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Question

The reaction of cyanamide, NH2CN(s) with oxygen was run in a bomb calorimeter and ΔU was found to be 742.24kJmol1.The magnitude of ΔH298 for the reaction
NH2CN(s)+32(g)N2(g)+CO2(g)+H2O(l) is ______ kJ. (Rounded off to the nearest integer)

[Assume ideal gases and R=8.314Jmol1K1]


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Solution

NH2CN(s)+32O2(g)N2(g)+CO2(g)+H2O(l)

ΔH=ΔU+ΔngRT

Δng=232=0.5

Assume that the ΔU is given at the same temperature.
ΔH298=742.24 kJ+0.5×8.314×2981000 kJ

= - 742.24 + 1.24
= -741 kJ
|ΔH298|=741 kJ


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