Chapter 17, Problem 17.78QP

(a)

Interpretation Introduction

Interpretation:

The reaction type should be identified given sulfur formation reaction.

Concept Introduction:

Disproportionation reaction: These are a special type of reaction where an element in one oxidation state is simultaneously oxidized and reduced.

One of the reacting substance in a disproportionation reaction always contains an element that can exist in at least oxidation state.

The element in the form of reacting substance is in the intermediate oxidation state.

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant $Kp$ value should be derived given the redox reaction at ${\text{25}}^{°}\text{C}$.

Concept Introduction:

Free energy: is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work.  The free energy is represented by the letter $\text{G}$.  All spontaneous process is associated with the decrease of free energy in the system.  The free energy change ${\text{(ΔG}}_{\text{rxn}})$ is the difference in free energy of the reactants and products in their standard state.

$\begin{array}{l}{\text{ΔG}}^{\text{0}}\text{=-RTln}\text{K}\\ \text{ΔG}=Freeenergy\\ {\text{ΔG}}^{\text{0}}=S\tan dard-statefreeenergy\\ \text{R}\text{=}\text{Gas}\text{Constant}(8.31\text{4}\text{J/K×mol/K}\text{.mol)}\\ T=\text{Temprature}2\text{73}\text{K}\\ \text{K=}\text{Equlibrium}\text{Constant}{\text{(K}}_{\text{P}}\text{and}{\text{K}}_{\text{C}}\text{)}\\ \ln =(-ve(\log )\text{State Function})\end{array}$

(c)

Interpretation Introduction

Interpretation:

It should be determine that given sulfur dioxide deposits reaction more or less effective at a higher temperature.

Concept Introduction:

Free energy (Gibbs free energy) is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work.  The free energy is represented by the letter $\text{G}$.  All spontaneous process is associated with the decrease of free energy in the system.  The standard free energy change ${\text{(ΔG}}^{\text{°}}{}_{\text{rxn}})$ is the difference in free energy of the reactants and products in their standard state.

${\text{ΔG}}^{\text{°}}{}_{\text{rxn}}\text{=}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Products)-}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Reactants)}$

Where,

$\text{"n"}$ is the number of moles