The total pressure of a mixture of non-reacting gases $X ( 0 . 6g )$ and $Y ( 0 . 45g )$ in a vessel is $740mm$ of $Hg$ . The partial pressure of the gas $X$ is $mm$ of $Hg .$ (Nearest Integer)
(Given : molar mass $X = 20$ and $Y = 45g{mol}^{- 1}$ )

Question

The total pressure of a mixture of non-reacting gases

X ( 0 . 6g )

and

Y ( 0 . 45g )

in a vessel is

740mm

of

Hg

. The partial pressure of the gas

X

is

mm

of

Hg .

(Nearest Integer)
(Given : molar mass

X = 20

and

Y = 45g{mol}^{- 1}

)

Quantrex Academy · Accepted Answer

Correct answer: 0

Total pressure ( P _ Total ) = 740mm 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 . 04mole The partial pressure of the gas X = Mole fraction × Total pressure X = (0 . 03)/(0 . 04) × 740 = 555

The total pressure of a mixture of non-reacting gases X ( 0 . 6g )...

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