Question

The following data were obtained for a given reaction at $300$ $K$:

Reaction	Energy of activation $\left(kJ/mol\right)$
1. Uncatalysed	$76$
2. Catalysed	$57$

Calculate by what factor the rate of catalysed reaction is increased?

Answer 1

We have $K={Ae}^{-E_A/RT}$

Factors by which rate of catalyst reaction has increased will by

$\frac{K_1}{K_2}=\frac{{Ae}^{-E_{A1}/RT}}{{Ae}^{-E_{A2}/RT}}=e^{\frac{E_{A1}-E_{A2}}{RT}}=e^{\frac{(76-57)\times {10}^3}{8.314\times 300}}$

$=2033.82$