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0.5 g of benzoic acid was subjected to combustion in a bomb calorimeter at 15°C when the temperature of the calorimeter system (including water) wasfound to rise by 0.55°C. Calculate the heat of combustion of benzoic acid: (i) at constant volume and (ii) at constant pressure. The thermal capacity of the calorimeter system including water was found to be 23.85 kJ.

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answer is 1367.75 KJ.

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Detailed Solution

The chemical equation is C2H5OH(l)+3O2(g)⟶2CO2(g)+3H2O(l) So, Δn=−1Heat evolved here is at constant volume. So,ΔE=QV=C⋅ΔT=1600JK−1(37.1K)= 59360 JThis heat is given by 2 g of C2H5OH, so 1 mol will give,(59360J)46gmol−12g=1365.28kJmol−1That is =ΔE=−1365.28kJmol−1 Using equation ΔH=ΔE+RTΔnΔH=(−1365.28)+(−1)8.314×10−3(298)ΔH=−1367.75kJmol−1

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