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Calculate the value of the free energy change, ΔG, for the reaction below at 300.0ºC when the pressures of NOCl (g) = 2.00 atm, NO (g) = 0.200 atm, and Cl₂ (g) = 0.200 atm. 2 NOCl (g) → 2 NO (g) + Cl₂ (g) ΔGº = 41.00 kJ ΔHº = 77.08 kJ ΔSº = 121.24 J/K ΔG = ____ kJ

Calculate the value of the free energy change, ΔG, for the reaction below at 300.0ºC when the pressures of NOCl (g) = 2.00 atm, NO (g) = 0.200 atm, and Cl₂ (g) = 0.200 atm. 2 NOCl (g) → 2 NO (g) + Cl₂ (g) ΔGº = 41.00 kJ ΔHº = 77.08 kJ ΔSº = 121.24 J/K ΔG = ____ kJ

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Calculate the value of the free energy change, ΔG, for the reaction below at 300.0ºC when the pressures of NOCl (g) = 2.00 atm, NO (g) = 0.200 atm, and Cl₂ (g) = 0.200 atm.

2 NOCl (g) → 2 NO (g) + Cl₂ (g)

ΔGº = 41.00 kJ
ΔHº = 77.08 kJ
ΔSº = 121.24 J/K

ΔG = ____ kJ

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