Chapter 14, Problem 14.51QP

Interpretation Introduction

Interpretation:

The normal boiling point of the mercury has to be found.

Concept introduction:

At normal boiling point the liquid phase of any substance is in equilibrium with its gaseous phase.  This means, the difference in free energy between the two phases is zero.  Using this assumption the normal boiling point of mercury can be found.

The equation given below helps us to calculate the change in free energy in a system.

$\text{ΔG = }\Delta {\rm H}\text{- T}\Delta \text{S}$

Entropy is the measure of randomness in the system. Entropy change in a reaction is the difference in entropy of theproducts and reactants.  $\text{(ΔS)}$ can be calculated by the following equation.

${\text{ΔS}}_{\text{rxn}}{\text{ = S}}_{\text{Products}}-{\text{ S}}_{\text{reactants}}$

Where,

${\text{S}}_{\text{reactants}}$ is the standard entropy of the reactants

${\text{S}}_{\text{Products}}$ is the standard entropy of the products

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $\text{(Δ}{{\rm H}}_{\text{sys}}\text{)}$ can be calculated by the following equation.

${\text{ΔH}}_{\text{rxn}}{\text{ = ΔH}}_{\text{produdcts}}{\text{- ΔH}}_{\text{reactants}}$

Where,

${\text{ΔH}}_{\text{reactants}}$ is the standard entropy of the reactants

${\text{ΔH}}_{\text{produdcts}}$ is the standard entropy of the products