Energy Differences
Endergonic reactions involve a change in potential energy between reactants and products. The difference in potential energy determines the amount of energy required for the reaction to proceed. Higher potential energy in the products compared to the reactants indicates an endergonic reaction, while lower potential energy signifies an exergonic reaction.
Understanding the factors influencing endergonic reactions is crucial for comprehending the energy requirements and dynamics of various biochemical processes. By studying these factors, scientists can gain insights into how energy is stored, released, and utilized in living organisms, contributing to our understanding of fundamental biological processes such as cellular respiration and energy storage.
Importance of Endergonic Reactions in Metabolism
Endergonic reactions play a crucial role in the complex web of metabolic processes that occur within living organisms. These reactions are characterized by the absorption of energy, making them non-spontaneous and requiring an input of energy to proceed. Understanding the importance of endergonic reactions is essential for comprehending the intricate mechanisms that drive biochemical reactions in cells.
In metabolism, endergonic reactions are responsible for energy storage and utilization. One notable example is the process of ATP synthesis, where energy input is required to combine adenosine diphosphate (ADP) with an inorganic phosphate (Pi) to form adenosine triphosphate (ATP). ATP serves as a universal energy currency in cells, providing the necessary energy for various cellular activities.
To better grasp the significance of endergonic reactions, let’s explore some key concepts related to thermodynamics and bioenergetics. In a chemical reaction, the change in Gibbs free energy (ΔG) determines its spontaneity. Endergonic reactions have a positive ΔG, indicating that they require an input of energy to occur. This energy input is often provided by exergonic reactions, which release energy.
One way endergonic reactions are facilitated is through a process called reaction coupling. By coupling an endergonic reaction with an exergonic reaction, the overall energy change can be negative, allowing the endergonic reaction to proceed. This coupling is crucial for anabolic reactions, where complex molecules are synthesized from simpler ones. For instance, during photosynthesis, the endergonic process of converting carbon dioxide and water into glucose is coupled with the exergonic process of capturing sunlight energy.
Another important aspect of endergonic reactions is the role of enzymes. Enzymes act as catalysts, lowering the activation energy required for a reaction to occur. This reduction in activation energy enables endergonic reactions to proceed at a faster rate, facilitating the metabolic processes within cells.
Reversible Nature of Endergonic Reactions
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Endergonic reactions are a fascinating aspect of chemical reactions that involve the absorption of energy. Unlike exergonic reactions, which release energy, endergonic reactions require an input of energy to proceed. These reactions play a crucial role in various biochemical processes, such as photosynthesis and ATP synthesis, where energy input is necessary for the formation of complex molecules and the storage of energy.
In terms of thermodynamics, endergonic reactions have a positive change in Gibbs free energy (∆G), indicating that they are non-spontaneous under standard conditions. However, this does not mean that these reactions cannot occur. In fact, many endergonic reactions take place in living organisms as part of essential metabolic processes.
To better understand the reversible nature of endergonic reactions, let’s consider an example. Imagine a chemical reaction that requires an input of energy to proceed. Initially, the reaction may seem unfavorable due to the positive ∆G value. However, by coupling this endergonic reaction with an exergonic reaction, where energy is released, the overall process becomes favorable.
This concept of reaction coupling is crucial in anabolic reactions, where complex molecules are synthesized from simpler ones. For instance, in cellular respiration, the breakdown of glucose releases energy that is then used to drive the endergonic synthesis of ATP. This energy storage molecule is essential for various cellular processes.
In terms of bioenergetics, endergonic reactions can be visualized as reactions that require an input of potential energy to overcome the activation energy barrier. Once this energy is provided, the reaction proceeds, and the products are formed. However, it is important to note that the reverse reaction, where the products revert back to the reactants, is also possible.
The reversible nature of endergonic reactions is closely related to the concept of chemical equilibrium. In a reversible reaction, both the forward and reverse reactions occur simultaneously, but the net change in the concentrations of reactants and products reaches a dynamic equilibrium. This equilibrium is influenced by factors such as temperature, pressure, and the concentrations of reactants and products.
Supply of Energy for Endergonic Reactions
Endergonic reactions are chemical reactions that require an input of energy to proceed. Unlike exergonic reactions, which release energy, endergonic reactions have a positive change in free energy. These reactions are non-spontaneous and do not occur naturally without an energy input. In this article, we will explore how energy is supplied for endergonic reactions and the role it plays in various biological processes.
