2g of ${\mathrm{H}}_2$  gas diffused through a porous pot in 10 minutes. Under the same conditions how many grams of ${\mathrm{O}}_2$  will diffuse through the same pot

Two different gases are diffuse in same time

${\mathrm{t}}_1={\mathrm{t}}_2=10 \min$

mass of hydrogen, m=2g

Molar mass of hydrogen

${\mathrm{M}}_{{\mathrm{H}}_2}=2\mathrm{g}/\mathrm{mol}$

Molar mass of oxygen

${\mathrm{M}}_{{\mathrm{O}}_2}=32 \mathrm{g}/\mathrm{mol}$

The relation between time and molar mass is as follows:

$\frac{t_1}{t_1}=\sqrt{\frac{m_2}{m_1}}=\frac{w_1}{t_1}\times \frac{t_2}{w_2}=\sqrt{\frac{M_1}{M_2}}$

$\Rightarrow \frac{t_1}{t_1}=\sqrt{\frac{32}{2}}=\sqrt{16}=4:1$

$\frac{2}{10}\times \frac{10}{w_2}=\sqrt{\frac{2}{32}}=\frac{1}{4}$

The weight of $w_2$=8g