The first order rate constant for the decomposition of N205, according to the reaction: 2 N2O5(g) -> 4 NO2(g) + O2(g) at 70°C is 6.82 x 103 s. Suppose we start with 0.0250 moles of N,Os(g) in a volume of 2.0L. a) How many moles of N2O5 will remain after 5.0 min? b) How many minutes will it take for the quantity of N2Os to drop to 0.010 moles? c) What is the half-life of N,Os at 70°C

The first order rate constant for the decomposition of N205, according to the reaction: 2 N2O5(g) -> 4 NO2(g) + O2(g) at 70°C is 6.82 x 103 s. Suppose we start with 0.0250 moles of N,Os(g) in a volume of 2.0L. a) How many moles of N2O5 will remain after 5.0 min? b) How many minutes will it take for the quantity of N2Os to drop to 0.010 moles? c) What is the half-life of N,Os at 70°C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

100%

The first order rate constant for the decomposition of N205, according to the reaction:
2 N2O5(g)
->
4 NO2(g) + O2(g)
at 70°C is 6.82 x 103 s.
Suppose we start with 0.0250 moles of N,Os(g) in a volume of 2.0L.
a) How many moles of N2O5 will remain after 5.0 min?
b) How many minutes will it take for the quantity of N2Os to drop to 0.010 moles?
c) What is the half-life of N,Os at 70°C

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