Question

A 10.0 L tank at 2.59 °C is filled with 6.79 g of boron trifluoride gas and 2.90 g of carbon monoxide 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: boron trifluoride partial pressure: x 5 ? mole fraction: carbon monoxide partial pressure: Total pressure in tank

Answer 1

Answero- илм Given volume = v=102 Temp = T = 2.59°C = 2.59+273 T=275.59K. BF given mass =W, = 6.79 BE molar mass=M, = 67082 (n) not of moles of BF, = W1 = 6.79 = 0.1 co given massa W = 2.90 co molar massa m2 = 28 no" of moles of 2039 = 2.90 +6103 28 Total moles anth= 0.1 +0.103=0.203. hof ñ ool - auart -0-4926 (♡ moles braction of BF Bet no 0.203 neo 0.103 -0.507 0.203 (1) 03 neo . co-, not theo mole fraction of (10) 0.203x8.0821+278159 -chith RT p "Total 10 - 4.593 20.4593 atm. Protal = To Exp = 0.4926 0.4593 = 0.2262 atm BF = 2 x P & Total (10) parsial pressure of (1) Partial pressure of co=XX Porotan 0.50788.4593=0.2328 aly