   # The equilibrium constant, K p , for N 2 O 4 (g) ⇄ 2 NO 2 (g) is 0.14 at 25 °C. Calculate Δ r G ° for the conversion of N 2 O 4 (g) to NO 2 (g) from this constant, and compare this value with that determined from the Δ f G ° values in Appendix L. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18, Problem 51GQ
Textbook Problem
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## The equilibrium constant, Kp, for N2O4(g) ⇄ 2 NO2(g) is 0.14 at 25 °C. Calculate ΔrG° for the conversion of N2O4(g) to NO2(g) from this constant, and compare this value with that determined from the ΔfG° values in Appendix L.

Interpretation Introduction

Interpretation:

The value of ΔrG for the given process of conversing N2O4(g) to NO2(g) should be calculated.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It is related to the equilibrium constant K by the equation,

ΔrG=RTlnK

### Explanation of Solution

The ΔrG value for thegiven process of conversion of N2O4(g) to NO2(g) is calculated below.

For the process of conversion of N2O4(g) to NO2(g)  value of equilibrium constant K is 0.14 at 25 C

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