Final answer:
The limiting reactant is Fe2O3, with the theoretical yield of Fe being 7.07 g and the percent yield being approximately 86.3%.
Step-by-step explanation:
To determine which substance is the limiting reactant in the reaction of Fe2O3 with CO, you must compare the mole ratio of the reactants to the coefficients in the balanced chemical equation Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g). First, calculate the number of moles of each reactant. The molar mass of Fe2O3 is 159.7 g/mol, which gives us 0.0633 moles of Fe2O3. The molar mass of CO is 28.01 g/mol, which gives us about 0.696 moles of CO. Using the mole ratio from the balanced equation, we find that all of the Fe2O3 reacts, but there will be excess CO; therefore, Fe2O3 is the limiting reactant.
The theoretical yield of Fe can be found by using the stoichiometry of the balanced equation. With 0.0633 moles of Fe2O3, we can produce twice that amount in moles of Fe, which is 0.1266 moles of Fe. Multiplying this by the molar mass of Fe (55.85 g/mol), we get the theoretical yield of Fe to be approximately 7.07 g.
The percent yield of Fe is calculated using the actual yield and the theoretical yield. To find the percent yield, divide the actual yield (6.10 g) by the theoretical yield (7.07 g) and multiply by 100, which results in a percent yield of approximately 86.3%.