Question

Close Problem Tutored Practice Problem 11.4.1 STOWANITED Calculate pressure using Dalton's law of partial pressures. A gas mixture is made up of Ar (11.2 g), CO (10.9 g), and Oz (10.3 g). The mixture has a volume of 27.4 L at 38 °C. Calculate the partial pressure of each gas in the mixture and the total pressure of the gas mixture. atm atm Par- Pco, Po, Ptotal = atm atm Check & Submit Answer Show Approach

Answer 1

mall a Ar - 11.29 moler mass of Ar - 39.989 1mor male of Ar = 129 – 0.280 ml Ag. 39.958) mel mass of car – (0.99 molar mag of Ca = 44.olglog receTO . ०.११ - 0.2477 nel uy.eslime mass of cr – 10. 3 9 melor mass of Oz= 32 g lines mole of or a 10.39 I = 0.3218 and on 32g|my ca total maes = o 280+ 0.2477+ 0.3218 tetal maefn) = 0.84957 mol Volume = 24.7L I-3.8+273=311k. o8u9s ] moxo.082, Lam mette & 3116 24.7L = 0.8 78 am

Mole fraction of Ar= 0.28onde 0.84957 ml = 0.3295 Toled precure nude sraction of xx partial of Ar- puellure 0.878 atm = 0.3295 x = 0.2893 atm = 0.289 atm a no = 0. 29155 Molfraction of col = 0.247 Inde 0.84957 mole autant pulsouse of co - 0.291558 0.878 alm -0.256 atn noe traction of g = 0.3218 moll 0.84957 hole 0.37877 nesene q 9:0:37877 X 0.878a6m - 0.3325 atm - 0.333 am PAs - 0.289 atm Po 0.256 alm Po2 = 0.333 dn Plat 0.878 alm