Question

How many moles of FeS2 are required to produce 32 g of So2

Answer 1

To produce 32 g of SO2, approximately 0.250 moles of FeS2 are required. The calculation utilizes the molar mass of SO2 and the stoichiometry of the reaction.

Step-by-step explanation:

To find out how many moles of FeS2 are required to produce 32 g of SO2, we first need the balanced chemical equation for the conversion. The reaction producing sulfur dioxide from iron(II) disulfide is:

4FeS2 + 11O2 → 2Fe2O3 + 8SO2

Next, we need to calculate the molar mass of SO2, which is 32.065 g/mol for sulfur plus 2 × 15.999 g/mol for oxygen, totaling 64.063 g/mol.

Now, we can use stoichiometry:

1. Convert grams of SO2 to moles using its molar mass: (32 g SO2) × (1 mol SO2/64.063 g SO2) = 0.499 moles of SO2.
2. Use the mole ratio from the balanced equation to find moles of FeS2: (0.499 moles SO2) × (1 mol FeS2/2 moles SO2) = 0.2495 moles of FeS2.

We would need approximately 0.250 moles of FeS2 (rounded to three significant figures) to produce 32 g of SO2.

Answer 2

So, the right answer is. No. of moles of FeS₂ = 0.25 mole. Explanation: From the balanced. 4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2.

Step-by-step explanation: