Chemical equilibrium is indeed a dynamic equilibrium, meaning that both the forward and reverse reactions continue to occur even after the equilibrium state has been reached. This is because the rates of the forward and reverse reactions become equal, resulting in no net change in the concentrations of reactants and products over time.
Understanding Dynamic Equilibrium
The Concept of Dynamic Equilibrium
In a chemical reaction, the concept of dynamic equilibrium is crucial to understanding the behavior of the system. Dynamic equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time.
This can be represented by the following general equation:
A + B ⇌ C + D
At equilibrium, the concentrations of A, B, C, and D do not change, but the reactions are still occurring in both directions. This can be visualized as a game of tag, where the “it” person (reactants) and “not it” people (products) are constantly changing, but the total number of “it” and “not it” people remains constant.
The Equilibrium Constant (Keq)
The equilibrium constant (Keq) is a measure of the concentrations of products and reactants at equilibrium and is a constant for a given reaction at a constant temperature. The value of Keq does not depend on the initial concentrations used to reach the point of equilibrium.
The equilibrium constant is defined as:
Keq = [C]^c [D]^d / [A]^a [B]^b
Where:
– [C], [D], [A], and [B] are the equilibrium concentrations of the respective species
– a, b, c, and d are the stoichiometric coefficients of the reaction
Example: Hydrogen and Iodine Reaction
Consider the following reaction:
H2(g) + I2(g) ⇌ 2HI(g)
If we start the reaction with equal initial concentrations of H2 and I2, the reaction will go forward, with the concentrations of hydrogen and iodine decreasing and the concentration of hydrogen iodide increasing until it achieves equilibrium. If we reverse the reaction, the concentration of hydrogen iodide falls while the concentrations of hydrogen and iodine grow until equilibrium is reached.
Properties of an Equilibrium System
The following are the criteria and properties of an equilibrium system:
Closed System: The system must be closed, which means that no substances may enter or exit it.
Continuous Reactions: Equilibrium is a living, breathing thing. Even if we cannot see the reactions, both forward and reverse reactions are occurring.
Equal Reaction Rates: The rates of the forward and backward reactions must be equal.
Constant Concentrations: The number of reactants and products does not have to be the same. However, once equilibrium is reached, the amounts of reactants and products remain constant.
Factors Affecting Equilibrium
The equilibrium state of a system can be affected by various factors, such as:
Temperature: Changes in temperature can shift the equilibrium position, as described by the Le Chatelier’s principle.
Pressure: Changes in pressure can also shift the equilibrium position, particularly for reactions involving gases.
Concentration: Adding or removing reactants or products can shift the equilibrium position, as described by the Le Chatelier’s principle.
Numerical Examples
Example 1: Consider the reaction: 2NO(g) + O2(g) ⇌ 2NO2(g)
At equilibrium, the concentrations are: [NO] = 0.20 M, [O2] = 0.10 M, and [NO2] = 0.40 M.
Calculate the equilibrium constant (Keq) for this reaction.
In summary, chemical equilibrium is a dynamic equilibrium in which both the forward and reverse reactions continue to occur, but the rates of the reactions become equal, resulting in no net change in the concentrations of reactants and products over time. The equilibrium constant (Keq) is a measure of the concentrations of products and reactants at equilibrium and is a constant for a given reaction at a constant temperature. Understanding the properties and factors affecting equilibrium is crucial in the study of chemical reactions and their applications.
In the present article, we intend to discuss about the important chemical equilibrium examples you should know. We can always witness a state corresponding to a system in which it is found that the reactant concentration and the product concentration both evidently remain unchanged and also further more changes across properties cannot be seen to occur in correspondence to the system.
Ionization of acids and bases
Buffer solution
Methanol production
Ethanol production
Ammonia production
Solubility equilibria
Equilibrium in chemical processes
Ionization of acids and bases
Here, we can say that there is a splitting up of molecules that are generally neutral giving rise to the charged ions when they come in contact with the solution is itself the ionization. In this case, there occurs a point at which we can see a rate of both forward as well as backward reactions to be same.
Thus, is nothing but the chemical equilibrium. i.e., the expenditure of reactants in the reaction is compromised by the reverse reaction producing the same without any loss. It is one of the chemical equilibrium examples.
At such equilibrium point, there will be no variation in the concentration of the reactants as well as the products in accordance with time. In the aqueous medium there will be a production of hydrogen ions when dissociation of the acids takes place in that medium.
For the functioning of cells to be normal we need to maintain the pH of the respective substance. For this purpose, we require a solution generally referred as a buffer. Even in several chemical as well as biochemical processes also we may find a prime utility of the buffer solution. This is because of the mandatory need to control the pH.
The ideal pH of blood so that there is a normal functioning in the human body is found to be 7.35. By the use of buffer solution, the reactant concentration and the product concentration both evidently remain unchanged and also further more changes across properties cannot be seen to occur in correspondence to the system. It is one of the chemical equilibrium examples.
The conditions that are experimentally found to be favourable for the production are referred as the compromise conditions. The forward reaction in turn the production of methanol is usually favoured by a temperature that is comparatively lower which is around 500K as the forward reaction that is responsible for generating a lesser moles of gas is recognized to be an exothermic reaction.
Along with lower temperature, a higher pressure is also found to be in favour of the forward reaction. A copper catalyst may be of great use in order to increase the rection rate. It is one of the chemical equilibrium examples.
Ethanol production
The conditions that are experimentally found to be favourable for the production are referred as the compromise conditions. The forward reaction in turn the production of ethanol is usually favoured by a temperature that is comparatively lower approximately 570K as the forward reaction that is responsible for generating a lesser moles of gas is recognized to be an exothermic reaction.
Along with lower temperature, a higher pressure is also found to be in favour of the forward reaction. A phosphoric acid catalyst may be of great use in order to increase the rection rate. It is one of the examples of chemical equilibrium examples.
Ammonia production
The conditions that are experimentally found to be favourable for the production are referred as the compromise conditions. The forward reaction in turn the production of ammonia is usually favoured by a temperature that is comparatively lower i.e., around 670K as the forward reaction that is responsible for generating a lesser moles of gas is recognized to be an exothermic reaction.
Along with lower temperature, a higher pressure is also found to be in favour of the forward reaction. A iron catalyst may be of great use in order to increase the rection rate. It is one of the chemical equilibrium examples.
