Answer:
124.24 g of S₈.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
8SO₂ + 16H₂S —> 3S₈ + 16H₂O
Next, we shall determine the masses of SO₂ and H₂S that reacted and the mass of S₈ produced from the balanced equation.
This is illustrated below:
Molar mass of SO₂ = 32 + (16×2)
= 32 + 32 = 64 g/mol
Mass of SO₂ from the balanced equation = 8 × 64 = 512 g
Molar mass of H₂S = (2×1) + 32
= 2 + 32 = 34 g/mol
Mass of H₂S from the balanced equation = 16 × 34 = 544 g
Molar mass of S₈ = 32 × 8 = 256 g/mol
Mass of S₈ from the balanced equation = 3 × 256 = 768 g
Thus,
From the balanced equation above,
512 g of SO₂ reacted with 544 g of H₂S to produce 768 g of S₈.
Next, we shall determine the limiting reactant. This can be obtained as follow:
From the balanced equation above,
512 g of SO₂ reacted with 544 g of H₂S.
Therefore, 88 g of SO₂ will react with = (88 × 544) / 512 = 93.5 g of H₂S.
From the calculation made above, we can see that it will take a higher mass (i.e 93.5 g) than what was given (i.e 88g) of H₂S to react completely with 88 g of SO₂.
Therefore, H₂S is the limiting reactant and SO₂ is the excess reactant.
Finally, we shall determine the maximum mass of S₈ produced from the reaction.
In this case, we shall use the limiting reactant because it will give the maximum yield of S₈ since all of it is consumed in the reaction.
The limiting reactant is H₂S and the maximum mass of S₈ produced can be obtained as follow:
From the balanced equation above,
544 g of H₂S reacted to produce 768 g of S₈.
Therefore, 88 g of H₂S will react to produce = (88 × 768) / 544 = 124.24 g of S₈.
Therefore, the maximum mass of S₈ produced from the reaction is 124.24 g.
