$56$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

According to Dalton's law, Partial pressure of a component = Mole fraction x Total pressure

Given. Mass of $N_2=56$g 

mass of ${\mathrm{O}}_2=96g$

Total pressure $=10\mathrm{arm}$

$n_{N_2}=\frac{56}{28}=2,{}^n\mathrm{O}_2=\frac{96}{32}=3$

$X_{N_2}=\frac{2}{2+3}=0.4$

$X_{O_2}=\frac{3}{2+3}=0.6$

$\therefore p_{N_7}=0.4\times 10=\pm \cdots \cdots$

${\mathrm{P}}_{{\mathrm{O}}_2}=0.6\times 10=6\mathrm{ct}$