Question

please make sure answers are correct, I've gotten a lot of these back that are wrong & its frustrating

A 9.00 L tank at 13.4 °C is filled with 18,6 g of sulfur tetrafluoride gas and 3.45 g of boron trifluoride gas. You can assume both gases behave as ideal gase 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 tetrafluoride partial pressure x 5 ? mole fraction boron trifluoride partial pressure Total pressure in tank

Answer 1

Moles of SFu = 186 g = 00172 mol 108.67 g mal! ..u u BFz = 30459/67082 gmol = Total number of males niotal = (0.172+0.0509) mal = 0.2229 mol - Province = MORT (002299mal) x (0.082 L arm mol-k-1) x (1304+ 273)k (9.00 e) = 0.581 arm

00172 mol Male fraction of SFu NgFu = 0.2229 mol = 0.771 (Ang) o u a BF XBF2 = 1- 20SF = -0.7H = 0.228 (Ana) partial pressure of SF4 =gg Fu X Prot = 600771JX (80581) alm = 00448 afm (Ams) u au BFF F = BET Prot = (0228.x 60.581.) alm = 00132 abr (Am)