Question

The percentage yield for the reaction

Answer 1

Answer:

92.87 g.

Explanation:

∵ The percentage yield = (actual yield/theoretical yield)*100.

• We need to calculate the theoretical yield:

From the balanced reaction:

PCl₃ + Cl₂ → PCl₅,

It is clear that 1 mol of PCl₃ reacts with 1 mol of Cl₂ to produce 1 mol of PCl₅.

• We need to calculate the no. of moles of 73.7 g PCl₃:

n = mass/molar mass = (73.7 g)/(137.33 g/mol) = 0.536 mol.

Using cross multiplication:

1 mol of PCl₃ produce  → 1 mol of PCl₅, from stichiometry.

∴ 0.536 mol of PCl₃ produce  → 0.536 mol of PCl₅.

∴ The mass of PCl₅ (theoretical yield) = (no. of moles) * (molar mass) = (0.536 mol)*(208.24 g/mol) = 111.62 g.

∵ The percentage yield = (actual yield/theoretical yield)*100.

The percentage yield = 83.2%, theoretical yield = 111.62 g.

∴ The actual yield of PCl₅ = (The percentage yield)(theoretical yield)/100 = (83.2%)(111.62 g)/100 = 92.87 g.