In this case, the considered solid molecules intend to produce individual molecules that are found to be aqueous by undergoing the process of dissolving. Below given reaction is an example for the same,
H2O C12H22O11(S) —————> C12H22O11(aq)
Whereas, there is a production of positive as well as the negative ions separately by the occurrence of dissociation of ionic solids. i.e.,
NaCl (s) ————————-> Na + (aq) + Cl – (aq )
The salt solutions are experimentally recognized to be a good conductors corresponding to the electricity as thus formed ions are responsible for carrying the electric current. It is one of the examples of chemical equilibrium examples.
We can always witness a state corresponding to a chemical reaction in which it is found that the reactant concentration and the product concentration both evidently remain unchanged and also further more changes across properties cannot be seen to occur in correspondence to the system.
As we all know, in chemical reactions we find the interconversion of products and reactants through forward and backward reactions respectively.
There occurs a point at which we can see a same rate of both forward and backward reactions. Thus, is nothing but the chemical equilibrium. i.e., the expenditure of amount of reactants in the reaction is compromised by the reverse reaction producing the same without any loss. It is one of the chemical equilibrium examples.
What are the different types that are associated with the chemical equilibrium?
In general, we can witness two types of chemical equilibrium. i.e.,
Homogeneous equilibrium
Heterogeneous equilibrium
Homogeneous equilibrium
In this type of chemical equilibrium, we may observe that the products of the reaction happen to be in the same phase as that of the reactants.
Heterogeneous equilibrium
In this type of chemical equilibrium, we may observe that the products of the reaction happen to be in a different phase when compared to that of the reactants.
Why chemical equilibrium is dynamic?
The chemical equilibrium can also be called as the dynamic equilibrium as, As we all know, in chemical reactions we find the interconversion of products and reactants through forward and backward reactions respectively.
There occurs a point at which we can see a same rate of both forward and backward reactions. Thus, is nothing but the chemical equilibrium. i.e., the expenditure of amount of reactants in the reaction is compromised by the reverse reaction producing the same without any loss.
Name the factors that influence the chemical equilibrium.
The factors that are proved to be influencing the chemical equilibrium are,
Change in concentration
Pressure change
Temperature change
Effect of catalyst
Addition of acids and bases
What do you mean by chemical equilibrium?
We can always witness a state corresponding to a system in which it is found that the reactant concentration and the product concentration both evidently remain unchanged and also further more changes across properties cannot be seen to occur in correspondence to the system.
As we all know, in chemical reactions we find the interconversion of products and reactants through forward and backward reactions respectively.
There occurs a point at which we can see the same rate of both forward and backward reactions. Thus, it is nothing but the chemical equilibrium. i.e., the expenditure of the number of reactants in the reaction is compromised by the reverse reaction producing the same without any loss.
Conclusion
As we all know, in chemical reactions we find the interconversion of products and reactants through forward and backward reactions respectively. There occurs a point at which we can see a same rate of both forward and backward reactions. Thus, is nothing but the chemical equilibrium.
The chemical change is the transformation of a molecule into an entirely different molecule.
There are principally three fundamental chemical change types: inorganic, organic, and biochemical changes. The chemical reactions can also be further branched into – synthesis, decomposition, single displacement, and double displacement.
In this segment, we shall intend to learn about the different chemical change types.
Inorganic Changes
Inorganic type changes describe all reactions that do not involve carbon in them.
This type of reaction typically involves the process of neutralization that is an acid- base reaction, redox reactions that involve oxidation and reduction, Decomposition reactions and displacement reactions about which we will further try to understand in this article.
There are numerous applications of inorganic changes that mainly occur in laboratories and industries.
There are a vast number of applications and to name a few:
Ammonia – a rich source of fertilizer. It is also used in nylons, plastics, fibre, hydrazine (used as rocket and jet fuel), etc.
Titanium Dioxide – used as white powder based pigment in paints, coatings, plastics, paper, inks, fibre, foods, cosmetics, photocatalysts, etc.
Chlorine – used for pipes, clothes, furniture, fertilizer, insecticide, water treatment, sterilization, etc.
Organic Changes
The organic types of changes describe all reactions involving carbon in them.
This type of reactions typically involves the process of halogenations – reactions dealing with halogens, polymerization – monomers to polymers, condensation reaction – loss of water, methylation – adding a methyl group to a substrate, etc.
Applications of organic changes:
Like inorganic changes, organic changes also have a large number of applications. As we know that organic changes are the changes that involve carbon and its compounds; identifying its applications are easy.
Diamond – diamond is largely used in the fashion industry as jewellery, also used for cutting and drilling as it is extremely hard.
Amorphous Carbon – used to make paints, inks and batteries.
Graphite – used as lead in pencils.
Coal – used as fuel.
The examples mentioned above are all different allotropes of carbon.
Bio- chemical Changes
Changes that occur in living organisms such as humans, plants, animals, and other organisms are all categorized under bio- chemical change.
These types of reactions typically involve the process of photosynthesis – plants convert light energy into chemical energy, digestion of food, protein synthesis – the creation of protein in molecules, etc.
Usually, bio- chemical changes are naturally occurring and cannot be artificially synthesized. Though, with the rise of new technologies, there’s a lot of room for new inventions. But, that is still in process. For now, one can jolt up a reaction but not synthesize it.
Thus, the application of bio- chemical change and its examples are the same, such as the process of photosynthesis, the process of digestion of food, the process of protein synthesis, etc.
There are four basic classes of chemical reactions about which we will learn in this section of the article.
Chemical reactions are further fractionated as – synthesis, decomposition, single displacement, and double displacement.
General Equation for types of Chemical Reactions
1. Synthesis
In a chemical synthesis, two or more reactants combine together for the creation of a complex product. In other words, it can also be expressed as two molecules interacting with each other to form a single complex molecule. The chemical properties of this newly formed product will be different from both the reactants.
This reaction is also referred by the name – combination reaction. The common equation for the reaction is given as:
A+B→AB
One of the most common examples of this reaction is the formation of salt, which we use in our day- to- day lives.
Na++Cl–→Salt(NaCl)
Another easy yet most important example is the formation of water.
2H2+O2→2H2O
Applications of a synthesis reaction:
It is easy to identify the applications of such easy examples. Yet another example that we observe more often is the rusting of iron, in which iron combines with oxygen to form rust. Synthesis reaction has a wide range of applications, as innumerable products can be obtained by combining various chemical elements from the periodic table.
2.Decomposition
A reactant is broken down into two or more simpler products in the decomposition reaction. These reactions need energy in the guise of heat, light, or electricity to disrupt the bonds within the reactants.
