Two gas cylinders having same capacity have been filled with $44 g$ of $H_{2}$ and $44 g$ of $C O_{2}$ respectively. If the pressure in $C O_{2}$ cylinder is $1$ atmosphere at a particular temperature, the pressure in the hydrogen cylinder at the same temperature is :

2

atmosphere

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1

atmosphere

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22

atmosphere

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44

atmosphere

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Solution

The correct option is C $22$ atmosphere
The pressure in the hydrogen cylinder at the same temperature is 22 atmosphere.
Pressure at constant volume and constant temperature is directly proportional to the number of moles of the gas.
Molar masses of carbon dioxide and hydrogen are 44 g/mol and 2 g/mol respectively.

Number of moles of carbon dioxide $= \frac{44 g}{44 g / m o l} = 1 m o l$
Number of moles of hydrogen $= \frac{44 g}{2 g / m o l} = 22 g / m o l$
$\frac{n_{C O_{2}}}{n_{H_{2}}} = \frac{P_{C O_{2}}}{P_{H_{2}}}$

$\frac{1 m o l}{22 m o l} = \frac{1 a t m}{P_{H_{2}}}$

$P_{H_{2}} = 22 a t m$

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Two gas cylinders having same capacity have been filled with 44 g of H2 and 44 g of CO2 respectively. If the pressure in CO2 cylinder is 1 atmosphere at a particular temperature, the pressure in the hydrogen cylinder at the same temperature is :

Two gas cylinders having same capacity have been filled with $44 g$ of $H_{2}$ and $44 g$ of $C O_{2}$ respectively. If the pressure in $C O_{2}$ cylinder is $1$ atmosphere at a particular temperature, the pressure in the hydrogen cylinder at the same temperature is :