The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the reaction at 343 K than at 316 K? (R = 8.314 J/mol • K)

Answer 1

Arrhenius equation:

ln (k2/k1) = -Ea/R (1/T2 - 1/T1)

ln (k2/k1) = -42.2 kJ/mol / 0.008314 kJ/mol-K (1/343 - 1/316) ... note to change units of R

ln (k2/k1) = -5076 (0.002915 - 0.003165)

ln (k2/k1) = -5076 (-0.00025) = +1.269

k2/k1 = 3.56

This suggest that the rate would be 3.6 times faster at the higher temperature.