A 5.00L tank at 7.03°C is filled with 17.7g of dinitrogen monoxide gas and 7.77g of sulfur tetrafluoride gas

dinitrogen-monoxide
tetrafluoride-gas

#1

A 5.00L tank at 7.03°C is filled with 17.7g of dinitrogen monoxide gas and 7.77g
of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank.

Answer:

Amount of N2O in tank = 17.7 / (14.0 x 2 + 16.0) = 0.40227 mol
Amount of SF4 in tank = 7.77 / (32.1 + 19.0 x 4) = 0.07187 mol
Mole fraction of N2O = 0.40227 / (0.40227+0.07187) = 0.848 (3sf)
Mole fraction of SF4 = 0.07187 / 0.47414 = 0.152 (3sf)

PV=nRT
P(N2O) = (0.40227)(8.31)(273+7.03) / (0.005) = 187.22 = 187 kPa (3sf)
P(SF4) = (0.07187)(8.31)(280.03) / (0.005) = 33.449 = 33.4 kPa (3sf)

Total Pressure = 187.22 + 33.449 = 221 kPa (3sf)