Consider the following reaction: 1. 2 N2O5 (g) → 4 NO, (g) + O2 (g) The initial concentration of N¿O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,O5 has been consumed. (a) Calculate the average rate of the reaction over this 25-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.

Consider the following reaction: 1. 2 N2O5 (g) → 4 NO, (g) + O2 (g) The initial concentration of N¿O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,O5 has been consumed. (a) Calculate the average rate of the reaction over this 25-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.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.3CE

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