Chapter 18.6, Problem 18.6CYU

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Oxygen was first prepared by Joseph Priestley (1733-1804) by heating HgO. Use data in Appendix L to estimate the temperature required to decompose HgO(s) into Hg(ℓ) and O2(g).

Interpretation Introduction

Interpretation:

The temperature required for decomposition of HgO (s) into Hg(l) and O2(g) should be estimated by using data in Appendix L.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and entropy by the following expression,

ΔGo= ΔHo-TΔSo

Here, ΔHo is the change in enthalpy and ΔSo is the change in entropy.

Explanation

The temperature required to decompose HgO (s) is calculated below.

Given: Decomposition of HgO (s) into Hg(l) and O2(g).

The Appendix L was referred for the values of standard entropies and enthalpies.

HgO(s)Hg(l)+12O2(g)ΔfH°(kJ/mol)- 90.8300So( J/K×mol)+70.29+ 76.02+ 205.07

ΔrH°fH°(products) - fH°(reactants)

ΔrH°[[(1 mol Hg(l)/mol-rxn)ΔfH°[Hg(l)]+(0.5 mol O2(g)/mol-rxn)ΔfH°[O2(g)]](1 mol HgO(s)/mol-rxn)ΔfH°[HgO(s)]]

Substituting the enthalpies values,

ΔrH°=[[(1 mol Hg(l)/mol-rxn)(0)+(0.5 mol O2(g)/mol-rxn)(0)](1 mol HgO(s)/mol-rxn)(-90

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