Consider the dimerization equilibrium of NO2(g): 2NO2(g) N2O4(g) Answer the following questions using only the information provided. a. (7%) At a total pressure of 1 bar and T = 298. 15 K, the partial pressure of NO2(g) and N2O4(g) in an equilibrium mixture of the two gases are found to be 0.3181 and 0.6819 bar, respectively. Calculate the equilibrium constant and ° for the reaction. b. (17%) Suppose you insert one mole of NO2(g) at 298.15 K into a different 1 .0 L container. Determine the number of moles of NO2(g) and N2O4(g) present in the container after reaching equilibrium. In addition, compute AG and AA for the process. Is the dimerization spontaneous in this system?

Consider the dimerization equilibrium of NO2(g): 2NO2(g) N2O4(g) Answer the following questions using only the information provided. a. (7%) At a total pressure of 1 bar and T = 298. 15 K, the partial pressure of NO2(g) and N2O4(g) in an equilibrium mixture of the two gases are found to be 0.3181 and 0.6819 bar, respectively. Calculate the equilibrium constant and ° for the reaction. b. (17%) Suppose you insert one mole of NO2(g) at 298.15 K into a different 1 .0 L container. Determine the number of moles of NO2(g) and N2O4(g) present in the container after reaching equilibrium. In addition, compute AG and AA for the process. Is the dimerization spontaneous in this system?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 51E: In the laboratory, hydrogen chloride (HCl(g)) and ammonia (NH3(g)) often escape from bottles of...

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