The thermal decomposition of dinitrogen pentoxide in the gas phase is often simplified as
overall reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
A proposed mechanism with the first step rate-limiting is given below.
Step 1 (slow): N₂O₅ → NO₂ + NO₃
Step 2 (fast): NO₃ + NO → 2 NO₂
Step 3 (fast): NO + O₂ → NO₂
Assume all steps are elementary and irreversible.
(a) Write the rate law predicted by this mechanism.
(b) State the overall reaction order implied by your rate law.
(c) Experimental studies report that doubling the initial concentration of N₂O₅ doubles the reaction rate while changing the concentrations of all other species has no measurable effect. Discuss whether the proposed mechanism is consistent with this observation.