Suppose that in an industrial process N2 at 1.00 bar is mixed with H2 at 3.00 bar and the two gases are allowed to come to equilibrium with the product ammonia gas in a reactor of constant volume. At the temperature of the reactor, 25 °C, it has been determined experimentally that K= 977. The ΔfG for ammonia gas is -16.45 kJ/mol. a)Calculate the value of ΔG° for this equilibrium. b) Calculate the value of K. c)Calculate the value of ΔG.
Suppose that in an industrial process N2 at 1.00 bar is mixed with H2 at 3.00 bar and the two gases are allowed to come to equilibrium with the product ammonia gas in a reactor of constant volume. At the temperature of the reactor, 25 °C, it has been determined experimentally that K= 977. The ΔfG for ammonia gas is -16.45 kJ/mol. a)Calculate the value of ΔG° for this equilibrium. b) Calculate the value of K. c)Calculate the value of ΔG.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 101SCQ
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- Suppose that in an industrial process N2 at 1.00 bar is mixed with H2 at 3.00 bar and the two gases are allowed to come to equilibrium with the product ammonia gas in a reactor of constant volume. At the temperature of the reactor, 25 °C, it has been determined experimentally that K= 977. The ΔfG for ammonia gas is -16.45 kJ/mol.
a)Calculate the value of ΔG° for this equilibrium.
b) Calculate the value of K.
c)Calculate the value of ΔG.
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