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

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TestHub · Accepted Answer

Total pressure ( P Total ) = 740 mm of Hg Number of moles of gas X = 0 . 6 20 Number of moles of gas Y = 0 . 45 45 Total number of moles = 0 . 03 + 0 . 01 = 0 . 04 mole The partial pressure of the gas X = Mole fraction × Total pressure X = 0 . 03 0 . 04 × 740 = 555

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