The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N2O(g) → N2(g) + O(g). If the activation energy is 250 kJ/mol and the frequency factor is 8.0 × 1011 s-1,

Question

what is the rate constant for the first-order reaction at 1000 K?

Answer 1

Refer to the Arrhenius equation:

K = A*e^(-Ea/RT)

e^(-Ea/RT) = K/A

-Ea/RT = ln(K/A)

ln K = -Ea/RT + ln A = 250 / (0.008314)(1000) + ln 8x10^11

Solve for K