Question

You already saw that 1.00 g of Al should yield 3.53 g of copper for the reaction below. 3CuCl2(aq) + 2Al(s)⟶ 2AlCl3(aq) + 3Cu(s) However, impurities and errors can occur easily. Suppose that only 2.86 g of copper is produced. What is the percent yield of the reaction

Answer 1

Answer:

81 %

Explanation:

Percent yield = actual yield/ theoretical yield x 100

Percent yield is the ratio of the actual yield to the theoretical yield  

Given,  

Actual yield = 2.86 g

Theoretical yield = 3.53 g  

Percent yield =$\frac{2.86 g x 100}{3.53 g}$= 81 %

Answer 2

Answer:

81.02%

Explanation:

$3CuCl_{2}_{(aq)}+2Al_{(s)} \longrightarrow 2AlCl_{3}_{(aq)} +3Cu_{(s)}$

We know that 3.53 grams of Cu should be produced, but we get 2.86 grams of this compound.

The yield of a reaction is the amount of product obtained in a chemical reaction

To know the performance of a reaction in percentage we use the following formula

$\%= \frac{mass obtained}{mass calculated} .100\%\\\%=\frac{2.86}{3.53}.100\%\\\%=81.02\%$