Two sealed containers of same capacity at the same temperature are filled with 44g of hydrogen gas in one and 44 g of ${\mathrm{CO}}_2$ in the other. If the pressure of ${\mathrm{CO}}_2$  is 1 atm, what is the pressure in the hydrogen container

The pressure of carbon$\Rightarrow 1=\frac{1}{1+22}\times {\mathrm{P}}_{\mathrm{total}}$dioxed  is

${\mathrm{P}}_{{\mathrm{CO}}_2}=1 \mathrm{atm}$

Mass of hydrogen ,m = 44 g

Molar mass of hydrogen MW= 2 g/mol

Mass of  ${\mathrm{CO}}_2=44\mathrm{g}$

Molar mass of ${\mathrm{CO}}_2=44\mathrm{g}/\mathrm{mol}$

${\mathrm{n}}_{{\mathrm{H}}_2}=\frac{44\mathrm{g}}{2\mathrm{g}/\mathrm{mol}}=22 \mathrm{mol}$

${\mathrm{n}}_{{\mathrm{CO}}_2}=\frac{44\mathrm{g}}{44\mathrm{g}/\mathrm{mol}}=1 \mathrm{mol}$

Now, we will use the following formula to find the partial pressure of hydrogen.

${{\mathrm{P}}_{\mathrm{CO}}}_2={\mathrm{x}}_{{\mathrm{co}}_2}.{\mathrm{P}}_{\mathrm{total}}$

${\mathrm{P}}_{\mathrm{total}}=23 \mathrm{atm}$

$\mathrm{Then},{\mathrm{P}}_{{\mathrm{H}}_2}={\mathrm{P}}_{\mathrm{total}}-{\mathrm{P}}_{{\mathrm{co}}_2}$

=23-1

=22 atm

Partial pressure of  Hydrogen in the container = 22 atm.