The decomposition of ethyl bromide is a first-order reaction with an activation energy of 226 kJ/mol.?

Question

At 450oC the rate constant for the reaction is 8.80 x 10-3 /s; what is the rate constant at 973 K?

Answer 1

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

ln k1/k2 = (226,000 J / 8.314 J etc.) (1/937 - 1/723)

ln k1/k2 = (226,000 J / 8.314 J etc.) (0.001067 - 0.001381)

ln k1/k2 = (226,000 J / 8.314 J etc.) (- 0.0003138)

ln k1/k2 = - 8.529

e^x both sides

K1/k2 = 1.976e-4

k2 = k1 / 1.976e-4

k2 = 8.80 x 10-3 / 1.976e-4

your answer is: k2 = 44.5 / s