Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1

Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 15P

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