Statement I: With increase in temperature activation energy of the reaction decreases

Statement II: For every 10° rise in temperature, the rate of the reaction doubles for most of the reactions

Statement I is false but statement II is correct.

Statement I: With an increase in temperature, the activation energy of the reaction decreases.
This statement is false. With an increase in temperature, the average kinetic energy of the molecules increases, but the activation energy of the reaction remains the same. Activation energy is a characteristic property of a reaction and is not affected by changes in temperature.

Statement II: For every 10° rise in temperature, the rate of the reaction doubles for most reactions.
This statement is correct. The rate of many reactions approximately doubles for every 10-degree Celsius increase in temperature. This behavior is described by the Arrhenius equation, which shows that the rate constant (and thus the reaction rate) is exponentially dependent on temperature.

Therefore, the correct answer is: Statement I is false, but Statement II is correct.