posted by gaby .
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)
did i set this up right?