Question

Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 21.8 g iron (Fe) is reacted with 16.2 g oxygen (O2). Step 1: What is the limiting reactant? Step 2: Calculate the theoretical yield of iron (fe) Stepp 3: The reaction produces 5.52 g Fe2⁢O3. What is the percent yield of the reaction?

Answer 1

The limiting reactant in a reaction between Fe and O2, compare the moles of each reactant. Calculate the theoretical yield of Fe using the mole ratio in the balanced equation. To find the percent yield, divide the actual yield by the theoretical yield and multiply by 100%.

Step-by-step explanation:

Step 1: To determine the limiting reactant, we need to compare the moles of Fe and O2 present in the given amounts. We can calculate the moles of Fe using its molar mass (55.85 g/mol) and the given mass of Fe (21.8 g). Similarly, we can calculate the moles of O2 using its molar mass (32 g/mol) and the given mass of O2 (16.2 g). The mole ratio of Fe to O2 in the balanced equation is 4:3, so we can compare the moles of Fe and O2 using this ratio.

Step 2: The limiting reactant is the one that produces the fewer moles of the product. In this case, Fe is the limiting reactant because it produces fewer moles of Fe2O3 than O2. To calculate the theoretical yield of Fe, we can use the mole ratio of Fe to Fe2O3 in the balanced equation (4:2). We multiply the moles of Fe by this ratio and then convert the moles of Fe2O3 to grams using its molar mass (159.69 g/mol).

Step 3: The percent yield can be calculated using the formula: (actual yield / theoretical yield) x 100%. In this case, the actual yield of Fe2O3 is given as 5.52 g. We divide this by the theoretical yield of Fe2O3 calculated in Step 2 and then multiply by 100% to find the percent yield.