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The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2 NO2(g) 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 x 10-12 L/mol-s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.4 atm to 1.1 atm at 500. K? Assume ideal gas behavior. Time = S

The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2 NO2(g) 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 x 10-12 L/mol-s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.4 atm to 1.1 atm at 500. K? Assume ideal gas behavior. Time = S

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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The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2 NO2(g) 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 x 10-12 L/mol-s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.4 atm to 1.1 atm at 500. K? Assume ideal gas behavior. Time = S
Transcribed Image Text:The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2 NO2(g) 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 x 10-12 L/mol-s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.4 atm to 1.1 atm at 500. K? Assume ideal gas behavior. Time = S
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