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 250kJ/mol and the frequency factor is 8.0 x 10^11 /s, what is the rate constant for the first-order reaction at 1000K?

0.0698

Explanation:

k = Ae^-Ea/RT

A= frequency factor = 8.0 x 10^11 /s

Ea = activation energy= 250 * 10^3J/mol

R= 8.314 J/mol/K

T = 1000K

Substituting values;

k = 8.0 x 10^11 * e^-250 * 10^3/ 8.314 * 1000

k = 0.0698

i'm assuming that the correct answer is indeed the first one/ "a"..

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