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Question

Compute the heat of formation of liquid methyl alcohol in kilojoules per mole using the following data.
The heat of vaporisation of liquid methyl alcohol = 38 kJ/mol.
The heats of formation of gaseous atoms from the elements in their standard states: H,218 kJ/mol; C,715 kJ/mol; O,249 kJ/mol.
Average bond energies: CH=415 kJ/mol; CO=365 kJ/mol; OH=463 kJ/mol.

A
275 kJ/mol
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B
488 kJ/mol
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C
Zero
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D
356 kJ/mol
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Solution

The correct option is A 275 kJ/mol
C(s)+2H2(g)+12O2(g)CH3OH(l);ΔH=?
So, ΔHf=[ΔHC(s)C(g)+2ΔHHH+1/2ΔHO=O][3ΔHCH+ΔHCO+ΔHOH+ΔHvap.CH3OH]
For reactants;
Heat of atomisation of 1 mole of C=715 kJ
Heat of atomisation of 4 moles of H=4×218 kJ
Heat of atomisation of 1 mole of O=249 kJ
For products:
Heat of formation of 3 moles of CH bonds = 3×415 kJ
Heat of formation of 1 mole of CO bonds = 356 kJ
Heat of formation of 1 mole of OH bonds = 463 kJ
Heat of condenstation of 1 mole of CH3OH to liquid =38 kJ
So, On adding, we get ΔH of formation of CH3OH(l):
ΔH=715+(4×218)+249(3×415)36546338
ΔH=275 kJ/mol

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