Question

A gaseous mixture contains 433.0 Torr of H2(g), 365.5 Torr of N2(g), and 78.1 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases. XH2= , XN2=, XAr=?

Answer 1

According to dalton's law total pressure of gas is equal to sum of partial pressure exerted by each individual gas

P_total = P₁ + P₂ + P₃

Total pressure = 433 + 365.5 + 78.1 = 876.6 torr

we know the formla

X_i = P_i / P where, X_i =mole fraction of indivisual gas, P_i = partial pressure of indivisual gas, P = total pressure of gas mixture

mole fraction of H₂ = 433/876.6 = 0.4939

mole fraction of N₂ = 365.5.5/876.6 = 0.4169

mole fraction of Ar = 78.1/ 876.6 = 0.08909