Answer:
11.4g of S₂Cl₂ is the expected yield
9.69g of S₂Cl₂ are produced with a 85% yield
Explanation:
The reaction of sulfur S₈ with Cl₂ to produce S₂Cl₂ is:
S₈ + 4Cl₂ → 4S₂Cl₂
Where 1 mole of sulfur reacts with four moles of chlorine to produce four moles of disulfur dichloride.
To find the limiting reactant you need to convert mass of each reactant to moles using its molar mass, thus:
S₈ (Molar mass: 256.52g/mol): 10.0g ₓ (1mol / 256.52g) = 0.0390 moles S₈
Cl₂ (Molar mass: 70.9g/mol): 6.00g ₓ (1mol / 70.9g) = 0.0846 moles Cl₂
For a complete reaction of 0.0390 moles of sulfur, there are necessaries:
0.0390 mol S₈ ₓ (4 mol Cl₂ / 1 mol S₈) = 0.156 moles Cl₂. As you have just 0.0846 moles of chlorine, Cl₂ is the limiting reactant.
As 4 moles of Cl₂ produce 4 moles of S₂Cl₂. 0.0846 moles of Cl₂ produce, in theory, 0.0846 moles of S₂Cl₂ (Molar mass: 135.04g/mol). In mass:
0.0846 moles S₂Cl₂ ₓ (135.04g/mol) =
If you produce just the 85.0% of yield, mass of S₂Cl₂ is:
11.4g ₓ 85% =