Energy Absorption and Endergonic Reactions
Endergonic reactions are commonly found in biochemical processes such as photosynthesis and ATP synthesis. These reactions involve the conversion of reactants into products, but they require an input of energy to overcome the energy barrier and proceed. The energy input for endergonic reactions is usually obtained from exergonic reactions, which release energy. This process is known as reaction coupling, where the energy released from an exergonic reaction is used to drive an endergonic reaction.
ATP: The Energy Currency of Cells
One of the primary sources of energy for endergonic reactions in cells is adenosine triphosphate (ATP). ATP is a molecule that stores and transports energy within cells. It consists of a nucleotide base (adenine), a sugar (ribose), and three phosphate groups. The high-energy phosphate bonds in ATP can be broken through hydrolysis, releasing energy that can be used to drive endergonic reactions.
During cellular respiration, energy is extracted from nutrients and used to synthesize ATP. The ATP molecules then serve as a source of energy for various cellular processes, including endergonic reactions. When ATP is hydrolyzed, it releases a phosphate group, becoming adenosine diphosphate (ADP) and inorganic phosphate (Pi). This release of energy allows endergonic reactions to occur.
Enzyme Catalysis and Energy Input
Enzymes play a crucial role in facilitating endergonic reactions by reducing the activation energy required for the reaction to proceed. Enzymes are biological catalysts that speed up chemical reactions by lowering the energy barrier. They achieve this by binding to reactant molecules and bringing them closer together, allowing the reaction to occur more easily.
In endergonic reactions, enzymes provide the necessary energy input by stabilizing the transition state of the reaction. By reducing the energy required for the reaction to proceed, enzymes enable endergonic reactions to occur at a faster rate. This energy input is essential for driving various metabolic processes and maintaining the overall energy balance within cells.
Energy Input and Chemical Equilibrium
In endergonic reactions, the energy input is required to shift the reaction towards the formation of products. This energy input helps overcome the energy barrier and allows the reaction to proceed. Without the necessary energy input, the reaction would remain at a standstill or reach a state of chemical equilibrium, where the forward and reverse reactions occur at equal rates.
By providing the required energy input, endergonic reactions can proceed and reach a state where the concentration of products is higher than that of reactants. This shift towards product formation is crucial for anabolic reactions, where complex molecules are synthesized from simpler ones. These reactions play a vital role in processes such as growth, repair, and the storage of energy in the form of complex molecules.
Examples of Endergonic Reactions with Explanation
Endergonic reactions are chemical reactions that require an input of energy to proceed. These reactions are non-spontaneous and have a positive change in free energy. In this article, we will explore several examples of endergonic reactions and their significance in various biochemical and metabolic processes.
Photosynthesis: 6CO2 + 6H2O → C6H12O6 + 6O2
Photosynthesis is a vital endergonic process that occurs in plants, algae, and some bacteria. It is responsible for converting carbon dioxide (CO2) and water (H2O) into glucose (C6H12O6) and oxygen (O2) using energy from sunlight. This reaction is crucial for the production of food and oxygen in the ecosystem. The energy input required for photosynthesis is provided by ATP synthesis, which is driven by the absorption of light energy.
Protein Synthesis
Protein synthesis is an essential endergonic process that occurs in all living organisms. It involves the formation of proteins from amino acids through a series of biochemical reactions. The process requires energy input in the form of ATP to link the amino acids together and form peptide bonds. Protein synthesis plays a crucial role in cell growth, repair, and the functioning of enzymes and other cellular components.
Dissolving Potassium Chloride in Water: KCl (s) → K+ (aq) + Cl– (aq)
The dissolution of potassium chloride (KCl) in water is an example of an endergonic reaction. In this process, solid KCl dissociates into potassium ions (K+) and chloride ions (Cl–) in the aqueous solution. The energy required for this reaction to occur is provided by the breaking of ionic bonds in the solid KCl. This endergonic reaction is commonly observed in various chemical and biological systems.
Na+/K+ Pump
The Na+/K+ pump is an important endergonic process that maintains the electrochemical gradient across the cell membrane in animal cells. It actively transports sodium ions (Na+) out of the cell and potassium ions (K+) into the cell against their concentration gradients. This process requires the hydrolysis of ATP to provide the energy needed for ion transport. The Na+/K+ pump is crucial for various cellular functions, including nerve impulse transmission and muscle contraction.
