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(D) For a collision to be effective,the colliding molecules must possess energy equal to or greater than a specific value known as the threshold energ

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increase in the number of effective collisions

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(D) For a collision to be effective,the colliding molecules must possess energy equal to or greater than a specific value known as the threshold energy. At room temperature,most reactant molecules have energy less than this threshold value. When the temperature increases,the kinetic energy of the reactant molecules increases,leading to a higher fraction of molecules possessing energy equal to or greater than the threshold energy. Consequently,the number of effective collisions per unit time increases,which results in an increase in the rate of reaction.

The rate of reaction increases with a rise in temperature because of:

Similar Questions

Which graph shows zero activation energy?

Find True $(T)$ and False $(F)$ statements among the following:
$1.$ All collisions in a reaction result in the formation of products.
$2.$ All collisions in a reaction are effective.
$3.$ The number of collisions depends on the rate of reaction.

Which of the following graphs for $\ln k$ versus $\frac{1}{T}$ is correct?

An endothermic reaction with high activation energy for the forward reaction is given by the diagram:

The differential form of the Arrhenius equation is:

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