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 x 1011 s-1, what is the rate constant for the first-order reaction at 1000 K?

Question

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 x 1011 s-1, what is the rate constant for the first-order reaction at 1000 K?

k = A * exp ( -Ea / RT )

k = rate constant (s-1)
A = frequency factor or preexponential factor (s-1)
Ea = activation energy (J / mol)
R = gas constant (J / K*mol)
T = Temp (K)

k=8.0x10^11s-1(250kj/mol/8.314472*1000K)

did i set this up right?

gaby · Answer

Never mind i know i didn't what goes in the exp?

DrBob222 · Answer

I use it in the form that follows: ln(k2/k1) = Ea/R(1/T1 - 1/T2) You must insert A appropriately.

Confused · Answer

i don't understand where k1 k2 t1 t2 come from... :(