Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. PART A. 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol. Part B. Br2(g)+Cl2(g)⇌2BrCl(g). ΔH∘f for BrCl(g) is 14.6 kJ/mol. K=?
Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. PART A. 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol. Part B. Br2(g)+Cl2(g)⇌2BrCl(g). ΔH∘f for BrCl(g) is 14.6 kJ/mol. K=?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 105QRT
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Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K.
PART A. 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol.
Part B. Br2(g)+Cl2(g)⇌2BrCl(g). ΔH∘f for BrCl(g) is 14.6 kJ/mol.
K=?
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