The rate of diffusion of Hydrogen is about

Molar mass of ${\mathrm{H}}_2\left({\mathrm{M}}_1\right)=2\mathrm{g}$

Molar mass of He $\left({\mathrm{M}}_2\right)=4g$

${\mathrm{M}}_2=4\mathrm{g}$

$\frac{{\mathrm{r}}_1}{{\mathrm{r}}_2}=\sqrt{\frac{M_2}{M_1}}$

$\frac{{\mathrm{r}}_{\mathrm{H}}}{{\mathrm{r}}_{\mathrm{He}}}=\sqrt{\frac{4}{2}}$

${\mathrm{r}}_{\mathrm{H}}=\sqrt{2}{\mathrm{r}}_{\mathrm{He}}$

${\mathrm{r}}_{\mathrm{H}}=1.414 \mathrm{times} \mathrm{of} \mathrm{He}$

∴ The rate of diffusion of H2 is about 1.414 times that of He.