Question

Iron (IV) sulfide + Oxygen gas → Iron (III) oxide + sulfur dioxide

4FeS2 + 1102 → 2Fe2O3 + 8SO2

Mole to Mole Problem:
Using the chemical equation above, assume that 14.56 moles of iron(IV) sulfide are reacted. How moles of Iron(III) oxide will form.

Answer 1

Step-by-step explanation:

From the balanced chemical equation, we see that 4 moles of FeS2 react with 11 moles of O2 to form 2 moles of Fe2O3.

So, for every 4 moles of FeS2, we get 2 moles of Fe2O3.

To find the moles of Fe2O3 formed from 14.56 moles of FeS2, we can use a proportion:

4 moles FeS2 / 2 moles Fe2O3 = 14.56 moles FeS2 / x moles Fe2O3

Cross-multiplying, we get:

4 moles FeS2 * x moles Fe2O3 = 2 moles Fe2O3 * 14.56 moles FeS2

Simplifying, we get:

x moles Fe2O3 = (2 moles Fe2O3 * 14.56 moles FeS2) / 4 moles FeS2

x moles Fe2O3 = 7.28 moles Fe2O3

Therefore, 7.28 moles of Fe2O3 will be formed when 14.56 moles of FeS2 reacts.