1. Tardigrade
  2. Question
  3. Chemistry
  4. The reaction of cyanamide NH 2 CN ( s ) with oxygen was carried out in a bomb calorimeter and Δ q v at 300 K was measured to be -750 kJ / mol. The value of Δ H per mole of NH 2 CN ( s ) in the given reaction is

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Q. The reaction of cyanamide $NH _{2} CN ( s )$ with oxygen was carried out in a bomb calorimeter and $\Delta q_{ v }$ at $300\, K$ was measured to be $-750 \,kJ / \,mol$. The value of $\Delta H$ per mole of $NH _{2} CN ( s )$ in the given reaction is

Thermodynamics

Solution:

The combustion reaction is:

$NH _{2} CN ( s )+\frac{3}{2} O _{2}( g ) \rightarrow N _{2}( g )+ CO _{2}( g )+ H _{2} O ( l )$

$\Delta n=\frac{1}{2}$

$\Delta H=\Delta E+\Delta n R T=-750+\frac{1}{2} \times 8.314 \times 10^{-3} \times 300$

or $\Delta H=-750+0.15 \times 8.314=-748.75\, kJ /\, mol$