Chapter 5, Problem 5.55E

(a)

Interpretation Introduction

Interpretation: The side that is favored for equilibrium on increasing temperature for an exothermic process is to be explained.

Concept introduction: The temperature is related to equilibrium constant by the standard enthalpy of reaction. This ${\Delta }_{\text{rxn}}H°$ is given the formula written below.

${\Delta }_{\text{rxn}}H°={\Delta }_{\text{products}}H°-{\Delta }_{\text{reactants}}H°$

The temperature is related to equilibrium constant by the relation given below.

$\frac{\partial \ln K}{\partial T}=\frac{{\Delta }_{\text{rxn}}H°}{R{T}^2}$

In the above relation, $K$ is the equilibrium constant, ${\Delta }_{\text{rxn}}H°$ is standard enthalpy of reaction, $T$ is temperature and $R$ is gas constant. The above equation is known as van’t Hoff equation.

(b)

Interpretation Introduction

Interpretation: The side that is favored for equilibrium on increasing temperature for an endothermic process is to be stated.

Concept introduction: The temperature is related to equilibrium constant by the standard enthalpy of reaction. This ${\Delta }_{\text{rxn}}H°$ is given the formula written below.

${\Delta }_{\text{rxn}}H°={\Delta }_{\text{products}}H°-{\Delta }_{\text{reactants}}H°$

The temperature is related to equilibrium constant by the relation given below.

$\frac{\partial \ln K}{\partial T}=\frac{{\Delta }_{\text{rxn}}H°}{R{T}^2}$

In the above relation, $K$ is the equilibrium constant, ${\Delta }_{\text{rxn}}H°$ is standard enthalpy of reaction, $T$ is temperature and $R$ is gas constant. The above equation is known as van’t Hoff equation.