Question

The closed containers of the same capacity and at the same temperature are filled with $44g$ of $H_2$ in one and $44g$ of ${CO}_2$ in the other. If the pressure of carbon of carbon dioxide in the second container is 1 atm. That of hydrogen in the first container would be:

• A. 1 atm
• B. 10atm
• C. 22atm
• D. 44atm

Answer 1

Answer: (C)

22atm

Molecular weight of $C{O}_2$ = 44 g

Molecular weight of $H_2$ = 2 g

Weight of $C{O}_2$ = 44 g

Weight of $H_2$ = 44g

$\therefore$ Moles of $C{O}_2$ in the container = $\frac{\text{Given weight}}{\text{Molecular weight}}=\frac{44}{44}=1\text{mole}$

Moles of $H_2$ in the container = $\frac{\text{Given weight}}{\text{Molecular weight}}=\frac{44}{2}=22\text{mole}$

Given that 44g of $C{O}_2$ (1 mole), exerts 1 atm pressure, i.e. x mole of a gas will exert a pressure of x atm.

Hence,44g of $H_2$ (22 mole) will exert a pressure of 22 atm.