Chapter 7, Problem 7.20UKC

(a)

Interpretation Introduction

Interpretation:

The balanced equation for the given spontaneous reaction is to be determined.

Concept Introduction:

• Enthalpy $\left(H\right)$: It is the total amount of heat in a particular system.
• Entropy $\left(S\right)$: it is used to describe the disorder. It is the amount of arrangements possible in a system at a particular state.
• Free energy change $\left(\Delta G\right)$: change in the free energy takes place while reactants convert to product.
• Chemical equation is the representation of a chemical reaction, in which the reactants and products of the reactions are represented left and right side of an arrow respectively by using their respective chemical formulas.

(b)

Interpretation Introduction

Interpretation:

The signs of $\Delta H$, $\Delta S$ and $\Delta G$ for the given  spontaneous reaction is to be determined.

Concept Introduction:

• Enthalpy $\left(H\right)$: It is the total amount of heat in a particular system.

If the value obtained for $\text{ΔH}$ in a reaction is positive then it is an endothermic reaction whereas the value obtained for $\text{ΔH}$ is negative it is an exothermic reaction.

• Entropy $\left(S\right)$: it is used to describe the disorder.  It is the amount of arrangements possible in a system at a particular state.

If the disorder increases in a system, then $\Delta S>0$

If the disorder decreases in a system, then $\Delta S<0$

• Free energy change $\left(\Delta G\right)$: change in the free energy takes place while reactants convert to product.

Spontaneous reactions releases the free energy and has $\Delta G<0$ (exergonic)

Nonspontaneous reactions absorbs the free energy and has $\Delta G>0$ (endergonic)