Answer:
A. 650 moles of sulphur.
B. 30 g of FeS₂
Step-by-step 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.