Chapter 5.10, Problem 30P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

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.
• 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.
• Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

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.
• 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.
• Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.