Question

a mixture of h2 and he are in a 10.0 l vessel at 273 k. the total pressure is 756 torr. what is the partial pressure of h2 in the vessel if xhe

Answer 1

Partial pressure of H₂ in the vessel is 189 torr.

What does Dalton's Law of Partial Pressures state?

According to Dalton's law of partial pressures, the total pressure a gas mixture exerts is equal to the sum of the partial pressures of its individual constituent gases. The partial pressure is the pressure that each gas would have if it occupied the same volume of the mixture at the same temperature on its own.

According to Dalton's law of partial pressures,

$P_{Total} = P_{A} +P_{B} + P_{C}$

$P_A},P_{B} ,P_{C}$ are partial pressures of A,B,C

And $P_{A} =P_{Total} .X_{A}$

$X_{A}= mole refraction of A.$

Also $X_{A} +X_{B} +X_{C} =1$

Here, 2 gases, H₂ and He

and $X_{He}$=0.75

$X_{He}+X_{H_{2} }$ = 1

$X_{H_{2} } = 1- X_{He}$

$X_{H_{2} }$=1 - 0.75

$X_{H_{2} }$=0.25

Then, $P_{H_{2} } = P_{Total} .X_{H_{2} }$

$P_{H_{2} }$= 756×0.25

$P_{H_{2} }$= 189 torr.

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