Question

7. Disulfur dichloride can be made by reacting chlorine gas with molten sulfur. What is the yield of S2Cl2 expected in a laboratory experiment from the reaction of 10.0 g S8 and 6.00 g Cl2? What if the reaction consistently gives an 85.0 % yield?

Answer 1

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) =

11.4g of S₂Cl₂ is the expected yield

If you produce just the 85.0% of yield, mass of S₂Cl₂ is:

11.4g ₓ 85% =

9.69g of S₂Cl₂