Question

Fifty grams of Chlorine reacts completely with Phosphorus obtaining ninety grams of the product.

P4(s) + Cl2(g) = PCl3(l) 

a. Balance the chemical equation;

b. Identify the limiting reactant and the excess reactant if applicable;

c. Compute for the theoretical yield; d. Determine the percent yield of the reaction;

e. Calculate the percent error and

f. Compute for the excess amount of the excess reactant if applicable.

g. Show the complete solutions for your answers in a separate paper.

Answer 1

Balanced :

P4 + 6Cl₂ → 4PCl₃

Moles of Cl₂ $= \frac{50}{35}=1.43moles$

Moles of product$(PCl_3)=\frac{4×1.43}{6}=0.95 moles$

Limiting reactant is $PCl_3$ and the excess reactant is $Cl_3$

Theoretical yield $= 0.95× 137= 130.15 g$

Percent yield $= \frac { 90}{130.15}×100=69.15$%