Statement 1: If the activation energy of reaction is zero temperature will have no effect on the rate constant Statement 2: Lower the activation energy faster is the reaction

Question

Statement 1: If the activation energy of reaction is zero temperature will have no effect on the rate constant Statement 2: Lower the activation energy faster is the reaction (A) If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1. (B) If both Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1. (C) If Statement 1 is true but Statement 2 is false. (D) If Statement 1 is false but Statement 2 is true.

Tardigrade Admin · Accepted Answer

According to Arrhenius equation K=Ae-Ea/RT when Ea=0, K=A

Q. Statement 1: If the activation energy of reaction is zero temperature will have no effect on the rate constant
Statement 2: Lower the activation energy faster is the reaction

If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1.

If both Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1.

If Statement 1 is true but Statement 2 is false.

If Statement 1 is false but Statement 2 is true.

According to Arrhenius equation $K = A e^{- E_{a / RT}}$ when $E_{a} = 0, K = A$

Q. Statement 1: If the activation energy of reaction is zero temperature will have no effect on the rate constant Statement 2: Lower the activation energy faster is the reaction