56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a...

56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 atm . The partial pressures of oxygen and nitrogen (in atm) are respectively

Options

A4,6
B5,5
C2,8
D6,4

Correct answer

D. 6,4

Step-by-step solution

According to Dalton's law,

p_{\text{solute }}=x_{\text{solute }} \times p

Given, mass of

\mathrm{N}_2=56 \mathrm{~g}\therefore

Moles of

\mathrm{N}_2\left(n_{\mathrm{N}_2}\right)=\frac{56}{28}=2 \mathrm{~mol}

Mass of

\mathrm{O}_2=96 \mathrm{~g}\therefore

Moles of

\mathrm{O}_2\left(n_{\mathrm{O}_2}\right)=\frac{96}{32}=3 \mathrm{~mol}x_{\mathrm{N}_2}=\frac{2}{2+3}=0.4 x_{\mathrm{O}_2}=\frac{3}{2+3}=0.6 \therefore \quad p_{\mathrm{N}_2}=x_{\mathrm{N}_2} \times p=0.4 \times 10=4 \mathrm{~atm} p_{\mathrm{O}_2}=x_{\mathrm{O}_2} \times p=0.6 \times 10=6 \mathrm{~atm}

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