The general equation for this reaction is given as:
AB→A+B
It can be stated that the decomposition reaction is the rearward reaction of the combination reaction. And thus, we can take the same example of water, but instead, this time, we separate hydrogen and oxygen from the water through the electrolysis process.
2H2O→2H2+O2
The electrolysis process is nothing but enhancing the reaction with the help of electricity.
Decomposition reaction would not necessarily yield two or more single products. Occasionally, the products formed might still be a compound, just like the reaction mentioned above. Such reactions are still considered to be decomposition reactions.
Decomposition reaction can be both endothermic (heat- absorbing) as well as exothermic (heat- releasing).
For instance, the decomposition of nitrogen oxide into nitrogen and oxygen is exothermic or heat- releasing, while the decomposition of ozone (O3) into dioxide (O2) and oxygen (O) is endothermic or heat- absorbing.
In a single displacement reaction, one reactant gets replaced by another reactant, which is why this reaction is well known as a substitution reaction.
The general equation for this reaction is given as:
AB+C→AC+B
From the above equation, we can see that reactant ‘C’ has replaced reactant ‘B’ and formed new products. In such a reaction, the same types of reactants are usually replaced. For example, metal replaces metal; non- metal replaces non- metal, etc.
Here, the more reactive element replaces the less reactive.
The mixture of zinc with hydrochloric acid yields zinc chloride and hydrogen.
Zn+2HCl→ZnCl2+H2
As zinc is a stronger element than hydrogen, it will replace hydrogen and bond with chlorine.
Substitution reactions are further identified into two types:
Nucleophilic substitution reaction
Electrophilic substitution reaction
Let us try to understand these reactions in brief.
Nucleophilic substitution reaction
Nucleophile means nucleus loving or electron- rich element. The replacement is the same as the simple replacement. Here, a stronger Nucleophile replaces a weaker Nucleophile.
Electrophilic substitution reaction
Electrophiles are electron loving. They look for available electron pairs for bonding. They seek nucleophiles as they want to give away their electrons.
Applications of single replacement reactions:
Used for making steel.
Also used in thermite welding
Metal extraction
Nucleophiles and Electrophiles are used in various industrial, pharmaceutical and agrochemical processes.
4.Double replacement
In double replacement, two reactants replace each other to form new products. It is also known as metathesis. In this reaction, cations (Positively charged ions) and anions (Negatively charged ions) replace each other, but not both together.
It generally occurs with reactants that are aqueous or dissolved in a liquid solution, which is usually water. One of the products without exception is in the form of a gas, or a precipitate, or molecule such as water.
The general equation for this reaction is given as:
AB+CD→AC+BD
Here we can assume that reactants ‘A’ and ‘D’ are cations, and reactants ‘B’ and ‘C’ are anions.
Chemical changes are processes in which one or more substances are transformed into different substances with new properties. These changes are often irreversible, meaning that once a chemical change occurs, it cannot be easily undone. However, there are some ways in which a chemical change can be reversed. One common method is through the use of a chemical reaction called a reversible reaction. In a reversible reaction, the products of the reaction can react with each other to reform the original reactants. This allows the chemical change to be reversed, at least to some extent. Another way to reverse a chemical change is through physical means, such as separating the substances or changing the conditions in which the reaction occurred. By understanding these methods, scientists can explore ways to reverse chemical changes and develop new technologies.
Key Takeaways
Method
Description
Reversible reaction
Involves the products of a chemical reaction reacting with each other to reform the original reactants.
Physical separation
Involves separating the substances involved in the chemical change.
Changing conditions
Involves altering the conditions in which the reaction occurred to reverse the chemical change.
Understanding Chemical Changes
Chemical changes, also known as chemical reactions, occur when substances undergo a transformation, resulting in the formation of new substances with different properties. In this article, we will explore the fascinating world of chemical changes and delve into the various factors that influence them.
Reactants to Products and Back to Reactants
Chemical reactions involve the conversion of reactants into products through a series of molecular rearrangements. However, it is important to note that these reactions are not always one-way processes. In some cases, it is possible to reverse the reaction and reform the original reactants. This reversibility is a fundamental characteristic of chemical changes.
The reformation of reactants from products is known as the reverse reaction process. It occurs when the conditions are favorable for the reactants to recombine and form the original substances. This reversal can be achieved through various methods, such as altering the temperature, pressure, or concentration of the reactants. By manipulating these factors, it is possible to shift the equilibrium of the reaction towards the formation of the reactants.
The Role of Energy in Chemical Changes
Energy plays a crucial role in chemical changes. During a chemical reaction, energy is either released or absorbed. Reactions that release energy in the form of heat are called exothermic reactions, while those that absorb energy from the surroundings are known as endothermic reactions.
The energy input in chemical changes determines the feasibility and spontaneity of the reaction. In some cases, additional energy is required to initiate the reaction, known as the activation energy. This energy input can be provided through various means, such as heat, light, or the presence of a catalyst.
The Impact of Concentration, Temperature, and Pressure
Concentration, temperature, and pressure are important factors that influence the rate and direction of chemical changes. By altering these variables, it is possible to manipulate the equilibrium of the reaction and favor the formation of products or reactants.
Increasing the concentration of the reactants generally leads to an increase in the rate of the reaction. This is because a higher concentration provides more reactant particles, increasing the chances of successful collisions and subsequent chemical reactions.
Temperature also plays a significant role in chemical changes. As the temperature increases, the kinetic energy of the particles also increases, leading to more frequent and energetic collisions. This results in a higher reaction rate and a shift towards the formation of products or reactants, depending on the specific reaction.
Pressure, on the other hand, primarily affects reactions involving gases. By increasing the pressure, the volume available for the gas particles decreases, leading to a higher concentration of particles. This increased concentration promotes more collisions and enhances the reaction rate.
In conclusion, understanding chemical changes is essential for comprehending the behavior of substances and their transformations. By exploring the reversibility of reactions, the role of energy, and the impact of concentration, temperature, and pressure, we gain valuable insights into the intricate world of chemistry. So, let’s dive deeper into the fascinating realm of chemical reactions and uncover the secrets behind their remarkable transformations.
The Concept of Reversible Chemical Changes
Chemical changes are a fundamental part of our everyday lives. From cooking food to burning fuel, these reactions occur all around us. But did you know that not all chemical changes are irreversible? In fact, some reactions can be reversed under certain conditions, leading to the reformation of the original reactants. This concept is known as reversible chemical changes.
Is Chemical Change Reversible?
The reversibility of a chemical change refers to the ability of a reaction to proceed in both the forward and reverse directions. In other words, it means that the products of a reaction can react with each other to form the original reactants. This process is often influenced by various factors, which we will explore in the next section.
