Consider the following reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) The initial concentration of N2O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N2O5 has been consumed.   a) Calculate the average rate of the reaction over this 35-minute time interval.   b) Is it correct to assume that the rate law is Rate = k[N2O5]2 based on the balanced chemical equation? Briefly explain your answer.   c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N2O5 concentration (–∆[N2O5]/∆t) and the rate of increase of NO2 concentration (∆[NO2]/∆t). Which rate will be higher and by what factor?

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