Chemistry
Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 23, Problem 38QP
Interpretation Introduction

Interpretation:

The value of ΔH for the decomposition reaction is to be determined.

Concept Introduction:

The enthalpy of reaction is calculated by the expression as

ΔH=ΔHf(products)ΔHf(reactants).

Here, ΔH is the standard change in enthalpy of reaction, ΔHf(reactants) is the sum of standard change in enthalpy of reactants, ΔHf(products) is the standard change in enthalpy of products.

Expert Solution & Answer
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Answer to Problem 38QP

Solution:

The ΔH value for the decomposition reaction is equal to 117.6 kJ/mol.

The ΔH value for the decomposition reaction is equal to 177.8 kJ/mol.

Explanation of Solution

a) MgCO3(s)MgO(s)+CO2(g).

The value of ΔHf(MgCO3) from appendix 2 is -1112.9kJ/mol.

The value of ΔHf(CO2) from appendix 2 is 393.5kJ/mol.

The value of ΔHf(MgO) from appendix 2 is -601.8kJ/mol.

The value of ΔH for the given reaction is calculated by using the relation given below:

ΔH=ΔHf(MgO)+ΔHf(CO2)ΔHf(MgCO3)

Here, ΔH is the standard change in enthalpy, ΔHf(MgO) is the standard change in enthalpy of MgO, ΔHf(CO2) is the standard change in enthalpy of CO2 and ΔHf(MgCO3) is the standard change in enthalpy of MgCO3.

Substitute -601.8kJ/mol for ΔHf(MgO), 393.5kJ/mol for ΔHf(CO2), and -1112.9kJ/mol for ΔHf(MgCO3) in the equation as:

ΔH=(1)(-601.8kJ/mol)+(1)(393.5kJ/mol)(1)(-1112.9kJ/mol)=117.6 kJ/mol.

b) CaCO3(s)CaO(s)+CO2(g).

The value of ΔHf(CaCO3) from appendix 2 is 1206.9 kJ/mol.

The value of ΔHf(CO2) from appendix 2 is 393.5kJ/mol.

The value of ΔHf(CaO) from appendix 2 is -635.6kJ/mol.

The value of ΔH for the given reaction is calculated by using the relation given below:

ΔH=ΔHf(CaO)+ΔHf(CO2)ΔHf(CaCO3).

Here, ΔH is the standard change in enthalpy, ΔHf(CaO) is the standard change in enthalpy of CaO, ΔHf(CO2) is the standard change in enthalpy of CO2 and ΔHf(CaCO3) is the standard change in enthalpy of CaCO3.

Substitute -635.6kJ/mol for ΔHf(CaO), 393.5kJ/mol for ΔHf(CO2), and 1206.9 kJ/mol for ΔHf(CaCO3) in the equation as

ΔH=(1)(-635.6kJ/mol)+(1)(393.5kJ/mol)(1)(1206.9 kJ/mol)=177.8 kJ/mol.

The value of ΔH for MgCO3 is less as compared to the value of ΔH for CaCO3, and thus on heating, MgCO3 is more easily decomposed.

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Chapter 23 Solutions

Chemistry

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