For a reaction where the activation energies of the forward and reverse directions are equal in value,then:

If for two reactions $E_{a_1} > E_{a_2}$ and $\mu_1$ and $\mu_2$ are their respective temperature coefficients,then which of the following is correct?

The activation energy of a reaction is zero. The rate constant of this reaction

In a reaction,for every $10 ^\circ C$ rise in temperature,the rate is doubled. If the temperature is increased from $10 ^\circ C$ to $100 ^\circ C$,the rate of the reaction will become ......... times.

The time required for $10 \%$ completion of a first order reaction at $298 \,K$ is equal to that required for its $25 \%$ completion at $308 \,K$. If the value of $A$ is $4 \times 10^{10} \,s^{-1}$,calculate $k$ at $318 \,K$ and $E_a$.

The activation energy of a reaction is $0$. The rate constant of the reaction: