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Liquefaction of Gases and Critical Constants

400 mL of hyd...

Question

400 mL of hydrogen gas at a pressure of 300 mm $H g$ and 200 mL of hydrogen chloride gas at a pressure of 600 mm $H g$ are mixed in a one litre evacuated flask. Calculate the resulting pressure (in $mm Hg$ ) of the mixture at the same temperature.

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Solution

Mole after mixing = Mole before mixing
$n_{T} = n_{H_{2}} + n_{H C l}$ (where, $n_{T}$ = total mole of mixture)
From the ideal gas equation,
$P V = n R T$
$n = \frac{R T}{P V}$
Since, $n_{T} = n_{H_{2}} + n_{H C l}$
So
$P_{T} V_{T} / R T = P_{H_{2}} V_{H_{2}} / R T + P_{H C l} V_{H C l} / R T$
$P_{T} \times 1000 = 300 \times 400 + 600 \times 200$
$P_{T} = 240 mm Hg$

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