In a mixture of gases, the total pressure is equivalent to the aggregate of all the partial pressures of the single element of the gas.
It can be written as [tex]\rm P _{total}[/tex] = P₁ + P₂ + P₃ and so on.
The partial pressure will be:
Option A. 0. 31 atm
Pressure can be estimated by:
PV = nRT
[tex]\rm P_{total} = \dfrac{n _{total }RT}{ V}[/tex]
[tex]\rm P_{total} = \dfrac{n _{H_{2}} + n _{\rm other \;gases}}{ V}[/tex]
Where,
[tex]\rm nH_{2} = 25\% \times n_{Total}[/tex]
And,
[tex]\begin{aligned}\rm P_{H_{2}} &= 25\% \times \rm P_{Total}\\\\& = 25\% \times 1.24 \;\rm atm\\\\& = 1.24 \rm \;atm \times 25 \end{aligned}[/tex]
Solving finally we get,
[tex]\rm P_{H_{2}} = 0.31 \;\rm atm[/tex]
Therefore, 0.31 atm is the partial pressure of the hydrogen gas.
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https://brainly.com/question/1471705
