We have — given,
weight of N2 = 2.8 g
molecular weight of N2 = 28 g/mol
Number of moles of N2 \(=\frac{2.8\,g}{28\,g/mol}\)
= 0.1 mol
weight of CO = 2.8 g
molecular weight of CO = 28 g/mol
Number of moles of CO \(=\frac{2.8\,g}{28\,g/mol}\)
= 0.1 mol
weight of CO2 = 4.4 g
molecular weight of CO2 = 44 g/mol
Number of moles CO2 \(=\frac{4.4\,g}{44\,g/mol}\)
= 0.1 mol
Mole fraction of N2 \(=\frac{\text{moles of }N_2\,gas}{\text{Total moles of gas}}\)
= 0.1/0.1+0.1+0.1
= 0.1/0.3
= 0.33333.....
We know that —
PA = xAP
where, PA = Partially pressure of 'A'
xA = mole fraction of 'A'
P = Total pressure = 700 Torr.
Therefore,
Partially pressure of N2 = 0.3333 x 700 Torr
= 233.3 Torr
Hence option (B) is right answer.