Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s) A) 61.03% B) 28.65% C) 57.30% D) 20.02% E) 81.93%

Question

Quizplus · Accepted Answer

The theoretical yield of Fe is calculated from the stoichiometry of the reaction. The molar mass of Fe2O3 is 159.7 g/mol, and 50.00 g corresponds to 0.313 mol. This produces 0.626 mol of Fe (since 1 mol Fe2O3 produces 2 mol Fe), which is 34.96 g of Fe. The percent yield is (28.65 g / 34.96 g) * 100% = 81.93%.

Determine the Percent Yield of a Reaction That Produces 28