Question

A 9.00 L tank at -10.2 °C is filled with 15.9 g of sulfur tetrafluoride gas and 2.60 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas mole fraction 1 x s ? sulfur tetrafluoride boron trifluoride

Answer 1

Mole fraction of a ratio of number the total number component of moles of mole is defined as the of that component to present. - No. of moles – & Given Moss Molar Mass (1) Sulfur Tetrafluoride (stu). Molar Mass & 32 + 4x 19 - 108 g/mol Given Moss - is a gm. Moles of sty: 15.9 - 0. 147 108 Since three significant figures in 15.9. (11) Baron Trifluord (BF3) Molar Mass - 11+ 3x 19. - 68 g/mol Given mass = 2.60 Moles of BF3 - 2.60 Three signifactfigure – 0.0382 67 Total Moles = 0.147 + 0.0382 - 0.185 - Mole Fraction of sty= 0.147 - 0.794 Ans 0.185 Mole fraction of Br₂ = 0.0382 = 0.206 Ans. 0.185

Solution is provided in the Image.