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Question

The fat, glyceryl trioleate, is metabolized via the following reaction. Given the enthaplies of formation, calculate the energy (kJ) liberated when 1.00 g of this fat reacts.
(Atomic weights : C=12.01,H=1.008,O=16.00).
C57H104O6(s)+80O2(g)57CO2(g)+52H2O(I)
ΔHC57H107O6=70870kJ/mole
ΔHH2O(I)=285.8kJ/mole
ΔHCO2(g)=393.5kJ/mole

A
40.4
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B
33.4
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C
37.8
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D
42.6
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Solution

The correct option is C 37.8
ΔHr = 57XΔHCO2(g) + 52XΔHH2O(I) - ΔHC57H107O6
ΔHr = -14861.6 -22429.5 +70870 = 33578.9 kJ/mol
Molar mass of C57H107O6 = 888.402 g/mol
when 888.402 g of C57H107O6 is metabolized ΔHr = 33578.9 kJ
Therefore, when 1g of C57H107O6 is metabolized ΔHr = 33578.9/888.402 = 37.8 kJ

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