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A. 650 moles of sulphur.

B. 30 g of FeS₂

Explanation:

The balanced equation for the reaction is given below:

Fe + 2S —> FeS₂

From the balanced equation above,

1 mole of Fe reacted with 2 moles of S to produce 1 mole of FeS₂.

A. Determination of the mole of sulphur needed for the reaction.

From the balanced equation above,

2 moles of S reacted to produce 1 mole of FeS₂.

Therefore, Xmol of S will react to produce 325 moles of FeS₂ i.e

Xmol of S = 2 × 325

Xmol of S = 650 moles

Thus, 650 moles of sulphur are needed for the reaction.

B. Determination of the mass of FeS₂ produced by the reaction of 0.5 mole of sulphur.

From the balanced equation above,

2 moles of S reacted to produce 1 mole of FeS₂.

Therefore, 0.5 mole of S will react to produce = (0.5 × 1)/2 = 0.25 mole of FeS₂.

Finally, we shall determine the mass of 0.25 mole of FeS₂. This can be obtained as follow:

Mole of FeS₂ = 0.25 mole

Molar mass of FeS₂ = 56 + (32×2)

= 56 + 64

= 120 g/mol

Mass of FeS₂ =?

Mass = mole × molar mass

Mass of FeS₂ = 0.25 × 120

Mass of FeS₂ = 30 g

Thus, 30 g of FeS₂ were obtained from the reaction.