Factors Determining the Reversibility of Chemical Changes
Several factors play a crucial role in determining whether a chemical change can be reversed. Let’s take a closer look at some of these factors:
Energy Input:Reversing chemical reactions usually involve the input of energy. Endothermic reactions, which absorb heat from the surroundings, are more likely to be reversible. On the other hand, exothermic reactions, which release heat, are often irreversible.
Catalysts: Catalysts are substances that can speed up a chemical reaction without being consumed in the process. In the context of reversing reactions, catalysts can play a significant role in increasing the rate of the reverse reaction, making it more feasible.
Entropy and Enthalpy: Entropy refers to the degree of disorder in a system, while enthalpy represents the total energy of a system. The interplay between these two factors can influence the reversibility of a chemical change. Generally, reactions with a higher entropy and lower enthalpy are more likely to be reversible.
Le Chatelier’s Principle: This principle states that when a system at equilibrium is subjected to a change in conditions, it will respond in a way that minimizes the effect of that change. By manipulating factors such as temperature, pressure, or concentration, it is possible to shift the equilibrium towards the reverse reaction.
Reaction Rates:The rate at which a chemical reaction occurs can also impact its reversibility. Reactions with faster rates are often more difficult to reverse, as the forward reaction is favored.
By considering these factors, scientists can better understand the conditions under which a chemical change can be reversed. This knowledge is crucial in fields such as industrial chemistry, where the ability to control and manipulate reactions is of utmost importance.
In summary, reversible chemical changes are a fascinating aspect of chemistry. They demonstrate that the transformation of substances can be a two-way process, with the ability to revert back to the original reactants. Understanding the factors that influence reversibility allows us to harness these reactions for various applications, from developing new materials to optimizing industrial processes.
Why Some Chemical Changes Cannot Be Reversed
Chemical changes are transformations that occur when substances undergo a chemical reaction, resulting in the formation of new substances with different properties. While many chemical changes can be reversed under certain conditions, there are instances where this is not possible. Let’s explore some reasons why certain chemical changes cannot be easily reversed.
Stability of Reaction Products
One reason why some chemical changes cannot be reversed is due to the stability of the reaction products. When a chemical reaction occurs, new substances are formed with different chemical properties than the reactants. In some cases, these products are highly stable and resistant to change. This stability makes it difficult for the reaction to be reversed and for the original reactants to reform.
Different Chemical Composition of Products
Another factor that contributes to the irreversibility of certain chemical changes is the different chemical composition of the products compared to the reactants. During a chemical reaction, atoms are rearranged and bonds are broken and formed. This rearrangement leads to the formation of new substances with distinct chemical compositions. Reversing the reaction would require breaking the newly formed bonds and reforming the original bonds, which may not be energetically favorable or feasible.
Energy Requirements for Reversing Chemical Changes
The energy requirements for reversing chemical changes also play a crucial role in their irreversibility. Chemical reactions can be classified as either endothermic or exothermic based on the energy changes involved. Endothermic reactions absorb energy from their surroundings, while exothermic reactions release energy. Reversing an endothermic reaction would require an input of energy to break the bonds in the products and reform the reactants. Similarly, reversing an exothermic reaction would require the removal of energy released during the forward reaction. These energy requirements make the reverse reaction process challenging and often impractical.
In addition to the factors mentioned above, several other factors influence the reversibility of chemical changes. Catalysts can facilitate the reverse reaction process by lowering the activation energy required. The principles of entropy and enthalpy also play a role, as chemical reactions tend to proceed in the direction that increases the overall entropy of the system. Le Chatelier’s principle, which states that a system will shift to counteract any changes imposed upon it, can also affect the reversibility of chemical reactions.
It is important to note that not all chemical changes are irreversible. Some reactions can be reversed under specific conditions, such as adjusting the reaction conditions, applying external energy, or using catalysts. Balancing chemical equations and understanding the reaction rates are essential in determining the feasibility of reversing a chemical change.
In conclusion, the irreversibility of certain chemical changes can be attributed to the stability of reaction products, the different chemical composition of products compared to reactants, and the energy requirements for reversing the changes. While some chemical changes can be reversed, others are inherently irreversible due to these factors. Understanding the reasons behind the irreversibility of chemical changes helps us appreciate the complexity and intricacies of chemical reactions.
How Some Chemical Changes Can Be Reversed
Chemical changes, also known as chemical reactions, occur when substances undergo a transformation and form new substances with different properties. While many chemical changes are irreversible, there are certain cases where these changes can be reversed. In this article, we will explore the concept of reversing chemical changes and discuss examples of reversible chemical reactions as well as the conditions required for their reversal.
Examples of Reversible Chemical Changes
Reversible chemical changes involve a process where the reactants can reform from the products. This means that the reaction can proceed in both the forward and reverse directions. Let’s take a look at some examples of reversible chemical changes:
Water Dissociation: When water molecules dissociate into hydrogen ions (H+) and hydroxide ions (OH-), it is a reversible process. The forward reaction involves the formation of these ions, while the reverse reaction involves the recombination of the ions to form water molecules again.
Ammonium Chloride Dissolution: When ammonium chloride (NH4Cl) dissolves in water, it undergoes a reversible chemical change. The forward reaction involves the dissolution of NH4Cl into NH4+ and Cl- ions, while the reverse reaction involves the precipitation of NH4Cl from the ions.
Hydrogen Iodide Decomposition: Hydrogen iodide (HI) can decompose into hydrogen (H2) and iodine (I2) gases. This reaction is reversible, as the forward reaction involves the decomposition of HI, while the reverse reaction involves the reformation of HI from H2 and I2.
Conditions Required for Reversing Chemical Changes
To reverse a chemical change, certain conditions need to be met. These conditions vary depending on the specific reaction and its properties. Here are some factors that influence the reversibility of chemical changes:
Energy Input: Reversing a chemical change often requires an input of energy. Endothermic reactions, which absorb heat from the surroundings, are more likely to be reversible. By providing the necessary energy, the reverse reaction can occur, leading to the reformation of the reactants.
Catalysts: Catalysts are substances that can speed up chemical reactions without being consumed in the process. In the context of reversing chemical changes, catalysts can facilitate the reverse reaction by lowering the activation energy required. This increases the likelihood of the reaction being reversible.
Entropy and Enthalpy: The concepts of entropy and enthalpy play a role in the reversibility of chemical changes. Entropy refers to the degree of disorder in a system, while enthalpy represents the heat content of a system. Reversible reactions often involve a balance between these two factors, allowing the reaction to proceed in both directions.
Le Chatelier’s Principle: Le Chatelier’s Principle states that when a system at equilibrium is subjected to a change in conditions, the system will adjust to counteract the change. By manipulating the conditions, such as temperature, pressure, or concentration, it is possible to shift the equilibrium towards the reverse reaction, effectively reversing the chemical change.
In conclusion, while many chemical changes are irreversible, there are instances where these changes can be reversed. By understanding the principles of chemical equilibrium, energy input, catalysts, and manipulating reaction conditions, it is possible to reverse certain chemical reactions. This ability to reverse chemical changes is not only fascinating but also crucial in various fields of science and industry.
Interesting Facts about Reversible Reactions
Reversible reactions are fascinating chemical processes that involve the transformation of reactants into products, followed by the reformation of reactants from the products. These reactions occur in both nature and industry, playing a crucial role in various chemical processes. Let’s explore some interesting facts about reversible reactions.
Unique Examples of Reversible Chemical Changes
Reversible chemical changes are quite common and can be observed in our daily lives. Here are a few unique examples:
Water Evaporation and Condensation: When water is heated, it evaporates and forms water vapor. However, when the vapor cools down, it condenses back into liquid water. This process is reversible and can occur repeatedly.
Melting and Freezing of Substances: The melting of a solid substance into a liquid and the subsequent freezing of the liquid back into a solid is another example of a reversible reaction. This can be observed when ice melts into water and then freezes again when the temperature drops.
Dissociation and Reformation of Acids: Acids can dissociate into ions when dissolved in water, forming a solution with a higher concentration of hydrogen ions. However, by adding a base, the reaction can be reversed, and the acid can be reformed.
The Role of Reversible Reactions in Nature and Industry
Reversible reactions play a crucial role in various natural and industrial processes. Here are some notable aspects:
Chemical Equilibrium: Reversible reactions reach a state of chemical equilibrium when the forward and reverse reactions occur at the same rate. This equilibrium allows for a dynamic balance between reactants and products, ensuring a stable system.
Energy Input in Chemical Changes: Reversible reactions often involve energy changes, such as endothermic and exothermic reactions. Endothermic reactions require an input of energy to proceed, while exothermic reactions release energy. These energy changes contribute to the reversibility of the reactions.
Catalysts in Reversing Reactions: Catalysts are substances that can speed up the rate of a chemical reaction without being consumed in the process. They play a significant role in reversing reactions by providing an alternative reaction pathway with lower activation energy.
Entropy and Enthalpy: Reversible reactions are influenced by both entropy (the measure of disorder in a system) and enthalpy (the heat content of a system). These factors determine the feasibility and direction of the reaction.
Le Chatelier’s Principle: Reversible reactions respond to changes in temperature, pressure, and concentration according to Le Chatelier’s Principle. When these factors are altered, the system adjusts to counteract the change and restore equilibrium.
Balancing Chemical Equations: Understanding reversible reactions is essential for balancing chemical equations accurately. Balancing ensures that the number of atoms on both sides of the equation remains equal, representing the reversibility of the reaction.
Chemical Reaction Conditions: Reversible reactions are highly dependent on reaction conditions such as temperature, pressure, and the presence of catalysts. These conditions can be manipulated to favor the forward or reverse reaction, allowing control over the process.
In conclusion, reversible reactions are intriguing phenomena that occur in various chemical processes. They demonstrate the dynamic nature of chemical changes and their ability to reverse under specific conditions. Understanding the principles behind reversible reactions is crucial for scientists and engineers in both research and industrial applications.
Conclusion
In conclusion, while chemical changes are typically irreversible, there are a few ways in which they can be reversed. One method is through the process of electrolysis, where an electric current is used to break down compounds into their original elements. Another way is through the use of catalysts, which can speed up the reaction in the opposite direction, effectively reversing the chemical change. Additionally, some chemical changes can be reversed by simply changing the conditions, such as temperature or pressure. However, it’s important to note that not all chemical changes can be reversed, and it largely depends on the specific reaction and compounds involved.
How can a chemical change be reversed?
A chemical change refers to the process in which one or more substances are transformed into different substances with distinct properties. To reverse a chemical change, it is necessary to understand the different types of chemical changes that can occur. By “Exploring Different Types of Chemical Changes”, we can identify reversible chemical reactions that can be reversed by applying specific conditions or altering the reaction conditions. By understanding the underlying principles of various chemical change types, scientists can develop strategies to reverse chemical changes and potentially recover the initial substances or restore their original properties.
Frequently Asked Questions
1. What is the usual cause of oxidation in a chemical reaction?
The usual cause of oxidation in a chemical reaction is the loss of electrons from an element or reactant. This process often involves the addition of oxygen or the removal of hydrogen.
2. Can a chemical change be easily reversed?
Chemical changes are usually permanent and cannot be easily reversed. This is because new products are formed which have a different chemical composition. However, some chemical changes can be reversed under certain conditions, such as changing temperature or pressure, or by using a catalyst.
3. Why can’t a chemical change be normally reversed?
A chemical change can’t be normally reversed because the reactants undergo a reaction to achieve stability. The reaction products become more stable than the reactants, so the reaction will not reverse under normal conditions.
4. How could some chemical changes be reversed? Give an example.
Some chemical changes can be reversed by applying energy or altering conditions. For example, the decomposition of water into hydrogen and oxygen gases is an endothermic reaction that can be reversed by recombining these gases under the right conditions.
5. What is the purpose of a catalyst in reversing reactions?
The purpose of a catalyst in reversing reactions is to lower the energy barrier for the reaction, allowing it to proceed at a faster rate or under milder conditions. Catalysts can be used to facilitate both forward and reverse reactions.
6. How can you reverse a chemical change?
Reversing a chemical change requires changing the conditions under which the reaction occurs. This might involve changing the temperature, pressure, or concentration of reactants, or introducing a catalyst. The specifics depend on the particular reaction.
7. How can a chemical reaction be reversed?
A chemical reaction can be reversed by applying the principles of Le Chatelier’s principle. This principle states that if a system at equilibrium is disturbed, the system will adjust itself to reduce the effect of the disturbance. This could involve changing conditions such as temperature, pressure, or concentration.
8. Is a chemical change reversible?
Not all chemical changes are reversible. Some are, under the right conditions, but many are not. Whether a chemical change is reversible depends on the specific reactants and products, as well as the conditions under which the reaction occurs.
