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)×8.3×3003000×10−6
⇒(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=0.24−n2
Substituting the value of n1 in (2), we get
⇒14(0.24−n2)+16n2=3.44 g
⇒3.36−14n2+16n2=3.44 g
⇒2n2=0.08
⇒n2=0.04 mol
Then, from (1) we get,
n1=0.24−0.04
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.