Question

Aluminum reacts with chlorine to form aluminum chloride. The equation for this
reaction is 2 Al(s) + 3 Cl2(g) 2 AlCl3(s). What is the percentage yield for a reaction in which 33.5 g of aluminum is reacted with excess chlorine to produce 164.5 g of aluminum chloride?

Answer 1

Answer:

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Answer 2

Given:

Mass of Al = 33.5 gm

Actual yield, i.e., Mass of AlCl₃ = 164.5 gm

To Find:

The percentage yield of the given reaction.

Calculation:

- According to the given reaction:

2 Al (s) + 3 Cl₂ (g) → 2 AlCl₃ (s)

54 gm of Aluminium (Al) reacts forms Aluminium Chloride (AlCl₃) = 267 gm

⇒ 33.5 gm of Aluminium will produce the amount of Aluminium Chloride = (267/54) × 33.5

⇒ Theoretical yield = 165.64 gm

- Percentage yield = (Actual yield / theoretical yield) × 100

⇒ Percentage yield = (164.5/165.64) × 100

⇒ Percentage yield = 99.31 %

- So the % yield for the given reaction is 99.31 %.