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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 Reaction and Catalyst
Reversible reactions are those reactions that can proceed in both forward and backward directions. A catalyst is a substance that increases the rate of a chemical reaction without undergoing any permanent change itself. Catalysts are known to affect the activation energy of a reaction.
Activation Energy
Activation energy is the minimum energy required for a chemical reaction to occur. It is the energy required to break the bonds of the reactants and form new bonds to produce the products.
Effect of Catalyst on Activation Energy
A catalyst lowers the activation energy of a reaction, which means that less energy is needed to start the reaction. This is because a catalyst provides an alternative pathway with a lower activation energy. This alternative pathway is known as the catalytic pathway.
Effect of Catalyst on Reversible Reaction
A catalyst affects both the forward and backward reactions in a reversible reaction. It lowers the activation energy of both the forward and backward reactions, making it easier for the reaction to proceed in both directions.
Conclusion
In conclusion, a catalyst decreases the activation energy of both the forward and backward reactions in a reversible reaction. This allows the reaction to proceed faster in both directions.
Reversible reactions are those reactions that can proceed in both forward and backward directions. A catalyst is a substance that increases the rate of a chemical reaction without undergoing any permanent change itself. Catalysts are known to affect the activation energy of a reaction.
Activation Energy
Activation energy is the minimum energy required for a chemical reaction to occur. It is the energy required to break the bonds of the reactants and form new bonds to produce the products.
Effect of Catalyst on Activation Energy
A catalyst lowers the activation energy of a reaction, which means that less energy is needed to start the reaction. This is because a catalyst provides an alternative pathway with a lower activation energy. This alternative pathway is known as the catalytic pathway.
Effect of Catalyst on Reversible Reaction
A catalyst affects both the forward and backward reactions in a reversible reaction. It lowers the activation energy of both the forward and backward reactions, making it easier for the reaction to proceed in both directions.
Conclusion
In conclusion, a catalyst decreases the activation energy of both the forward and backward reactions in a reversible reaction. This allows the reaction to proceed faster in both directions.
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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.Hence the correct option is D....
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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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