Question

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which statement best describes the relationship between activation energy and rate of reaction? options:

1. increasing the activation energy can increase the rate of a reaction.
2. reducing the activation energy can increase the rate of a reaction.
3. reducing the activation energy can decrease the rate of a reaction.
4. increasing the reaction energy does not alter the rate of reaction.

Explanation:

To determine the correct statement, we recall the concept of activation energy in chemical kinetics. Activation energy (\(E_a\)) is the minimum energy required for a reaction to occur. A catalyst works by reducing the activation energy. When activation energy is reduced, more reactant molecules have enough energy to overcome the energy barrier, leading to an increased rate of reaction.

• "Increasing the activation energy can increase the rate of a reaction" is incorrect because higher activation energy means fewer molecules can react, so the rate decreases.
• "Reducing the activation energy can decrease the rate of a reaction" is incorrect; reducing \(E_a\) should increase the rate.
• "Increasing the reaction energy does not alter the rate of reaction" is incorrect as reaction energy (related to activation energy) does affect the rate.
• "Reducing the activation energy can increase the rate of a reaction" is correct because lowering the energy barrier allows more successful collisions, thus increasing the reaction rate.

Answer:

Reducing the activation energy can increase the rate of a reaction.