Where, $\mathrm{p}_{2}=$ pressure of $\mathrm{N}_{2}$ at $\mathrm{STP}=760\, \mathrm{mm}$
$\mathrm{T}_{2}=$ Temperature of $\mathrm{N}_{2}$ at $\mathrm{STP}=273\, \mathrm{K}$
$V_{2}=?$
Volume of $\mathrm{N}_{2}$ at $\mathrm{STP}$ (by Gas equation)
$\left(\frac{\rho-\rho_{1}}{t+273}\right) V_{1} \times \frac{273}{160}=V_{2}$
Where $\mathrm{p}_{1}=\rho-\rho_{1}$
$\rho=715\, \mathrm{mm}$ (pressure at which $\mathrm{N}_{2}$ collected)
$\rho_{1}=$ aqueous tension of water $=15\, \mathrm{mm}$
$T_{1}=t+273=300\, k$
$\mathrm{V}_{1}=55\, \mathrm{mL}=$ volume of moist nitrogen in nitrometer $\therefore V_{2}=\frac{(715-15) \times 55}{300} \times \frac{273}{760}=40.098\, \mathrm{mL}$
$\%$ of nitrogen in given compound
$=\frac{28}{22400} \times \frac{V_{2}}{W} \times 100$
$=\frac{2}{22400} \times \frac{46.09}{0.35} \times 100$
$=16.45 \%$
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