Sarnali Mukherjee

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 Fe₂O_3. n(H₂O).

Read more about oxidation reaction example

Respiration

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:

C₆H₁₂O₆ (Glucose) +6O₂ (Oxygen) = 6CO₂ (Carbon Dioxide) + 6H₂O (Water)

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.

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.

One specific example of the above mentioned oxidation definition is the oxidation of the ethanol.

Chemical equation of the reaction:

CH3CH2OH (Ethanol) → CH3CHO (ethanal)

Photosynthesis

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.

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.

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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.

Chemical reaction: The below image could be the best reference top identify the lengthy biochemical process of glycolysis.

This reaction is the oldest example of exergonic reaction. The reaction is quite reliable in following the principles of exergonic reaction.

Read more about 12+ Exothermic Reaction Examples: Detailed Explanations

Fatty Acid catabolism

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.

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