The velocity constant of a reaction at $290 \ K$ was found to be $3.2 \times 10^{-3}$. At $300 \ K$ it will be

The rate constants $k_1$ and $k_2$ for two different reactions are $10^{16} \cdot e^{-2000/T}$ and $10^{15} \cdot e^{-1000/T},$ respectively. The temperature at which $k_1 = k_2$ is

$A$ catalyst increases the rate of a chemical reaction by

Explain: How is the value of activation energy determined based on the Arrhenius equation?

The temperature-dependent equation for the rate constant is written as:

For a first-order reaction,the time taken to complete $10\%$ at $298\, K$ is equal to the time taken to complete $25\%$ at $308\, K$. The activation energy of the reaction is ................ $kJ/mol$.