9. What is the difference between a physical change and a chemical change?
A physical change involves changes in the physical properties of a substance, such as its shape, size, or state, without altering its chemical composition. A chemical change, on the other hand, involves a change in the substance’s chemical composition, resulting in the formation of new products.
10. How does entropy and enthalpy affect the reversibility of a chemical reaction?
Entropy and enthalpy both play a role in determining whether a chemical reaction is reversible. Reactions that result in an increase in entropy (disorder) and a decrease in enthalpy (energy) are more likely to be spontaneous and irreversible. However, if the reaction results in a decrease in entropy and an increase in enthalpy, it may be reversible under the right conditions.
Firstly the term carbohydrate was used to define chemical compounds having an empirical formula CH2O.
Carbohydrates have been classified based on their structure, not by their formulae. Carbohydrates are the aldehydes and ketones having multiple hydroxyl groups hence known as polyhydroxy. Glycogen, Starch and Cellulose are amongst the composites that belong to carbohydrate family.
What’s the structure of carbohydrates?
Carbohydrates, such as starch, cellulose, and sugars, are organic molecules found in biological tissues and foods.
Sugars have a similar oxygen-to-hydrogen proportion as water, which is 2:1. It normally breaks down in the body of the organism to give out energy. The formula for all the carbohydrates is Cn(H2O)n, it applies for simple sugars. Sugars are “optically active as well.
Carbohydrates are also known as saccharides, a Greek term that meaning “sugar,” because nearly all carbohydrates have a sweet flavor. The word carbohydrate or carbon hydrate comes from its basic constituent formula, which has carbon linked to hydrogen and oxygen in the same ratio as water.
Grain carbohydrate classification is based on chemical structures or digestibility when taken by humans as food or by cattle as feed. Sugars or disaccharides are simple carbohydrates that are sweet and soluble in water, and the names of most sugars end in -ose. As a result, we have terms like sucrose for regular table sugar, glucose for blood sugar, and maltose for malt sugar.
Classification of carbohydrates
Figure: Classification of Carbohydrates. Image Credit: Med Libretexts
Carbohydrates are differentiated into two classes:
on the basis of their chemical structure and polymerization
Simple Carbohydrates
One, two, or a few sugar molecules constitutes the simple carbohydrates. They’re abundant in milk, vegetables, fruits and grains. These carbohydrates are referred to be “empty calories” since they lack minerals, vitamins and fibre.
Monosaccharides are sugars comprised of just one sugar unit. The quantity of carbon atom in the sugar atom is utilized to additionally differentiate monosaccharides.
Monosaccharide carbohydrates are those that cannot be further hydrolyzed to produce simpler polyhydroxy aldehyde or ketone molecules. Aldose alludes to a monosaccharide that has an aldehydic group, while ketose alludes to a monosaccharide that contains a keto group.
(i)Trioses (C3H6O3): Contain three carbon atoms. Example: Glyceraldehyde
(ii)Tetroses (C4H6O4): Contain four carbon atoms. Example: Erythrose
(iii) Pentoses: Contains five carbon atoms. Example: Ribose
(iv) Hexoses: contain six carbon atoms. Example: Glucose
Figure: Classification of monosaccharides on the basis of number of carbon atoms in their structure. Image Credit: Lumen Learning
Disaccharides
A disaccharide is synthesized when two monosaccharide sugars join properly. Examples: Sucrose, Lactose, Maltose, etc.
• When disaccharides are hydrolyzed, they produce two molecules of monosaccharides that are either the same or distinct.
• An oxide linkage, created by the loss of a water molecule, connects the two monosaccharide units, and this linkage is known as glycosidic linkage.
• Sucrose hydrolyze into glucose and fructose.
• Maltose (malt sugar) and lactose (commonly known as milk sugar) also belong to the class of disaccharides.
• There are two -D-glucose in maltose and one D-glucose and one D-galactose in lactose that are joined by a glycosidic bond.
Figure: Some common disaccharides. Image Credit: Lumen Learning
Oligosaccharides
“Few” is the meaning of the word “oligo.” Oligosaccharides are carbohydrate molecules generated by the condensation of 2-9 monomers (short chains of monosaccharides).
Oligosaccharide examples are Raffinose and stachyose.
Figure: Raffinose is a common oligosaccharide. Image Credit: Wikimedia
Complex Carbohydrates (Polysaccharides)
Carbohydrate rich food varieties contain at least two sugar units and are thus alluded to as complex carbohydrates. In contrast with simple carbs, complex carbs are digested gradually.
Lentils, beans, peanuts, potatoes, peas, maize, whole-grain bread, cereals, and other legumes.
Polysaccharides are made up of lengthy monosaccharide units linked together by glycosidic linkage, and the majority of them, such as starch, serve as food storage. Plants use starch as their primary storage polysaccharide.
It is a glucose polymer comprised of two parts: Amylose and Amylopectin.
Cellulose is quite possibly the most widely found polysaccharide in plant cell wall.
It is comprised of D-glucose units connected together by a glycosidic linkage between C1 of one glucose unit and C4 of the following.
Amylose and amylopectin are the two parts of starch. Amylopectin is a chain with branched structure that beginnings with amylose and terminates with amylopectin.
Glycogen is found in animals and it is a similar to starch. however with more prominent branching pattern.
The structural element of the plant cell wall is cellulose, which is a carbohydrate polymer. It’s a tough and fibrous polysaccharide. In contrast to starch and glycogen, cellulose polymerizes to give a linear structure.
What does the chemical structure of a carbohydrate look like?
Sugars are comprised of carbon (C), hydrogen (H), and oxygen (O), with hydrogen being double in number as compared with carbon and oxygen.
Carbs are simple sugars or monosaccharides in their most basic structure. These monomers can be joined to make more complex carbs. A disaccharide is a compound made up of two simple sugars. Carbohydrates containing two to ten simple sugars are known as oligosaccharides, whereas those with more are known as polysaccharides.
Sugars, starches, cellulose, and an assortment of different biomolecules found in living organisms are instances of carbohydrates.
Chemical and biological properties differ across saccharides with similar functional groups but differing spatial arrangements. Stereochemistry is the investigation of how atoms are organized in three dimensions. Stereoisomers are structures in which the atoms are associated in a similar pattern however are organized in a different way.
Enantiomers are structures that are mirror images of one another however are not same, like left and right shoes. Example D-Glucose and L-Glucose. By flipping and rotating identical molecules, they can be made to correspond to one another.
By flipping and rotating enantiomers, notwithstanding, they can’t be made to compare to their identical representations. Because it provides a more accurate representation of the molecule’s binding angles, glucose is frequently depicted as a “chair form.” Glucose in the “boat” form is unstable.
