Chapter 16, Problem 92QAP

Interpretation Introduction

(a)

Interpretation:

For the given reaction, the value of $\Delta S^{\circ }$ at all the temperatures needs to be determined.

Concept introduction:

Entropy is defined as degree of randomness in a system. It is due to the random motion of molecules in the reaction system. The entropy of a gaseous system is more than a liquid system as gaseous molecules are in constant motion. For any state of matter, some degree of randomness is always present in the system.

Interpretation Introduction

(b)

Interpretation:

For the given reaction, the value of $\Delta H^{\circ }$ at all the temperatures needs to be determined.

Concept introduction:

The relation between $\Delta G$, $\Delta H$ and $\Delta S$ is as follows:

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

Here, $\Delta G$ is change in Gibbs free energy, $\Delta H$ is change in enthalpy and $\Delta S$ is change in entropy of the reaction.

For a spontaneous reaction, the value of $\Delta G$ for the reaction is negative.

Interpretation Introduction

(c)

Interpretation:

For the given reaction, the value of $\Delta G^{\circ }$ at all the temperatures needs to be determined.

Concept introduction:

The relation between $\Delta G$, $\Delta H$ and $\Delta S$ is as follows:

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

Here, $\Delta G$ is change in Gibbs free energy, $\Delta H$ is change in enthalpy and $\Delta S$ is change in entropy of the reaction.

For a spontaneous reaction, the value of $\Delta G$ for the reaction is negative.