Statement I: If the activation energy of a reaction is zero, the temperature will have no effect on the rate constant

Statement II: Lower the activation energy, the faster is the reaction

Statement I and statement II are correct but statement II is not the correct explanation of statement I

The answer is 2.

Statement I is true. If the activation energy of a reaction is zero, then the temperature will have no effect on the rate constant. This is because the rate constant is a measure of the frequency of collisions between reactant molecules, and the activation energy is the minimum energy that the colliding molecules must have in order to react. If the activation energy is zero, then any collision between reactant molecules will result in a reaction.

Statement II is also true. In general, the lower the activation energy of a reaction, the faster the reaction will be. This is because the lower the activation energy, the less energy the reactant molecules need to have in order to react. Therefore, they will collide with each other more often and with more energy, resulting in a faster reaction.

However, statement II is not the correct explanation of statement I. The correct explanation of statement I is that the rate constant is independent of the activation energy if the activation energy is zero.