Consider the following reaction:

4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g)

If 4.0 mol of FeS2 and 4.0 mol of O2 react, how many moles of Fe2O3(s) are produced?

Question

Consider the following reaction:

4FeS2(s) + 11O2(g)  →  2Fe2O3(s) + 8SO2(g)

If 4.0 mol of FeS2 and 4.0 mol of O2 react, how many moles of Fe2O3(s) are produced?

BlackTom AI · Accepted Answer

Analyzing the reaction 4FeS2 + 11O2 -> 2Fe2O3 + 8SO2, we first identify the stoichiometric relationships: 4 moles of FeS2 require 11 moles of O2 to yield 2 moles of Fe2O3 and 8 moles of SO2.

Option 1: 11 mol
This would imply producing 2Fe2O3 from 11 moles of O2, but we only have 4.0 moles of O2. The ratio shows that 11 moles of O2 are needed for 2 moles of Fe2O3, so using just 4.0 moles O2 would yield far less Fe2O3. Therefore, 11 mol is not feasible given the reactant amounts.

Option 2: 2.0 mol
This corresponds to producing 2.0 moles of Fe2O3. The reaction shows that 2 Fe2O3 are produced per 11 O2 consumed. To produce 2.0 mol Fe2O3, you would need (11/2) × 2.0 = 11.0 moles of O2. Since only 4.0 moles of O2 are available, this option cannot occur. It overestimates the O2 required for the stated Fe2O3 amount.

Option 3: 0.73 mol
This aligns with the limiting-reactant calculation. Oxygen is the limiting reagent because 4.0 mol O2 is far less than the 11.0 moles of O2 required to use up 4.0 moles of FeS2 completely. From the stoichiometry, 11 O2 produce 2 Fe2O3, so 4.0 O2 would produce (2/11) × 4.0 = 8/11 ≈ 0.727 mol Fe2O3, which rounds to 0.73 mol. This is consistent with the limiting reactant principle.

Option 4: 22 mol
Producing 22 moles of Fe2O3 would require a proportionally enormous amount of O2 according to the 11 O2 : 2 Fe2O3 ratio. Specifically, to obtain 22 moles Fe2O3 you’d need (11/2) × 22 = 121 moles of O2. Since only 4.0 moles O2 are present, this option is impossible.

Option 5: 2.9 mol
Calculating from the same ratio, to get 2.9 mol Fe2O3 you would require O2 = (11/2) × 2.9 = 15.95 moles of O2, far exceeding the available 4.0 moles. Therefore this option cannot be correct given the reactant amounts.

Consider the following reaction: 4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g) If 4.0 mol of FeS2 and 4.0 mol of O2 react, how many moles of Fe2O3(s) are produced?

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