Question

If 107 g of iron reacts with excess oxygen gas to produce 10.2 g of solid iron(III) oxide (molar mass = 156.69 g/mol) according to the balanced equation:

4Fe(s)+3O₂​(g)→2Fe₂​O₃​(s)

What is the percent yield of this reaction?

Answer 1

To calculate the percent yield of a reaction, we compare the actual and theoretical yields and calculate the percentage.

Step-by-step explanation:

To calculate the percent yield of a reaction, we need to compare the actual yield (the amount of product obtained experimentally) to the theoretical yield (the amount of product that should be obtained according to stoichiometry ).

First, we calculate the theoretical yield of Fe2O3 by using the given mass of Fe and the stoichiometric mole ratio between Fe and Fe2O3. The molar mass of Fe is 55.85 g/mol. Theoretical yield of Fe2O3 = (mass of Fe) × (1 mol Fe2O3 / 4 mol Fe) × (molar mass Fe2O3)

Then, we calculate the percent yield by using the actual yield and the theoretical yield: Percent yield = (actual yield / theoretical yield) × 100%. Substituting the given mass of Fe2O3 and the mass of Fe obtained, we can calculate the percent yield of this reaction.