Answer:
11.4g of Sâ‚‚Clâ‚‚ is the expected yield
9.69g of Sâ‚‚Clâ‚‚ 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
Clâ‚‚ (Molar mass: 70.9g/mol): 6.00g â‚“ (1mol / 70.9g) = 0.0846 moles Clâ‚‚
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 Clâ‚‚ produce 4 moles of Sâ‚‚Clâ‚‚. 0.0846 moles of Clâ‚‚ produce, in theory, 0.0846 moles of Sâ‚‚Clâ‚‚ (Molar mass: 135.04g/mol). In mass:
0.0846 moles Sâ‚‚Clâ‚‚ â‚“ (135.04g/mol) =
If you produce just the 85.0% of yield, mass of Sâ‚‚Clâ‚‚ is:
11.4g â‚“ 85% =
