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Question

A sample of CH4 of 0.08 g was subjected to combustion at 27oC in a bomb calorimeter. The temperature of the calorimeter system was found to be raised by 0.25oC. If heat capacity of calorimeter is 18 kJ, ΔH for combustion of CH4 at 27oC is:

A
900 kJ/mole
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B
905 kJ/mole
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C
895 kJ/mole
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D
890 kJ/mole
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Solution

The correct option is B 905 kJ/mole
CH4(g)+2O2(g)CO2(g)+2H2O(l)
ΔE= Heat of combustion
= Heat capacity × rise in T × Molar massMass of compound
=18×0.25×160.08
=900 KJ/mole R=8.314×103KJmol1
ΔH=ΔE+ΔnRT Δn=13=2
=900+(2)×8.314×103×300 T=300K
=9004.9884=904.98905KJ/mol

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