Question

please make sure the answer is correct

A 7.00 L tank at 28.8 °C is filled with 8.41 g of sulfur hexafluoride gas and 14.6 g of dinitrogen difluoride 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 sulfur hexafluoride partial pressure mole fraction dinitrogen difuoride partial pressure Total pressure in tank:

Answer 1

The ans is given below

Quel - given & volume of tank = 0 TL Temp = 20.00 - 20.0+ 213 - (SFC) Sulfor hexafluoride - 146j o nig (M46) dinitrogen difloonide - 14-69 mol. mars of SFO = 146.06 glonus mol mans of Nafe - 66.01 grmol mol og stolenou 196.06 = 0.05950 mole MF w 14.6 66.06 I Mrafy = 0.221 Nr = nsat NH2E2 = 0.05750+ 0 221 [Mt = 0.2106

mole fraction of SF= mol Total mole 0:0 5750 0-2106 (R = 0.2067 m mole fraction of N2F2 = mole of Total Mare mole 0.221 0.2786 Arar -0.1933. Total Pressure PV=nRTs Prx (72) = 0.2186 x 0. 0820 X 301.8 (Latm mortist) & K mol 0.27064 0.0020 X301.8 am Pr = P = 0.9849 alm

Pantial Pressure of any any gan Af= x P 7 Partial Pressure For SFO :- x = 0.2067 Pr = 0.9849 Ise 0 2061 X 0.9899 TOE = 0.20357 am For Haf - 2 0 1933 P = 0.9049 Pript = 0.1933 09849 | Pret = 0.1813 Conclusion mole 0.05750 SF6 partial pressure : 0.20 351 am mole fraction – 0.2067 mole 0.92) M2 F2 mole fraction - 0.7933 fartial pressure - 0.71813 ahm Total Pressure 0.9849