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Q.

The reaction of cyanamide NH2CN(s) with oxygen was carried out in a bomb calorimeter and ∆qv at 300 K was measured to be - 750 kJ / mol. The value of ∆H per mole of NH2CN(s) in the given reaction is

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a

741.75 kJ/mol

b

- 748.75 kJ/mol

c

- 752.75 kJ/mol

d

-750 kJ/mol

answer is B.

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Detailed Solution

The combustion reaction is:NH2CN(s)+32O2(g)→N2(g)+CO2(g)+H2O(l)Δn=12ΔH=ΔE+ΔnRT=−750+12×8.314×10−3×300 or ΔH=−750+0.15×8.314=−748.75kJ/mol

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