Question

When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here:4Al+3O2→2Al2O3In Part A, we saw that the theoretical yield of aluminum oxide is 0.700 mol . Calculate the percent yield if the actual yield of aluminum oxide is 0.532 mol .

Answer 1

Answer:

The percent yield is 76%.

Explanation:

The information from the exercise is:

- Theoretical yield: 0.700 mol

- Actual yield: 0.532 mol

To calculate the percent yield, we have to replace the values of theoretical yield and actual yield in the percent yield formula:

$\begin{gathered} \text{ Percent yield}=\frac{\text{ Actual yield}}{\text{ Theoretical yield}}*100\% \\ \text{ Percent yield}=\frac{0.532}{0.700}*100\% \\ \text{ Percent yield}=76\% \end{gathered}$

So, the percent yield is 76%.