Question

Problem Page

A

9.00L

tank at

29.2°C

is filled with

10.1g

of carbon dioxide gas and

10.6g

of chlorine pentafluoride 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. Be sure your answers have the correct number of significant digits.

carbon dioxide mole fraction: partial pressure: atm chlorine pentafluoride mole fraction: partial pressure: atm Total pressure in tank: atm

Answer 1

> 0.08125 mole Solution - Griven that;- volume of tank = gol Tempreature of tank = 29.2°C or (273 +29.2)-302.2K mass of courbon dioxide (Cey) (Mco, ) = 100g molar mass of CO2 = 44 g/mol So mote of CO2 (Mco, J = Mcoz » 10:1g 20-2295 mol m (moler mass), con 44 g/mol mass of chlorine pentaftuoride = 10.69 molax meus of Cifig = 13045g/mo! So more of Cifg = (maus \molar mass ) cifs = 1069 130-45 g/mol According to ideal gas equation Pv=nRT or P= MRT do Particul poefsurs of coz (Roz) =) 0.2295 morso.0.0821 4. atm X302:28 Partial Pressure of CO2 (PCO) = 0.633 atm. 9.004 tmelik Partial forgsure of Cifs (Prifs) = 0.08125 mole 40.0 82 \alm #302. 2X 9.00 kk melk Partial Pressure of Gifs Celta)= 0.224 am mole fraction of coz (Xc0z) = Mole fraction of coz (X - mole of co2 => 0·22 95 mole Teted more ” 0.2295+0:08125) more 0.2295 mole = 0.738 0:31075 mele. mole fraction - more of Cifs of Cifs (Xcifs) = Toteul mole 0.03125 Male = 0.262 > Ö. 31075 molé Total Pressure = P62 t Parfs) = (0.633 70.224) = 0·857 alm. 0.738 0.633 atm Carbon dioxide more traction Partied Pressure mot fraction 10:262 Partley pressure (0.224 chlorine Penta tlaride. 0.857 att Hotel Pressure in Tank