1.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 N2Os(g) in a volume of 2.0L.a) How many moles of N,Os will remain after 5.0 min?b) How many minutes will it take for the quantity of N,O5 to drop to 0.010 moles?c) What is the half-life of N2O5 at 70°C

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1. 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 N2O5(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 N2O5 to drop to 0.010 moles? c) What is the half-life of N2O5 at 70°C

1. 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 N2O5(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 N2O5 to drop to 0.010 moles? c) What is the half-life of N2O5 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

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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