A 100 L flask contains a binary mixture of 100 g of Argon Ar

A 1.00 L flask contains a binary mixture of 1.00 g of Argon (Ar) gas and 1.00 g of CO₂ gas at 25 ºC. (PV = nRT; R= 0.0821 L-atm/mol.K)

Total number of moles = 1/40 + 1/44 = 0.0477

So from PV = nRT

P = 0.0477*0.0821*(273+25)/1 = 1.167 atm

mole fraction of Ar = (1/40) / 0.0477 = 0.524

molefraction of CO2 = (1/44) / 0.0477 = 0.476

so partial pressure of Ar = 0.524*1.167 = 0.612 atm

partial pressure of CO2 = 0.555 atm

Total pressure in torrs = 1.167*760 = 886.92 torrs

Mole faction of CO2 = 0.476