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Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2 (9) + O2(9) At 45°C the rate constant is 6.2 x 104s1. The reaction is first order. a What is the rate law for the reaction? Rate = k[N2Og] [NO21*[02] Rate = k[N2O5] Rate = k[NO2] [O2] Rate = k[N,O;]? b Calculate the rate of the reaction when [N2O5] is 0.40 M. Rate = 2.48x10^-4 V M/s C Calculate the half-life of the reaction. Half-life = 1.24x10^-4 x s d If the initial concentration of N2 O, is 0.20 M, what is the concentration of [ Concentration = M

Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2 (9) + O2(9) At 45°C the rate constant is 6.2 x 104s1. The reaction is first order. a What is the rate law for the reaction? Rate = k[N2Og] [NO21*[02] Rate = k[N2O5] Rate = k[NO2] [O2] Rate = k[N,O;]? b Calculate the rate of the reaction when [N2O5] is 0.40 M. Rate = 2.48x10^-4 V M/s C Calculate the half-life of the reaction. Half-life = 1.24x10^-4 x s d If the initial concentration of N2 O, is 0.20 M, what is the concentration of [ Concentration = M

Chemistry
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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Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2 (9) + O2(9) At 45°C the rate constant is 6.2 x 104s1. The reaction is first order. a What is the rate law for the reaction? Rate = k[N2Og]° [NO21*[O2] Rate = k[N2O5] Rate = k[NO2]*[O2] Rate = k[N,O;]? b Calculate the rate of the reaction when [N2O5] is 0.40 M. Rate = 2.48x10^-4 M/s C Calculate the half-life of the reaction. Half-life = 1.24x10^-4 x s d If the initial concentration of N2 O, is 0.20 M, what is the concentration of [N2O5] after 1.5 hours? Concentration = M
Transcribed Image Text:Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2 (9) + O2(9) At 45°C the rate constant is 6.2 x 104s1. The reaction is first order. a What is the rate law for the reaction? Rate = k[N2Og]° [NO21*[O2] Rate = k[N2O5] Rate = k[NO2]*[O2] Rate = k[N,O;]? b Calculate the rate of the reaction when [N2O5] is 0.40 M. Rate = 2.48x10^-4 M/s C Calculate the half-life of the reaction. Half-life = 1.24x10^-4 x s d If the initial concentration of N2 O, is 0.20 M, what is the concentration of [N2O5] after 1.5 hours? Concentration = M
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