When [tex]$NH_3$[/tex] is prepared from [tex]$28 \, \text{g} \, N_2$[/tex] and excess [tex]$H_2$[/tex], the theoretical yield of [tex]$NH_3$[/tex] is [tex]34 \, \text{g}$[/tex]. When this reaction is carried out in a given experiment, only [tex]$30 \, \text{g}$[/tex] is produced.

What is the percentage yield?

To find the percentage yield of a chemical reaction, you can use the formula:

[tex]\[
\text{Percentage yield} = \left(\frac{\text{Actual yield}}{\text{Theoretical yield}}\right) \times 100
\][/tex]

Here are the given values from the problem:

1. Theoretical yield of [tex]$ \text{NH}_3 $[/tex]: 34 grams
2. Actual yield of [tex]$ \text{NH}_3 $[/tex]: 30 grams

Using the formula, plug in the given values:

[tex]\[
\text{Percentage yield} = \left(\frac{30 \, \text{grams}}{34 \, \text{grams}}\right) \times 100
\][/tex]

Calculate the division first:

[tex]\[
\frac{30}{34} \approx 0.8824
\][/tex]

Next, multiply by 100 to convert it into a percentage:

[tex]\[
0.8824 \times 100 = 88.24
\][/tex]

Therefore, the percentage yield of the given reaction is approximately 88.24%.