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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?

A
XO2 = 0.2 ; XH2 = 0.8
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B
XO2 = 0.4 ; XH2 = 0.6
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C
XO2 = 0.6 ; XH2 = 0.4
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D
XO2 = 0.8 ; XH2 = 0.2
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Solution

The correct option is A XO2 = 0.2 ; XH2 = 0.8
Let pressure exerted by oxygen O2 be = PO2
and hydrogen M2 be = PH2
On ignition
H2+12O2H2O
due to ignition oxygen is removed now pressure is only due to remaining hydrogen
PH22PO2=0.4atm
PH2+PO2=1atm
on soloing PH2=0.8atm PO2=0.2atm
So composition be XH2=0.8 XO2=0.2

1073246_879488_ans_3badedde5d6c4f2a83521349a5dd9adf.png

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