A 900 L tank at 856 C is filled with 693 g of carbon monoxid

A 9.00 L tank at 8.56 °C is filled with 693 g of carbon monoxide gas and 14.3 g of boron trifuoride 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. mole fraction: carbon monoxide partial pressure: mole fraction: boron trifluoride partial pressure Total pressure in tank:

Solution

Volume = V= 9.00L

T= 8.56C= 8.56+273= 281.56K

R= 0.0821 L-atm/mol-K

mass of CO= 6.93 grams

Molar mass of CO= 12.0+15.999= 27.999 gram/mole

number of moles of CO= mass/molar mass = 6.93/27.999 = 0.248 moles

number of moles of CO= 0.248 moles

mass of BF3 = 14.3 grams

molar mass of BF3 = 10.811+3x18.998= 67.805 gram/mole

number of moles of BF3= 14.3/67.805 = 0.211 moles

Total number of moles = 0.248 + 0.211 = 0.459 moles

n-=0.459 moles

PV=nRT

P= nRT/V = 0.459 x0.0821x 281.56/9.00 = 1.179 atm

P= 1.179 atm

mole fraction of CO = number of moles of CO/total number of moles

molefraction of CO= 0.248/0.459= 0.54

molefraction of BF3 = 0.211/0.459 =0.46

partial pressure of CO= total pressure x molefraction of CO

partial pressure of CO= 1.179 x0.54 = 0.637 atm

partial pressure of BF3 = 1.179 x0.46= 0.542 atm

Total pressure = 1.179 atm