Calculate the ΔHof of C6H12O6(s) from the following data: ΔHcomb[C6H12O6(s)]=−2816kJ/mol ΔHof of CO2(g)=−393.5kJ/mol ΔHof of H2O(l)=−285.9kJ/mol
A
−126.0kJ/mol
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B
−1260kJ/mol
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C
−1220kJ/mol
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D
−160kJ/mol
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Solution
The correct option is C−1260kJ/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)=−1260KJmol−1