Hydrazine formed from Urea is further oxidised to $N_2$ as shown below:
$N{H_2} - \mathop {\mathop C\limits^\parallel }\limits^O - N{H_2} \xrightarrow[\text{Hoffmann Bromamide Degradation}]{\text{NaOBr}} N{H_2} - N{H_2} \longrightarrow {N_2}$
Assuming 1 dL of blood sample contains 30 mg of Urea, calculate the volume of $N_2$ gas obtained at NTP from the sample.
Solution
From the reaction, 1 mol of Urea liberates 22.4 L $N_2$ at NTP
Or, 60 gm Urea liberates 22.4 L $N_2$ at NTP
Or, 1 gm Urea liberates $\frac {22.4}{60}$ L $N_2$ at NTP
Or, 30 mg Urea liberates $\frac{{22.4}}{{60}} \times 30 \times {10^{ - 3}}$ L $N_2$ at NTP
= $1.12 \times 10^{-2}$ L $N_2$ at NTP
