Chapter 16, Problem 91QAP

Interpretation Introduction

Interpretation:

The graph for the reaction which is exothermic in nature, the value of $\Delta n_g$ less than zero and at equilibrium at 200 K 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.

The value of $\Delta G^{\circ }$ can be calculated from equilibrium constant as follows:

$\Delta G^{\circ }=-RT\mathrm{lnK}$

Here, R is Universal gas constant, T is temperature and K is equilibrium constant.