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Question

The difference between ΔH and ΔE on a molar basis for the combustion of n-octane at 25oC would be:

A
13.6 kJ
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B
1.14 kJ
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C
11.15 kJ
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D
+11.15 kJ
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Solution

The correct option is D 11.15 kJ
Let us consider the problem:
Combustion of n-octane is
C8H18(l)+252O28CO2(g)+9H2O
Hence, the relation between ΔH and ΔH is
ΔH=ΔE+(RTΔn)
Implies that
ΔHΔE=(RTΔn)
Therefore
Δn=npnr=9+8252=4.5
Hence the answer is
ΔHΔE=(8.314×298×4.5)
ΔH=11149.07J
ΔH=11.15KJ

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