Question

If sulfur dioxide diffuses through a porous barrier at the rate of 2.4 mol/min, at what rate would chlorine diffuse? Assume that the gases behave ideally.

Answer 1

Molecular mass of $SO_2(m_1)=64 gm$

Molecular mass of $Cl_2(m_2)=35.5 \times 2=71 \ gm$

By using Graham law of diffusion,

$\frac{r_1}{r_2}=\sqrt{\frac{m_2}{m_1}}$

where $r_1$ and $r_2$ are rate of diffusion respectively.

$r_1=2.4 \ mol/min$

Using the above equation,

$\frac{2.4}{r_2}=\sqrt{\frac{71}{64}}\implies r_2=2.28 \ mol/min$