Starch: Polymer of glucose joined together by alpha-1,4-glycosidic linkages.
Glycogen: Polymer of glucose joined together by alpha-1,4-glycosidic linkages.
Cellulose: Polymer of glucose joined together by Beta-1,4-glycosidic linkages.
Chitin: Polymer of N-Acetyl-Aminoglucose joined together by Beta-1,4-glycosidic linkages.
Starch is the stored food of plants while glycogen is the stored energy reserve/food found in animals. Cellulose is the component of plant cell wall while Chitin is the component of fungal cell wall and exoskeleton on insects.
Which atom is present in the structure of carbohydrates?
Sugars are comprised of carbon (C), hydrogen (H), and oxygen (O), with hydrogen being double in number as compared with carbon and oxygen
The formula in general for all carbohydrates is Cn(H2O)n. This equation just applies to simple sugars that contain a similar amount of carbon and water.
The Chemical change is irreversible as new bonds are made.
When a chemical change occurs, the molecules present in one type of reactants break their bonds and make bonds with another kind of reactants, or they break bonds and create an entirely different molecule.
Due to this reason solely it is simple to understand why chemical change is irreversible. Though some chemical changes are reversible, that is because they have formed simple bonds that can be transformed back to the original. Whereas in irreversible chemical change, numerous complex changes occur that change the bond formation entirely, and it is impossible to reverse.
In this article, we shall have a close look at why chemical change is irreversible.
List of Contents
Creation of New Bonds
When two or more molecules react with each other, they create different types of bonds between them. These bonds, once created, are complicated to transform to the original. Though new molecules can be made by altering them, but they cannot be brought back to their initial state.
The molecules that react with each other are known as ‘Reactants,’ and the resultant molecules are known as ‘Products.’ Thus, in other words, reactants can be transformed into products, but products cannot be converted back to reactants.
Such equations are symbolized with an arrow that points in one direction.
Say, for example, reactant ‘A’ and reactant ‘B’ are made to react with one another, and they yield product ‘C’ and product ‘D,’ then the equation for this scenario is written as:
A+B→C+D
General Equation for Irreversible Chemical Changes
Thus, the chemical properties of the material are altered entirely when such reactions occur. The change in chemical properties also changes the physical properties of a substance at times. Hence, such reactions are difficult to reverse, and in some cases, even impossible to reverse.
For instance, let’s take the example of cooking. Say a person is baking a cake. For making a cake, they will need flour, egg, butter, salt, sugar, milk, baking soda, water, and edible decorating ingredients.
First of all, all these ingredients will be mixed together. We can’t even begin to imagine the chemical processes taking place inside a material when nine ingredients are mixed all together. After the mixture, the cake is baked. Baking, frying, sautéing, etc., change the properties of a material to a whole another level.
Now, once the cake is baked, there’s no way we can transform the cake back to the nine initial ingredients that we used.
One of the most essential reasons why chemical change is irreversible is the energy difference. As we saw above that a chemical change occurs when bonds are broken or created.
Sometimes, there isn’t enough energy present in the system that can reverse a reaction, or there isn’t enough energy in the system that can break all the bonds in the products.
Here, energy does not necessarily mean heat. Nucleus, atoms, and molecules altogether have energy and energy levels of their own. Providing them external heat just won’t make the expected change sometimes.
Elimination of Reactant
When a chemical reaction is performed in an open system, more often than not, some amounts of reactants are lost to the environment. For example, elimination of oxygen (O2) or Carbon dioxide (CO2) as they are in gaseous form.
If the closed system is not appropriately maintained, the gaseous reactants or resultant products can also blow off in an open environment. A system in which there is no transfer of matter or energy, neither from inside nor from outside, is known as a closed system.
Though there are different closed systems in which the transfer of either of them is allowed, like, in thermodynamics, where transfer of energy is allowed, but the transfer of matter is not permitted in a closed system.
Consecutive Reactions
The formation of Carbon Tetrachloride from Methane involves many steps. Methane is chlorinated in the presence of light to obtain chloromethane, which is again chlorinated in the presence of light, giving dichloromethane. Further chlorination yields chloroform, chlorination of which will result in Carbon Tetrachloride.
The equation of the reaction is given as:
Chlorine is added to the products, and light works as a catalyst.
The initial reactants are the same, but the process is lengthy. Reversing this process is usually difficult or sometimes even impossible.
In this case, only chlorine is added at every step. There are also some reactions that involve more than two reactants at every stage, which makes the process even more complex.
Products are More Stable than Reactants
In some reactions, products are more stable than the reactants, and thus, transforming the products back to reactants is exceptionally burdensome. The products have double or triple bonds formed on occasions, which are not easy to break or even reverse.
Exothermic reactions are said to be irreversible. For example, combustion; when a log of wood is set to fire, it releases energy in the form of heat and light. This energy is emitted out of the system, and thus, it is an exothermic reaction. Hence, the products yielded will be more stable than the reactants, which is why we cannot bring back wood from ashes.
‘Is chemical change reversible?’ – This question has been asked numerous times and left people scratching their heads.
The Chemical change is reversible at times. Yes, you read it right! Well, a chemical change is usually an irreversible process, but the beauty of chemistry is that – it has exceptions, just like this one.
The reversible chemical reaction has the ability to progress in both ways, which simply means to move forward as well as backward. But this process occurs only till dynamic equilibrium is attained. Equilibrium, in this case, is achieved when two reactions, happening in opposite ways, occur at the same time and at the same rate.
What is a Reversible Process?
Reactions that do not reach to the absolute completion are reversible.
A reversible process or reaction is a reaction in which reactants are converted into products and products are converted into reactants simultaneously.
On occasions, the number of reactants getting converted back from products might vary from the original amount of reactants.
Give some advantages and disadvantages of a reversible chemical reaction.
Advantages
Disadvantages
Reversible chemical reactions or in general, every chemical reaction help us in understanding the properties of matter and in developing new technologies or new products.
Occasionally, the produced outcome may be harmful to the environment as well as to the other life forms on earth (like humans, animals, plants, marine life, etc.).
Increased reaction rates.
They cost more in terms of both, money and time.
Improved quality of the product.
Finite applications.
Less initial investment.
Requirement of complex operations when wanting to reverse the reaction.
Simple reactant to a product mixture.
Quite a time, complex product to reactants conversion.
Finer product quality.
Considerable experimental development is required.
Enhanced catalyst life.
