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  • The total pressure of a mixture of non-reacting gases <img alt="X(0.6 \mathrm{~g})$ and $Y(0.45 \mathrm{~g})" src="https://entrancecorner.oncodecogs.com/gif.latex?X%280.6%20%5Cmathrm%7B%7Eg%7D%29%2

The total pressure of a mixture of non-reacting gases X(0.6 \mathrm{~g})$ and $Y(0.45 \mathrm{~g}) in a vessel is 740 \mathrm{~mm} of \mathrm{Hg}. The partial pressure of the gas \mathrm{X} is \mathrm{mm} of \mathrm{Hg}.
(Nearest Integer)
(Given : molar mass \mathrm{X}=20 and \mathrm{Y}=45 \mathrm{~g} \mathrm{~mol}^{-1})

Option: 1

555


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

\text{Number of moles of gas}\, X=\frac{0.6}{20}=0.03
\text{Number of moles of gas}\, \mathrm{Y}=\frac{0.45}{45}=0.01
\text{Total number of moles}\, \mathrm{=0.03+0.01=0.04}\: \text{mole}

Partial pressure of gas X= Mole fraction \times  Total pressure

=\frac{0.03}{0.04} \times 740=555

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