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Question

Calculate the ΔHof of C6H12O6(s) from the following data:
ΔHcomb[C6H12O6(s)]=2816 kJ/mol
ΔHof of CO2(g)=393.5 kJ/mol
ΔHof of H2O(l)=285.9 kJ/mol

A
126.0 kJ/mol
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B
1260 kJ/mol
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C
1220 kJ/mol
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D
160 kJ/mol
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Solution

The correct option is C 1260 kJ/mol
Enthalpy of formation of C6H12O6 = 6× heat of formation of CO2 + 6 × heat of formation of water - heat of combustion of C6H12O6
Enthalpy of formation of C6H12O6 = 6(393.5)+6(285.9)(2816)=1260KJmol1

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