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

81.02%

Step-by-step 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

`\%= (mass obtained)/(mass calculated) .100\%\\\%=(2.86)/(3.53).100\%\\\%=81.02\%`

Answer 2

81 %

Step-by-step 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 =
`(2.86 g x 100)/(3.53 g)`= 81 %