   Chapter 5, Problem 49PS

Chapter
Section
Textbook Problem

The enthalpy changes for the following reactions can be measured:CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)ΔrH° = −802.4 kJ/mol-rxnCH3OH(g) + 3 2 O2(g) → CO2(g) + 2 H2O(g)ΔrH° = −676 kJ/mol-rxn (a) Use these values and Hess’s law to determine the enthalpy change for the reaction CH4(g) + ½ O2(g) → CH3OH(g) (b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.

(a)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation of CH3OH 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 those reactions-Hess’s law.

Explanation

The required equation for the formation of CH3OH is the reverse of 2rd

Equation i.e,

CO2+2H2OCH3OH+3/2O2

ΔrH20=676kJ/mol

2nd equation should be subtracted from the 1nd equation

The net equation is CH4+1/2O2-CH3OH

(b)

Interpretation Introduction

Interpretation:

The energy level diagram for the formation of CH3OH has to be drawn.

Concept Introduction:

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

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