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

Question

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}

)

Aicharya · Accepted Answer

Total pressure ( P Total ) = 740 &#160; mm of Hg Number of moles of gas X &#160; = &#160; 0 . 6 20 Number of moles of gas Y &#160; = &#160; 0 . 45 45 Total number of moles = &#160; 0 . 03 &#160; + &#160; 0 . 01 &#160; = &#160; 0 . 04 &#160; mole The partial pressure of the gas X &#160;=&#160; Mole&#160;fraction &#160;&#215;&#160; Total&#160;pressure X &#160; = &#160; 0 . 03 0 . 04 &#160; &#215; &#160; 740 &#160; = &#160; 555

The total pressure of a mixture of non-reacting gases X ( 0 . 6   g ) and Y ( 0 . 45   g ) in a…

Solution

The total pressure of a mixture of non-reacting gases X ( 0 . 6 &#160; g ) and Y ( 0 . 45 &#160; g ) in a…

Solution

The total pressure of a mixture of non-reacting gases X ( 0 . 6 g ) and Y ( 0 . 45 g ) in a…