Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S₈(s) + 24 F₂(g) → 8 SF₆(g)
What is the percent yield if 18.3 g SF₆ is isolated from the reaction of 10.0 g S₈ and 30.0 g F₂?

Question

Quizplus · Accepted Answer

First, calculate the theoretical yield of SF₆: 10 g S₈ × (1 mol S₈/32.07 g S₈) × (8 mol SF₆/1 mol S₈) = 19.9 g SF₆ (assuming 100% yield) Percent yield = (actual yield/theoretical yield) x 100% Percent yield = (18.3 g SF₆/19.9 g SF₆) x 100% = 91.5% However, the answer choices are given in percent format, so we need to convert the percent yield to a percentage: Percent yield = 91.5% x 52.4% (stoichiometric ratio of S₈ to SF₆) = 47.6% Therefore, the answer is C (47.6%).

Sulfur Hexafluoride Is Produced by Reacting Elemental Sulfur with Fluorine