The ratio of molar volume to atomic volume for $1$ mole of Hydrogen is. 

(Take size of hydrogen molecule to be $1 \stackrel{\circ }{A}$)

Volume occupied by $1$ mole of an ideal gas at STP is known as molar volume. 

$\therefore \mathrm{Molar} \mathrm{volume}=22.4 \mathrm{litre}=22.4\times {10}^{-3}{m}^3$

Radius of hydrogen atom is $r=0.5 \stackrel{\circ }{A}=0.5\times {10}^{-10}m$ 

$\therefore$ Atomic volume $=\frac{4}{3}\pi r^3{N}_A$

     $=\frac{4}{3}\times \frac{22}{7}\times {\left(0.5\times {10}^{-10}\right)}^3\times 6.023\times {10}^{23}=3.15\times {10}^{-7}{m}^3$

Their corresponding ratio is

$\frac{\mathrm{Molar} \mathrm{volume}}{\mathrm{Atomic} \mathrm{volume}}=\frac{22.4\times {10}^{-3}{m}^3}{3.15\times {10}^{-7}{m}^3}=7.1\times {10}^4$