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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...
Explanation:
Reversible Reaction:
In a reversible reaction, the reactants can form products, and the products can also react to form the original reactants. This means that the reaction can proceed in both the forward and backward directions.
Catalyst in a Reversible Reaction:
A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction. In a reversible reaction, a catalyst can facilitate both the forward and backward reactions by providing an alternative pathway with lower activation energy.
Effect of Catalyst on Activation Energy:
- Decreases Activation Energy of Forward Reaction: A catalyst lowers the activation energy required for the forward reaction to occur, allowing the reactants to form products more easily and quickly.
- Decreases Activation Energy of Backward Reaction: Similarly, the catalyst also lowers the activation energy required for the backward reaction to occur, enabling the products to revert back to the original reactants more efficiently.
Overall Impact of Catalyst:
- Decreases Activation Energy of Both Forward and Backward Reactions: By reducing the activation energy for both the forward and backward reactions, the catalyst speeds up the attainment of equilibrium in a reversible reaction. This leads to an increase in the rate of the reaction in both directions without changing the position of equilibrium.
Therefore, in a reversible reaction, the catalyst plays a crucial role in lowering the activation energy for both the forward and backward reactions, ultimately facilitating the reaction in both directions.
Reversible Reaction:
In a reversible reaction, the reactants can form products, and the products can also react to form the original reactants. This means that the reaction can proceed in both the forward and backward directions.
Catalyst in a Reversible Reaction:
A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction. In a reversible reaction, a catalyst can facilitate both the forward and backward reactions by providing an alternative pathway with lower activation energy.
Effect of Catalyst on Activation Energy:
- Decreases Activation Energy of Forward Reaction: A catalyst lowers the activation energy required for the forward reaction to occur, allowing the reactants to form products more easily and quickly.
- Decreases Activation Energy of Backward Reaction: Similarly, the catalyst also lowers the activation energy required for the backward reaction to occur, enabling the products to revert back to the original reactants more efficiently.
Overall Impact of Catalyst:
- Decreases Activation Energy of Both Forward and Backward Reactions: By reducing the activation energy for both the forward and backward reactions, the catalyst speeds up the attainment of equilibrium in a reversible reaction. This leads to an increase in the rate of the reaction in both directions without changing the position of equilibrium.
Therefore, in a reversible reaction, the catalyst plays a crucial role in lowering the activation energy for both the forward and backward reactions, ultimately facilitating the reaction in both directions.
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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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