The minimum energy a molecule should possess in order to enter into a fruitful collision is known as

When the temperature changes from $293 \ K$ to $313 \ K$,the rate of a certain reaction becomes four times. Find the activation energy of the reaction in $kJ \ mol^{-1}$. $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

Which plot of $\ln k$ vs $\frac{1}{T}$ is consistent with the Arrhenius equation?

Assertion : If the activation energy of a reaction is zero,temperature will have no effect on the rate constant.
Reason : Lower the activation energy,faster is the reaction.

The following graph is obtained for a reaction $(A \rightarrow P)$. The activation energy ($E_{a}$ in $kJ \ mol^{-1}$) and heat of reaction ($|\Delta H|$ in $kJ \ mol^{-1}$) for this reaction are respectively ($x=$ reaction coordinate; $y=E$ in $kJ \ mol^{-1}$)

Activation energy $(E_a)$ and rate constants $(k_1)$ and $(k_2)$ of a chemical reaction at two different temperatures $(T_1)$ and $(T_2)$ are related by