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Question

A mixture of Nitrogen and Oxygen has volume 3000 cm3 at temperature 300 K, pressure 200 kPa and mass 6.88 g. Then, which of the following options is/are correct?
[Take R=8.3 J/mol K]

A
Mass of Nitrogen in the mixture is 5.6 g.
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B
Mass of Nitrogen in the mixture is 1.28 g.
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C
Mass of Oxygen in the mixture is 1.28 g.
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D
Mass of oxygen in the mixture is 5.6 g.
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Solution

The correct option is C Mass of Oxygen in the mixture is 1.28 g.
Let us assume that n1 and n2 are the number of moles of Nitrogen and Oxygen respectively.
From Dalton's law of partial pressures, we can say that
P=P1+P2
Using ideal gas equation, we get
P=n1RTV+n2RTV
=(n1+n2)RTV
200×103=(n1+n2)×8.3×3003000×106
(n1+n2)=0.24 .....(1)

Given, mass of the mixture is 6.88 g.
i.e n1×28+n2×32=6.88
14n1+16n2=3.44.......(2)
Now, from (1),
n1=0.24n2
Substituting the value of n1 in (2), we get
14(0.24n2)+16n2=3.44 g
3.3614n2+16n2=3.44 g
2n2=0.08
n2=0.04 mol
Then, from (1) we get,
n1=0.240.04
n1=0.2 mol
Thus,
Mass of Nitrogen =0.2×28=5.6 g
Mass of oxygen =0.04×32=1.28 g
Hence, options (a) and (c) are the correct answers.

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