Chapter 5.10, Problem 29P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

Thermodynamic stability can be represented as $\Delta G^0$.  Depend upon the value of $\Delta G^0$ it is possible to find stability of the product compared with the reactant.

If $\Delta G^0$ is negative, then the product is thermodynamically stable compared with the reactant.

If $\Delta G^0$ is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

Kinetic stability can be represented as $\Delta G^{\mp }$.  Depend upon the value of $\Delta G^{\mp }$ it is possible to find stability of the product compared with the reactant.

If $\Delta G^{\mp }$ is large, then the reactant is kinetically stable because it reacts slowly.

If $\Delta G^{\mp }$ is small, then the reactant is kinetically unstable because it reacts rapidly.

If $\Delta G^{\mp }$ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

Kinetic stability can be represented as $\Delta G^{\mp }$.  Depend upon the value of $\Delta G^{\mp }$ it is possible to find stability of the product compared with the reactant.

If $\Delta G^{\mp }$ is large, then the reactant is kinetically stable because it reacts slowly.

If $\Delta G^{\mp }$ is small, then the reactant is kinetically unstable because it reacts rapidly.

If $\Delta G^{\mp }$ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.