Question

A mixture of nitrogen and hydrogen in the ratio of one mole of nitrogen to three moles of hydrogen was partially converted into $N{H}_3$, so that the final product was a mixture of all these three gases. The mixture was to have a density of $0.46$ g per litre at ${27}^{o}C$ and $1$ atm. The mass of gas in $22.4$ litres at $1$ atm and $273$ K is :

• A. $11.33$ g
• B. $21.42$ g
• C. $13.45$ g
• D. $17.23$ g

Answer 1

Answer: (A)

$11.33$ g

$PM=\rho RT$
Thus, $\rho \propto \frac{1}{T}$

${\rho }^{\prime }=\rho \times \frac{T}{T^{\prime }}=0.46\times \frac{300}{273}=0.505g/L$
The mass of gas in 22.4 L will be $22.4\times 0.505=11.33g$