Chapter 16, Problem 16.27CP

(a)

Interpretation Introduction

Interpretation:

A graph representing the free energy diagram of a reaction is given.  Shape of the graph is described.  The point at which $\Delta G$ becomes zero has to be identified.

Significance of that point has to be outlined.

Concept Introduction:

• Entropy refers to measurement of randomness or disorderliness in the system.  More the number of molecules in a system more will be the movement of molecules and greater will be the entropy given that weak intermolecular forces prevails between molecules.
• Entropy is denoted by ‘S’ and $\Delta S°$ refers to change in entropy of the system.  $\Delta S°$ value positive for a phenomenon indicates the process is spontaneous.  $\Delta S°$ value negative for a phenomenon indicates the process is non–spontaneous
• The term free energy G, refers to energy available in the system to do work and enthalpy H, refers to heat content of the system.  Change in standard free energy is $\Delta G°$ and change in standard enthalpy is $\Delta H°.$
• All these three parameters are related by an equation,

$\Delta G°=\Delta H°-T\Delta S°$

• Standard free energy change, $\Delta G°,$ is represented as,

$\Delta G°=\Delta H°-T\Delta S°$

       Where,

$\begin{array}{l}\Delta H°=\text{ standard enthalpy change}\\ \Delta \text{S}°\text{= standard entropy change}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The reason for minimum in the plot being on the left side of the graph has to be outlined.