The correct answer is the mole fraction of H 2 gas = 0.303 and the mole fraction of H2S gas = 0.652
Partial pressure of h2 = 1.787 atm - 0.543 atm
Partial pessure of h2= 1.244 atm
o 5.00L container at 30.9°C having the mixture of gases (h2s and h2) with given Pavial Ressures. Then then mole fractions =
Partial pressue of h2 = 0.543 atm
Partial pressure of h2s = 1.166 atm:
total partial pressure of the mixture (h2 and h2s) = 1.787 atm
According to Daltion low of partial pressures (from derivation)
Partial pressure of the gas= mole fraction x Total pressure
mole fraction= Partial Pressure / Total Pressure.
So mole fraction of h2 =0.543 atm / 1.787 =0.303
mole fraction of H2s =1.166/ 1.787 =0.652
According to Dalton's law of partial pressures, the total pressure of a gas mixture is equal to the sum of the partial pressures of the constituent gases
Learn more about Dalton's law of partial pressure here :-
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