
Concept explainers
(a)
Interpretation: The net energy exchange for the given combustion reaction of methanol and butanol needs to be determined.
Concept Introduction: In a combustion reaction, hydrocarbon reacts with oxygen to form carbon dioxide and water.
(a)

Explanation of Solution
The given reactions are as follows:
And,
The net energy change can be calculated using the following formula:
For methanol:
There are 3 C-H bonds, 1 C-O bond, and 1 O-H bond in CH3OH and 1 O=O bond in O2 thus the enthalpy of the bonds broken can be calculated as follows:
Now, there are 2 C=O bonds in CO2 and 2 H-O bonds in H2O thus the enthalpy of formation bonds is:
Now, the enthalpy of reaction can be calculated as follows:
Or,
Thus, the enthalpy of combustion of 1 mol methanol will be:
Similarly,
For butanol:
There are 3 C-C bonds, 9 C-H bonds, 1 C-O bond, and 1 O-H bond in
Now, there are 2 C=O bonds in CO2 and 2 H-O bonds in H2O thus the enthalpy of formation bonds is:
Now, the enthalpy of reaction can be calculated as follows:
Or,
Thus, the enthalpy of combustion of 1 mol butanol is -2029 kJ/mol.
(b)
Interpretation: The net energy exchange for each reaction needs to be compared with the known heat of combustion values.
Concept Introduction: The net energy change can be calculated using the following formula:
(b)

Explanation of Solution
From the bond enthalpy, the net energy exchange for the combustion of methanol and butanol is calculated as -535 kJ/mol and -2029 kJ/mol respectively.
The known heat of combustion values for methanol and butanol are -726 kJ/mol and -2671 kJ/mol. Thus, the calculated values are slightly less than the known values for the heat of combustion.
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