The first-order rate constant for the decomposition of N2O5, given below, at 70°C is 6.82 10-3 s-1. Suppose we start with 0.0200 mol of N2O5(g) in a volume of 1.0 L.2 N2O5(g) → 4 NO2(g) + O2(g)(a) How many moles of N2O5 will remain after 3.0 min? ____mol(b) How many minutes will it take for the quantity of N2O5 to drop to 0.005 mol? ________min(c) What is the half-life of N2O5 at 70°C? _________min

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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

Section: Chapter Questions

Problem 28QRT

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The first-order rate constant for the decomposition of N₂O₅, given below, at 70°C is 6.82 10^-3 s^-1. Suppose we start with 0.0200 mol of N₂O₅(g) in a volume of 1.0 L.

2 N₂O₅(g) → 4 NO₂(g) + O₂(g)

(a) How many moles of N₂O₅ will remain after 3.0 min?
____mol

(b) How many minutes will it take for the quantity of N₂O₅ to drop to 0.005 mol?
________min

(c) What is the half-life of N₂O₅ at 70°C?
_________min

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