Chapter 7, Problem 7.19UKC

Interpretation Introduction

Interpretation:

The signs of $\Delta H$, $\Delta S$ and $\Delta G$ for the spontaneous condensation reaction of vapor to liquid has 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)