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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 isNH2CN(s)+32 O2(g) → N2(g) + CO2(g) + H2O(g) ∆n=12 ∆H=∆E+∆nRT=-750 + 12 × 8.314 × 10-3 × 300 or ∆H=-750 + 0.15 × 8.314 = -748.75 kJ/mol

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