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In a reversible reaction, the catalyst
- a)increases activation energy of forward reaction
- b)decreases activation energy of forward reaction
- c)increases activation energy of backward reaction
- d)decreases activation energy of both forward and backward reactions
Correct answer is option 'D'. Can you explain this answer?
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In a reversible reaction, the catalysta)increases activation energy of...
Reversible Reactions and Catalysts
Reversible reactions are chemical reactions that can occur in both directions, converting reactants to products and vice versa. Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. Catalysts can be used in reversible reactions to speed up both the forward and backward reactions.
Effect of Catalysts on Activation Energy
Activation energy is the energy required to initiate a chemical reaction. Catalysts can decrease the activation energy required for a reaction to occur, making it easier for the reactants to form products. In the case of a reversible reaction, a catalyst can decrease the activation energy of both the forward and backward reactions, making it easier for the products to revert back to reactants.
The Effect of Catalysts on Equilibrium
In a reversible reaction, the equilibrium between reactants and products is established when the rate of the forward reaction is equal to the rate of the backward reaction. Catalysts do not affect the position of equilibrium, but they can speed up the rate at which equilibrium is reached. This means that the same amount of reactants and products will be present at equilibrium, but the time it takes to reach equilibrium will be shorter with the presence of a catalyst.
Conclusion
In summary, a catalyst in a reversible reaction can decrease the activation energy of both the forward and backward reactions, making it easier for the reactants to form products and for the products to revert back to reactants. While catalysts do not affect the position of equilibrium, they can speed up the rate at which equilibrium is reached.
Reversible reactions are chemical reactions that can occur in both directions, converting reactants to products and vice versa. Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. Catalysts can be used in reversible reactions to speed up both the forward and backward reactions.
Effect of Catalysts on Activation Energy
Activation energy is the energy required to initiate a chemical reaction. Catalysts can decrease the activation energy required for a reaction to occur, making it easier for the reactants to form products. In the case of a reversible reaction, a catalyst can decrease the activation energy of both the forward and backward reactions, making it easier for the products to revert back to reactants.
The Effect of Catalysts on Equilibrium
In a reversible reaction, the equilibrium between reactants and products is established when the rate of the forward reaction is equal to the rate of the backward reaction. Catalysts do not affect the position of equilibrium, but they can speed up the rate at which equilibrium is reached. This means that the same amount of reactants and products will be present at equilibrium, but the time it takes to reach equilibrium will be shorter with the presence of a catalyst.
Conclusion
In summary, a catalyst in a reversible reaction can decrease the activation energy of both the forward and backward reactions, making it easier for the reactants to form products and for the products to revert back to reactants. While catalysts do not affect the position of equilibrium, they can speed up the rate at which equilibrium is reached.
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In a reversible reaction, the catalysta)increases activation energy of...
In a reversible reaction, the catalyst decreases the activation energy of both, forward and backward reaction.
Catalyst provides an alternate pathway of lower activation energy for the reaction.
Catalyst provides an alternate pathway of lower activation energy for the reaction.
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In a reversible reaction, the catalysta)increases activation energy of forward reactionb)decreases activation energy of forward reactionc)increases activation energy of backward reactiond)decreases activation energy of both forward and backward reactionsCorrect answer is option 'D'. Can you explain this answer?
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In a reversible reaction, the catalysta)increases activation energy of forward reactionb)decreases activation energy of forward reactionc)increases activation energy of backward reactiond)decreases activation energy of both forward and backward reactionsCorrect answer is option 'D'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about In a reversible reaction, the catalysta)increases activation energy of forward reactionb)decreases activation energy of forward reactionc)increases activation energy of backward reactiond)decreases activation energy of both forward and backward reactionsCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In a reversible reaction, the catalysta)increases activation energy of forward reactionb)decreases activation energy of forward reactionc)increases activation energy of backward reactiond)decreases activation energy of both forward and backward reactionsCorrect answer is option 'D'. Can you explain this answer?.
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