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Standard XII

Chemistry

Dalton's Law of Partial Pressures

A gaseous mix...

Question

A gaseous mixture containing equal amount of nitrogen and methane has total pressure $7.86$ mm Hg at $300$ K. Calculate the partial pressure (in mm Hg) of methane in the mixture.

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Solution

Total pressure $= P$
Partial pressure of methane $= P_{m}$
Partial pressure of nitrogen $= P_{n}$
Partial pressure of methane $=$ mole fraction of methane $\times$ $P$
mol fraction of methane $= \frac{x}{16} / (\frac{x}{14} + \frac{x}{16}) = \frac{14}{30}$
$\Rightarrow \frac{14}{30} \times 7.86 = \frac{110.04}{30} = 3.668$ $m m H_{g}$ .

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A gaseous mixture containing equal amount of nitrogen and methane has total pressure 7.86 mm Hg at 300K. Calculate the partial pressure (in mm Hg) of methane in the mixture.

Total pressure =PPartial pressure of methane =PmPartial pressure of nitrogen =PnPartial pressure of methane = mole fraction of methane × Pmol fraction of methane =x16/(x14+x16)=1430⇒1430×7.86=110.0430=3.668 mmHg.

A gaseous mixture containing equal amount of nitrogen and methane has total pressure $7.86$ mm Hg at $300$ K. Calculate the partial pressure (in mm Hg) of methane in the mixture.