Melting of Ice into Liquid Water
The melting of ice into liquid water is an endergonic process that occurs when heat is applied to solid ice. The energy input in the form of heat breaks the hydrogen bonds between water molecules, allowing them to move more freely and transition from a solid to a liquid state. This endergonic reaction is important for the water cycle, as it enables the transformation of ice into liquid water, which is essential for various biological and environmental processes.
Fatty Acid Synthesis
Fatty acid synthesis is an endergonic process that occurs in cells to produce fatty acids, which are essential components of lipids. This anabolic reaction involves the step-by-step addition of acetyl-CoA molecules, with the input of energy in the form of ATP and NADPH. Fatty acid synthesis plays a crucial role in energy storage, insulation, and the formation of cell membranes.
Chemosynthesis
Chemosynthesis is an endergonic process that occurs in certain bacteria and archaea, allowing them to produce organic compounds without the use of sunlight. Instead, these organisms utilize energy from chemical reactions, such as the oxidation of inorganic compounds like hydrogen sulfide or ammonia. Chemosynthesis is important in deep-sea ecosystems and other environments where sunlight is not available.
DNA/RNA Synthesis
The synthesis of DNA and RNA is an endergonic process that occurs during DNA replication and transcription, respectively. These processes involve the formation of new DNA or RNA strands using existing nucleotides as building blocks. The energy input required for DNA/RNA synthesis is provided by the hydrolysis of ATP, which provides the necessary energy for the polymerization of nucleotides. DNA/RNA synthesis is essential for genetic information transfer and protein synthesis in all living organisms.
Electrolysis of Water: 2H2O → 2H2 + O2
Electrolysis of water is a chemical reaction that involves the decomposition of water molecules into hydrogen gas (H2) and oxygen gas (O2). This process is represented by the equation 2H2O → 2H2 + O2. It is an example of an endothermic reaction, meaning that it requires an input of energy to occur.
During electrolysis, an electric current is passed through a water solution, causing the water molecules to break apart into their constituent elements. The positive electrode, or anode, attracts negatively charged hydroxide ions (OH-) and undergoes oxidation, releasing oxygen gas. The negative electrode, or cathode, attracts positively charged hydrogen ions (H+) and undergoes reduction, producing hydrogen gas.
The electrolysis of water is a non-spontaneous reaction, meaning that it does not occur naturally and requires an external energy source. This energy input is necessary to overcome the activation energy barrier and drive the reaction forward. The process of electrolysis plays a crucial role in various applications, including the production of hydrogen gas for fuel cells and the generation of oxygen gas for industrial purposes.
The formation of nitrogen monoxide (NO) is another important chemical reaction. It involves the combination of nitrogen gas (N2) and oxygen gas (O2) to produce two molecules of nitrogen monoxide. This reaction is represented by the equation N2 (g) + O2 (g) → 2NO.
The formation of nitrogen monoxide is an example of an exothermic reaction, meaning that it releases energy in the form of heat. It occurs naturally in various processes, including combustion, lightning, and certain biochemical reactions in living organisms.
In biological systems, nitrogen monoxide plays a crucial role in regulating various metabolic processes. It is involved in the synthesis of ATP (adenosine triphosphate), the primary energy currency of cells. Nitrogen monoxide is also a signaling molecule that helps regulate blood pressure, immune responses, and neurotransmission.
The formation of nitrogen monoxide is a spontaneous reaction, meaning that it occurs without the need for an external energy input. However, it is important to note that the reaction is reversible and can reach a state of chemical equilibrium under certain conditions.
Overall, both the electrolysis of water and the formation of nitrogen monoxide are significant chemical reactions that play essential roles in various natural and industrial processes. They exemplify the principles of thermodynamics, energy transfer, and the interconnectedness of biochemical reactions in the world around us.
Frequently Asked Questions (FAQ)
What is the difference between an endergonic and an exergonic reaction?
Chemical reactions can be classified as either endergonic or exergonic based on the energy changes that occur during the reaction. An endergonic reaction is a non-spontaneous reaction that requires an input of energy to proceed. On the other hand, an exergonic reaction is a spontaneous reaction that releases energy. The main difference between the two is the direction of energy flow – endergonic reactions absorb energy, while exergonic reactions release energy.
What is the effect of temperature on an endergonic reaction?
