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Question

What will be the pressure exerted by a mixture of $$3.2\ g$$ of methane and $$4.4\ g$$ of $$CO_{2}$$ contained in a $$9\ dm^{3}$$ flask at $$27\ C$$.


Solution

The number of moles of methane is $$\displaystyle \frac {3.2}{16}=0.2 $$.
The pressure exerted by methane is $$\displaystyle P = \frac {nRT}{V} =   \frac {0.2 \times 8.314 \times 300}{9 \times 10^{-3}} = 5.54 \times 10^{4}Pa$$.
The number of moles of $$CO_2$$ is $$\displaystyle \frac {4.4}{44}=0.1 $$.
The pressure exerted by $$CO_2$$ is $$\displaystyle P' = \frac {n'RT}{V} =   \frac {0.1 \times 8.314 \times 300}{9 \times 10^{-3}} = 2.77 \times 10^{4}Pa$$.
The total pressure is $$\displaystyle P +P' = 5.54 \times 10^{4}Pa+2.77 \times 10^{4}Pa=8.31 \times 10^{4}Pa$$.

Chemistry
NCERT
Standard XI

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