Chapter 18.6, Problem 18.8CYU

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Determine the value of the equilibrium constant, Kp, for the decomposition of liquid water according to the following equation at 25.0 °C. 2   H 2 O ( l ) ⇄ 2   H 2 ( g ) + O 2 ( g )

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction 2H2O(l)2H2(g)+ O2(g) should be determined at 25oC.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrGo. It can be calculated in a similar manner as entropy and enthalpy.  The expression for the free energy change is:

ΔrG°fG°(products)fG°(reactants)

ΔGo is related to the equilibrium constant K by the equation,

ΔrGo= -RTlnKp.

The rearranged expression is,

Kp= e-ΔrGoRT

Explanation

The equilibrium constant for given reaction determined by calculating ΔrGo value and plugging it into the equation Kp= e-ΔrGoRT.

Given: 2H2O(l)2H2(g)+ O2(g)

The Appendix L was referred for the values of standard free energy.

The ΔrG° for H2O(l) is -237.15 kJ/mol

The ΔrG° for H2(g) is 0 kJ/mol

The ΔrG° for O2(g) is 0 kJ/mol

ΔrG°fG°(products)fG°(reactants)

ΔrG°[[(2 mol H2(g)/mol-rxn)ΔfG°[H2(g)]+(1 mol O2(g)/mol-rxn

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