Question

Mining companies use this reaction to obtain iron from iron ore: Fe2O3 (s) + 3CO(g) → 2Fe(s) + 3CO2(g) The reaction of 167 g of Fe2O3 with 84.0 g of CO produces 75.0 g of Fe.

Calculate the theoretical yield of solid iron?
What is the reagent in the access of the reactant?

Answer 1

The theoretical yield of solid iron is 116.6g.

Step-by-step explanation:

In the given reaction, Fe2O3 (s) + 3CO(g) → 2Fe(s) + 3CO2(g), the stoichiometry tells us that 1 mole of Fe2O3 reacts with 3 moles of CO to produce 2 moles of Fe. To calculate the theoretical yield of solid iron, we need to find the number of moles of Fe2O3 and CO reactants. From the given masses, we can convert them to moles using the molar mass.

For Fe2O3: 167 g Fe2O3 x (1 mol Fe2O3 / 159.70 g Fe2O3) = 1.048 moles

For CO: 84.0 g CO x (1 mol CO / 28.01 g CO) = 3.00 moles

Based on the stoichiometry, the reactant ratio is 1:3 (1 mole of Fe2O3 reacts with 3 moles of CO).

Therefore, we can determine the limiting reactant by comparing the mole ratios. Since we have 1.048 moles of Fe2O3 and 3.00 moles of CO, the limiting reactant is Fe2O3.

Now, we can calculate the theoretical yield of solid iron using the mole ratio. 1.048 moles Fe2O3 x (2 moles Fe / 1 mole Fe2O3) = 2.096 moles Fe

To convert the moles of Fe to grams, we multiply by the molar mass of Fe: 2.096 moles x (55.85 g / 1 mole) = 116.6 g (rounded to 2 decimal places)