In chemical reaction, the rate of reaction increases with temperature, because:

the number of collisions between molecules increases

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of decrease in the activation energy

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of increase in the number of the molecules with the activation energy

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the kinetic energy of reactants increases

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Solution

The correct option is D the kinetic energy of reactants increases
On increasing the temperature, the kinetic energy of molecules increase and thus, the fraction of molecules having energy greater than the activation energy increases.
A chemical reaction takes place due to a number of effective collisions between molecules having energy greater than the activation energy.

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Similar questions

Q. Which of the following will result when the temperature is increased as the chemical reaction proceeds?
I. Increased molecular collision frequency
II. Increased numbers of molecules possess energy greater than the activation energy
III. Decreased randomness of the system

Which of the following statements are in accordance with the Arrhenius equation?
(a) Rate of a reaction increases with increase in temperature
(b) Rate of a reaction increases with a decrease in activation energy
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(d) Rate of reaction decreases with a decrease in activation energy

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(ii) decrease the activation energy
(iii) alters the reaction mechanism
(iv) increases the frequency of collisions of reacting species.
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(3) fractional of the molecules possessing the activation energy for the reaction increases

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