Chapter 6, Problem 6.7IA

(a)

Interpretation Introduction

Interpretation:

The reason as to why the entropy of the system increases on hydrolysis of a triphosphate group into a diphosphate and phosphate group has to be stated.

Concept introduction:

The randomness present in the system is known as its entropy.  It is an extensive property.  At equilibrium, the entropy of the system is zero.  It is denoted by $S$.  The entropy that is measured under the standard conditions of temperature is known as standard entropy.  The standard entropy change is denoted by $\Delta S°$.

(b)

Interpretation Introduction

Interpretation:

The hypothesis that electrostatic repulsion between adjacent phosphate groups controls the exergonicity of the reaction has to be proved.  Whether the electrostatic repulsions affect ${\Delta }_{\text{r}}S$ and ${\Delta }_{\text{r}}H$ of the reaction or not has to be stated.

Concept introduction:

The Gibbs free energy of the system represents the maximum amount of work achieved by a thermodynamic system at isothermal and isobaric conditions.  The change in Gibbs free energy is used to predict the spontaneity of the process.  The change in Gibbs energy of the system is mathematically is represented as shown below.

  $\Delta G=\Delta H-T\Delta S$