Answer :
The partial pressure of each gas in the mixture is 443.91 mm of Hg and 407.09 mm of Hg, respectively.
In a gas mixture, each constituent gas has a partial pressure equal to the notional pressure of its constituent gases as if they alone occupied the entire volume of the original mixture at the same temperature.
Given,
mass of hydrogen = 0.482 gram
mole = 0.482 / 2
= 0.241
mass of helium = 0.441
mole = 0.441/2
= 0.221
Total mole = 0.241 + 0.221
= 0.462
total pressure = 851 mm of Hg
The partial pressure of hydrogen = 0.241 / 0.462 × 851
= 443.91 mm of Hg
The partial pressure of helium = 0.221 / 0.462 × 851
= 443.91 mm of Hg
= 407.09 mm of Hg
Partial pressure is defined as a vessel filled with multiple gases, each exerting pressure. The pressure of each gas in the container is called partial pressure. The concept of partial pressure comes from the fact that each particular gas constitutes part of the total pressure and that part is the partial pressure of that gas.
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