Question

Phosphorous trichloride (PCl3) is produced
from the reaction of white phosphorous (P4)
and chlorine:
P4(s) + 6 Cl2(g) → 4 PCl3(g).
A sample of PCl3 of mass 262.6 g was collected
from the reaction of 79.12 g of P4 with excess
chlorine. What is the percentage yield of the
reaction?
Answer in units of %.

Answer 1

The percentage yield obtained from the given reaction above is 74.8%

Balanced equation

P₄ + 6Cl₂ → 4PCl₃

Molar mass of P₄ = 31 × 4 = 124 g/mol

Mass of P₄ from the balanced equation = 1 × 124 = 124 g

Molar mass of PCl₃ = 31 + (35.5×3) = 137.5 g/mol

Mass of PCl₃ from the balanced equation = 4 × 137.5 = 550 g

SUMMARY

From the balanced equation above,

124 g of P₄ reacted to produce 550 g of PCl₃

How to determine the theoretical yield

From the balanced equation above,

124 g of P₄ reacted to produce 550 g of PCl₃

Therefore,

79.12 g of P₄ will react to produce = (79.12  × 550) / 124 = 350.9 g of PCl₃

How to determine the percentage yield

• Actual yield of PCl₃ = 262.6 g
• Theoretical yield of PCl₃ = 350.9 g

• Percentage yield =?

Percentage yield = (Actual /Theoretical) × 100

Percentage yield = (262.6 / 350.9) × 100

Percentage yield = 74.8%

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