   Chapter 5, Problem 57PS

Chapter
Section
Textbook Problem

Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following: (a) 1.0 g of white phosphorus burns, forming P4Ol0(s) (b) 0.20 mol of NO(g) decomposes to N2(g) and O2(g) (c) 2.40 g of NaCl(s) is formed from Na(s) and excess Cl2(g) (d) 250 g of iron is oxidized with oxygen to Fe2O3(s)

(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 -2984kJ/mol

P4+5O2P4O10  ΔfH0=-2984kJ/mol

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

<

(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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