# The reaction of cyanamide, NH2CN(s), with dioxygen was carried out in a bomb calorimeter, and ∆U was found to be –742.7 kJ mol–1 at 298 K

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The reaction of cyanamide, NH2CN(s), with dioxygen was carried out in a bomb calorimeter, and ∆U was found to be –742.7 kJ mol–1 at 298 K. Calculate enthalpy change for the reaction at 298 K.

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Enthalpy change for a reaction (∆H) is given by the expression,

∆H = ∆U + ∆ngRT

Where,

∆U = change in internal energy

∆ng = change in number of moles

For the given reaction,

∆ng = ∑ng (products) – ∑ng (reactants)

= (2 – 2.5) moles

∆ng = –0.5 moles

And,

∆U = –742.7 kJ mol–1

T = 298 K

R = 8.314 × 10–3 kJ mol–1 K –1

Substituting the values in the expression of ∆H:

∆H = (–742.7 kJ mol–1 ) + (–0.5 mol) (298 K) (8.314 × 10–3 kJ mol–1 K –1

= –742.7 – 1.2

∆H = –743.9 kJ mol–1

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