Temperature plays a crucial role in the rate of an endergonic reaction. Generally, an increase in temperature leads to an increase in the rate of reaction. This is because higher temperatures provide more energy to the reactant molecules, allowing them to overcome the activation energy barrier and proceed with the reaction. Conversely, lower temperatures can slow down the reaction rate as the molecules have less kinetic energy to initiate the reaction.
Does endergonic reaction take place slowly?
The speed at which an endergonic reaction occurs can vary depending on several factors, including the reactants involved, the presence of catalysts, and the reaction conditions. While endergonic reactions generally require an input of energy to proceed, the rate of the reaction can be influenced by factors such as temperature, concentration, and the presence of enzymes. In some cases, endergonic reactions can occur relatively quickly, especially when facilitated by enzymes or favorable reaction conditions.
How are endergonic reactions characterized?
Endergonic reactions are characterized by a positive change in free energy (∆G). This means that the reaction requires an input of energy to proceed. The free energy change (∆G) is a measure of the potential energy difference between the reactants and the products. In an endergonic reaction, the products have a higher free energy than the reactants, indicating the need for an energy input to drive the reaction forward.
What are some examples of endergonic reactions?
Endergonic reactions are commonly found in biochemical processes such as photosynthesis and ATP synthesis. In photosynthesis, plants convert light energy into chemical energy by absorbing energy from the surroundings. ATP synthesis, which occurs during cellular respiration, also involves endergonic reactions that require energy input to produce ATP molecules. These examples highlight the importance of endergonic reactions in energy storage and metabolic processes.
How do factors impact endergonic reactions?
Several factors can impact the rate and feasibility of endergonic reactions. Temperature, concentration of reactants, presence of catalysts, and pH are some of the factors that can influence the reaction. Higher temperatures generally increase the reaction rate, while higher reactant concentrations can drive the reaction forward. Catalysts can lower the activation energy required for the reaction, making it more favorable. pH levels can also affect the reaction rate by altering the ionization state of reactants and products.
What is activation energy?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It represents the energy barrier that reactant molecules must overcome to reach the transition state and form products. In endergonic reactions, the activation energy is typically higher compared to exergonic reactions due to the need for an energy input. Catalysts can lower the activation energy, making it easier for the reaction to proceed.
How do endergonic reactions happen?
Endergonic reactions occur when the energy input provided to the reactants is sufficient to overcome the activation energy barrier. This energy input can come from various sources, such as heat, light, or the energy released by other exergonic reactions. In some cases, endergonic reactions can be coupled with exergonic reactions, where the energy released from the exergonic reaction is used to drive the endergonic reaction forward. This coupling of reactions allows the overall process to be energetically favorable.
What is a reversible reaction?
A reversible reaction is a chemical reaction that can proceed in both the forward and reverse directions. In other words, the products of the reaction can react with each other to form the original reactants. This means that the reaction can go back and forth between the reactants and products, depending on the conditions.
Reversible reactions are an important concept in chemistry and play a crucial role in many natural and biochemical processes. They are governed by the principles of thermodynamics, which describe the energy changes that occur during chemical reactions.
How does photosynthesis relate to endergonic reactions?
Photosynthesis is an example of an endergonic reaction, which is a type of non-spontaneous reaction that requires an input of energy. In this case, the energy input comes from sunlight. Photosynthesis is a vital metabolic process that occurs in plants, algae, and some bacteria, and it is responsible for converting light energy into chemical energy in the form of glucose.
During photosynthesis, plants use energy from sunlight to convert carbon dioxide and water into glucose and oxygen. This process involves several steps and is driven by the absorption of energy. The primary energy carrier in photosynthesis is adenosine triphosphate (ATP), which is synthesized through a series of reactions known as the light-dependent reactions.
The light-dependent reactions of photosynthesis occur in the thylakoid membranes of chloroplasts. These reactions involve the absorption of light energy by chlorophyll molecules, which triggers a series of electron transfer reactions. The energy from these reactions is used to generate ATP, which is then used in the subsequent steps of photosynthesis.
In the light-independent reactions, also known as the Calvin cycle, ATP and another energy carrier called NADPH are used to convert carbon dioxide into glucose. This process requires an input of energy, making it an endergonic reaction. The energy input is necessary to drive the synthesis of glucose, which serves as a source of energy and a building block for other molecules in the plant.
Overall, photosynthesis is an example of how endergonic reactions play a crucial role in the bioenergetics of living organisms. By harnessing energy from sunlight, plants are able to convert carbon dioxide and water into glucose, storing energy for later use. This process is essential for the survival of plants and provides the foundation for most ecosystems on Earth.
