Two reactions $R_1$ and $R_2$
have identical pre-exponential factors. Activation energy
of $R_1$ exceeds that of $R_2$
by $10 kJ mol^{−1}$.
. If $k_1$ and $k_2$ are rate constants for reactions
$R_1$ and $R_2$ respectively at $300\; K$, then $ln(k2/k1)$ is equal to : $(R=8.314 \;J \;mol^{−1} K^{−1}
)$
