For an exothermic reaction $A \rightarrow B$,the activation energy of $A$ is $17 \, kJ/mol$. The heat of reaction is $40 \, kJ$. Calculate the activation energy for the reverse reaction $B \rightarrow A$.

Find the correct equation among the following.

In the plot of $\ln k$ versus $\frac{1}{T}$,what do the slope and intercept represent?

Write the Arrhenius equation to calculate the activation energy $(E_a)$ at two different temperatures.

Write the Arrhenius equation in the form $ln \, k = -\frac{E_a}{RT} + ln \, A$.

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 $E_a$.