The data below were obtained for the decomposition of N2O5 at 318 K.
t = 0 600 1200 2400 3600 4800 6000 7200
P(N2O5) 0.348 0.257 0.190 0.105 0.058 0.033 0.018 0.010 Atm
- What is the rate law for the reaction?
Give arguments for your answer.
- What is the rate constant at 318 K?
Show detail calculation.
- The proposed mechanism is
N2O5 -k1-> NO2 + NO3
NO2 + NO3 -k-1-> N2O5
These two steps reach fast equilibrium.
NO3 -k2-> NO + O2
NO + NO3 -k3-> 2 NO2
Apply the steady state approximation to both NO and NO3 to
derive the rate law. Comment on this in view of your answer
in the first part
- The rate constants as a function of temperature were determined
T/K 338 308 273
k 3.64e-4 3.11e-5 1.15e-6
Determine the activation energy for the reaction.