References
Chemical reactions are fundamental processes that occur in various biological and non-biological systems. These reactions involve the transformation of reactants into products, accompanied by the exchange or transfer of energy. In this section, we will explore the concept of energy in chemical reactions and its role in driving or inhibiting the spontaneity of a reaction.
Energy absorption and release are key aspects of chemical reactions. Some reactions require an input of energy to proceed, while others release energy. Reactions that require an input of energy are known as endergonic reactions, whereas reactions that release energy are called exergonic reactions. The energy input required for endergonic reactions is often provided by ATP (adenosine triphosphate), the primary energy currency in cells.
In the context of thermodynamics, the Gibbs free energy (ΔG) is a measure of the energy available to do work in a system. For a reaction to occur spontaneously, the ΔG must be negative, indicating a release of free energy. However, non-spontaneous reactions can still proceed if they are coupled with exergonic reactions that release enough energy to drive the overall process.
Biochemical reactions, such as photosynthesis and cellular respiration, are examples of complex metabolic processes that involve energy transformations. Photosynthesis is an endergonic process that converts light energy into chemical energy, stored in the form of glucose. This process requires an input of energy in the form of ATP and occurs in the chloroplasts of plants. On the other hand, cellular respiration is an exergonic process that releases energy by breaking down glucose to produce ATP. This process occurs in the mitochondria of cells.
Enzyme catalysis plays a crucial role in facilitating biochemical reactions by lowering the activation energy required for the reaction to proceed. Enzymes act as catalysts by providing an alternative pathway for the reaction, reducing the energy barrier and increasing the rate of reaction. This allows metabolic processes to occur efficiently within living organisms.
Frequently Asked Questions
What is the definition of an Endergonic Reaction?
An endergonic reaction is a type of chemical reaction where energy is absorbed from the surroundings. This is a non-spontaneous reaction, meaning it does not occur on its own without the input of energy.
How does an Endergonic Reaction function?
Endergonic reactions function by absorbing energy from their surroundings. This energy is often supplied in the form of heat or light. In biochemical reactions, such as photosynthesis or ATP synthesis, the energy is often supplied by other chemical reactions.
Can you provide an example of an Endergonic Reaction?
Photosynthesis is a prime example of an endergonic reaction. In photosynthesis, plants absorb light energy from the sun and convert it into chemical energy in the form of glucose.
What is the difference between endergonic and exergonic reactions?
Endergonic reactions absorb energy from their surroundings, while exergonic reactions release energy. This fundamental difference is related to the Gibbs free energy of the reactions. Endergonic reactions have a positive Gibbs free energy, indicating that they are non-spontaneous and require an input of energy. On the other hand, exergonic reactions have a negative Gibbs free energy, indicating that they are spontaneous and release energy.
How does temperature influence endergonic reactions?
Temperature can significantly influence the rate of endergonic reactions. Higher temperatures typically increase the rate of reaction by providing more kinetic energy to the reactant molecules. However, if the temperature is too high, it can denature enzymes that catalyze the reaction, slowing down or even stopping the reaction.
What is the importance of endergonic reactions in metabolism?
Endergonic reactions are crucial in metabolism as they allow the storage of energy in the form of chemical bonds. This stored energy can then be used by the body for various functions, such as muscle contraction, nerve impulse propagation, and the synthesis of biomolecules.
Are endergonic reactions reversible?
Yes, endergonic reactions are reversible. The direction of the reaction depends on the relative amounts of reactants and products, which is described by the principle of chemical equilibrium.
How does photosynthesis relate to endergonic reactions?
Photosynthesis is an example of an endergonic reaction. It involves the absorption of light energy by chlorophyll in plant cells, which is then used to convert carbon dioxide and water into glucose and oxygen. This process requires an input of energy, making it endergonic.
What is the impact of activation energy on endergonic reactions?
The activation energy is the minimum amount of energy required to initiate a chemical reaction. For endergonic reactions, the activation energy is typically high because these reactions require an input of energy. Enzymes can lower the activation energy, making it easier for the reaction to occur.
Can you provide an example of an endothermic reaction related to photosynthesis?
Photosynthesis is an example of an endothermic reaction. It is endothermic because it absorbs light energy from the sun, which is then used to convert carbon dioxide and water into glucose and oxygen.
