A mixture of $N_2$ and Ar gases in a cylinder contains 7 g of $N_2$ and 8 g of Ar. If the total pressure of th

Question

A mixture of $N_2$ and Ar gases in a cylinder contains 7 g of $N_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of $N_2$ is : [Use atomic masses (in g $mol^{-1}$) : N = 14, Ar = 40]

Accepted Answer

$n_{N_2} = \frac{7}{28} = \frac{1}{4} = 0.25$. $n_{Ar} = \frac{8}{40} = \frac{1}{5} = 0.20$. Now, Applying Dalton's law of partial pressure, $p_{N_2} = (\chi_{N_2}) P_{Total} = \frac{0.25}{0.45} 	imes 27 	ext{ bar} = \frac{5}{9} 	imes 27 = 15 	ext{ bar}$.

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