Only a few reactions can be reversed compared to more number of irreversible reactions.
Ammonium chloride, a mixture of ammonia and hydrogen chloride, which is a white solid. When hydrogen chloride and ammonia are mixed at room temperature, i.e., 25°C, they form ammonium chloride.
It again breaks down into ammonia and hydrogen chloride when heated.
Whenever a reversible chemical reaction takes place, a part of the reaction heading in one direction will always be exothermic, and the reaction heading in another direction will always be endothermic.
Remember, the reaction from left to right doesn’t need to be exothermic, and the reaction from right to left doesn’t need to be endothermic. It can occur in whichever way possible.
What should be the equilibrium position for a reversible reaction?
The equilibrium of a reversible chemical reaction is affected by several factors.
One can change the equilibrium of a reversible chemical reaction through various other conditions like adjusting the temperature, changing the pressure, changing the concentration, etc.
Say, one part of nitrogen molecules and three parts of hydrogen molecules are mixed together to get two parts of ammonia molecules.
Now, when we say one part means 1 N2 molecule and not 1 N, as Nitrogen (N) alone cannot exist. A single nitrogen atom immediately makes a bond with another nitrogen molecule to fulfill its valance band.
Similarly, three parts of hydrogen mean 3 H2 molecules.
Thus, the reaction for the Haber process is given as follows:
Now the question arises that 1N2 + 3H2 should yield 4NH3 but instead, we have 2NH3.
Well, when looked closely, there are 2 N molecules on the left side as well as 2 N molecules on the right side.
Similarly, for hydrogen on the left side, we have 3H2 molecules, which give 3×2 = 6 hydrogen atoms as well as 3×2 = 6 hydrogen atoms on the right side.
When the numbers of atoms or molecules on both sides are equal, the reaction is said to be balanced, and hence, we can say that it is in equilibrium.
When there is an increase in pressure, the reaction moves in the direction where there are less number of molecules, and when the pressure is decreased, the reaction proceeds in the order where there are more number of molecules.
When there is an increase in concentration, the equilibrium position will move in the opposite direction from the direction of the reactant, of which the concentration is increased. For e.g., if the concentration of reactant ‘A’, which is on the right side, is increased, the equilibrium will move on the left side.
Similarly, when there is an increase in the temperature, the equilibrium will move towards the endothermic process. Thus, if the forward reaction is exothermic, the reverse reaction ought to be endothermic, and if the forward reaction is endothermic, the reverse reaction should essentially be exothermic.
For remembering this information more effectively, it is better to put it in a tabular form.
Change
Equilibrium
Pressure Increased
Moves to fewer molecules
Concentration Increased
Moves to the opposite direction from that reactant
Chemical Changes occur when a new bond between molecules is either formed or broken. This change results in new and different kinds of properties than the parent molecule.
When a chemical change occurs, there is rearrangement of atoms which changes the chemical composition of the substance as a whole, due to which this process is generally irreversible. When multiple compounds react with one another, two types of changes can be observed, one is the chemical change, and another is the physical change.
How chemical change occurs is a question asked frequently.
In physical change, no bonds are broken or formed. Thus, physical change can be observed when there is a change in state of the material, i.e., solid, liquid or gaseous form, physical deformation, etc.
Chemical change is when the internal composition of the matter changes, which results in change in color, change in odor, change in melting and boiling points, formation of precipitate, formation of bubbles, release of gases, change in composition etc. One of the significant points is, if the reaction is difficult to reverse or impossible to reverse.
Energy is always required to put forward a chemical reaction. Sometimes, the energy is absorbed by the molecules to carry forward the reaction and sometimes, energy is released.
Factors like temperature, presence of catalysts, concentration of the reactants, presence of moisture (for some reactions), state of reactants (solid, liquid, gas, and ions), etc., affect the reaction rate.
In this section, we will learn about how chemical change occurs, factors affecting chemical change, requirements for a chemical change to occur, types of chemical change, etc.
1. How Chemical Change Occurs?
When chemical change occurs, a substance is transformed into a different substance.
Chemical change occurs when the bond between two or more reactants is created, broken or simply rearranged.
Energy is required for both breaking and creating a bond. Sometimes, the energy needed to break the bond is higher than the energy required in making a bond. This binding or splitting changes numerous properties of the substance such as odor, color, state, melting point, boiling point, taste, etc.
For E.g.:- Rusting of iron is an example of chemical change as the iron reacts with oxygen and water and a different substance is formed, which is rust while boiling of water is not a chemical change as the water molecules only change their state (i.e., from liquid to gaseous) but not its form.
Chemical change is usually irreversible but in some cases, it is reversible too!
For E.g.:- Tearing off a paper is a physical act or change but it cannot be reversed. Even if we try to join the paper with different means, it won’t come back to its original form.
2. Why are chemical reactions important?
Chemical Change assists us in understanding the properties of matter.
Chemical changes help us understand the processes happening all around the world as well as in the universe.
Every action that occurs in the universe is a result of chemical change. Once the properties of matter are understood, one can also understand how to control a reaction. All this information helps in recognizing the ongoing processes and in developing or inventing new things.
The basic necessity for all life forms to survive in the biosphere is oxygen and food.
Photosynthesiswas chosen as the most crucial chemical change in 1988.
Though humans, animals or other organisms do not perform photosynthesis on their own, they highly depend on plants (who carry out photosynthesis) for food and oxygen.
4. What are some examples of chemical change observed in everyday life?
One of the best and the most straightforward examples of chemical change that we observe in our day-to-day life is cooking.
Various physical and chemical changes take place when food is cooked. Another easy example is combustion.
Nowadays, the electric gas stove has taken over, but a large part of the world still uses the conventional gas stove that utilizes fire. Fire is nothing but a type of chemical reaction.
Yet, sometimes it is, but most of the time, it is converted into energy.
According to the famous equation given by Einstein, which states that mass can be converted into energy and energy can be converted into mass. The equation is given as:
E = mc2
Where, E = Energy; m = mass; c = speed of light in vacuum
More often than not, the mass converted into energy is in a negligible amount in atomic reactions. In nuclear reactions, the energy absorbed or released is relatively high, and thus, the change in mass is significantly visible.
7. What are the different types of chemical changes?
The different types of chemical changes are:
Organic Chemical Changes
Inorganic Chemical Changes
Biochemical changes
The organic type of chemical change deals with the chemistry of carbon, and the inorganic type of change deals with the chemistry of all the other elements and their compounds other than carbon. In contrast biochemical change involves the chemistry of the living organisms controlled by proteins and enzymes.
