Chapter 7, Problem 7.22UKC

(a)

Interpretation Introduction

Interpretation:

The sign of change in entropy has to be determined.

Concept Introduction:

Entropy $\left(S\right)$: It is used to describe the disorder. It is the amount of arrangements possible in a system at a particular state.

If the disorder increases in a system, then $\Delta S>0$

If the disorder decreases in a system, then $\Delta S<0$

(b)

Interpretation Introduction

Interpretation:

The spontaneity of the given reaction in all temperature has to be determined.

Concept Introduction:

• Enthalpy $\left(H\right)$: it is the total amount of heat in a particular system.
• Entropy $\left(S\right)$: It is used to describe the disorder. It is the amount of arrangements possible in a system at a particular state.
• Free energy change $\left(\Delta G^0\right)$: Change in the free energy takes place while reactants convert to product.
• The free energy $\Delta G$ can be determined by

$\Delta G=\Delta H-T\Delta S$

Where,

$\Delta G$ is the change in free energy

$\Delta H$ is the change in enthalpy

$\Delta S$ is the change in entropy

T is the temperature.

Spontaneous reactions releases the free energy and has $\Delta G<0$ (exergonic)

Nonspontaneous reactions absorbs the free energy and has $\Delta G>0$ (endergonic)