Q.
For the reaction of $H_2$ with $I_2$, the rate constant is $2.5 \times 10^{-4} dm^3 \; mol^{-1} s^{-1} $ at $327^{\circ}C$ and $1.0 \; dm^3 \; mol^{-1} \; s^{-1}$ at $527^{\circ} C$. The activation energy for the reaction, in $kJ \; mol^{-1}$ is:
$(R=8.314\,J \; K^{-1} mol^{-1})$
Solution: