   Chapter 5, Problem 58PS

Chapter
Section
Textbook Problem

Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:(a) 0.054 g of sulfur burns, forming SO2(g)(b) 0.20 mol of HgO(s) decomposes to Hg(ℓ) and O2(g)(c) 2.40 g of NH3(g) is formed from N2(g) and excess H2(g)(d) 1.05 × 10–2 mol of carbon is oxidized to CO2(g)

(a)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation the following reaction has to be determined.

Concept Introduction:

If a reaction proceeds in two or more other reaction,ΔrH0 for the overall process is the sum of ΔrH0 values of all those reactions-Hess’s law.

The change in enthalpy, ΔH in kJ per mole of a given reactant for the reaction can be calculated as:

ΔrH=enthalpy changenumber of moles

ΔrH=ΔHnumber of moles

Explanation

Given mass is 1.0g

The enthalpy of formation is  -296.8 KJ/Mol

S+O2SO2  ΔfH0= -296.8 KJ/Mol

The change in enthalpy, ΔH in kJ per mole of a given reactant for the reaction can be calculated as:

Δ

(b)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation the following reaction has to be determined.

Concept Introduction:

If a reaction proceeds in two or more other reaction,ΔrH0 for the overall process is the sum of ΔrH0 values of all those reactions-Hess’s law.

(c)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation the following reaction has to be determined.

Concept Introduction:

If a reaction proceeds in two or more other reaction,ΔrH0 for the overall process is the sum of ΔrH0 values of all those reactions-Hess’s law

(d)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation the following reaction has to be determined.

Concept Introduction:

If a reaction proceeds in two or more other reaction,ΔrH0 for the overall process is the sum of ΔrH0 values of all those reactions-Hess’s law.

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