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Ways to Define Concentration

The total pre...

Question

The total pressure of a mixture of oxygen and hydrogen is 1.0 atm. The mixture is ignited and the water is removed. The remaining gas is pure hydrogen and exerts a pressure of 0.40 atm when measured at the same value of T and V as the original mixture. What was the composition of the original mixture in mole present?

X_{O_{2}}

= 0.2 ;

X_{H_{2}}

= 0.8

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X_{O_{2}}

= 0.4 ;

X_{H_{2}}

= 0.6

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X_{O_{2}}

= 0.6 ;

X_{H_{2}}

= 0.4

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X_{O_{2}}

= 0.8 ;

X_{H_{2}}

= 0.2

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Solution

The correct option is A $X_{O_{2}}$ = 0.2 ; $X_{H_{2}}$ = 0.8
Let pressure exerted by oxygen $O_{2}$ be = $P O_{2}$
and hydrogen $M_{2}$ be = $P_{H_{2}}$
On ignition
$H_{2} + \frac{1}{2} O_{2} \to H_{2} O$
due to ignition oxygen is removed now pressure is only due to remaining hydrogen
$P H_{2} - 2 P O_{2} = 0.4 a t m$
$P H_{2} + P O_{2} = 1 a t m$
on soloing $P H_{2} = 0.8 a t m$ $P O_{2} = 0.2 a t m$
So composition be $X_{H_{2}} = 0.8$ $X_{O_{2}} = 0.2$

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