Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question

The reaction

                        2 NO(g)   ⇆  N2O4(g)

occurs at 25oC under standard state conditions with ΔGo = 13.1 kJ/mol. What is the free energy change (in J/mol) when the NO partial pressure is 0.649 Atm and the N2O4 partial pressure is 0.0015 Atm?

Expert Solution
Check Mark
Given

The equilibrium reaction given in the question is -

 2 NO (g)   ⇌  N2O4 (g)

Standard Gibbs free energy, ΔGo = 13.1 kJ/mol = 13100 J/mol

The partial pressure of NO = 0.649 atm

The partial pressure of N2O4 = 0.0015 atm

Temperature, T = 25oC = 298 K

The Gibbs free energy

The standard Gibbs free energy is given as-

∆G°=-RT ln K

The Gibbs free energy at non-standard conditions is given as-

∆G =∆G° + RT ln K

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