To determine the percent yield of nitrogen dioxide ([tex]\(\text{NO}_2\)[/tex]), we can follow these steps:
1. Write down the balanced chemical equation:
[tex]\[
2 \text{NO} + \text{O}_2 \rightarrow 2 \text{NO}_2
\][/tex]
2. Given information:
- Nitrogen oxide ([tex]\(\text{NO}\)[/tex]) consumed: 1500 kg
- Nitrogen dioxide ([tex]\(\text{NO}_2\)[/tex]) produced: 1500 kg
3. Determine the molar ratio:
- From the balanced equation, 2 moles of [tex]\(\text{NO}\)[/tex] produce 2 moles of [tex]\(\text{NO}_2\)[/tex]. This indicates a 1:1 molar ratio.
4. Theoretical yield:
- Since the reaction has a 1:1 molar ratio and we are starting with equal masses, the theoretical yield of [tex]\(\text{NO}_2\)[/tex] would be 1500 kg, the same as the amount of [tex]\(\text{NO}\)[/tex] consumed.
5. Calculate the percent yield:
- Use the formula for percent yield:
[tex]\[
\% \text{ Yield} = \frac{\text{Actual yield}}{\text{Theoretical yield}} \times 100
\][/tex]
- Actual yield of [tex]\(\text{NO}_2\)[/tex]: 1500 kg
- Theoretical yield of [tex]\(\text{NO}_2\)[/tex]: 1500 kg
Plugging in the values:
[tex]\[
\% \text{ Yield} = \frac{1500 \text{ kg}}{1500 \text{ kg}} \times 100 = 100\%
\][/tex]
Therefore, the percent yield of nitrogen dioxide in this reaction is [tex]\(100\%\)[/tex]. This indicates the actual yield equals the theoretical yield, and no loss or inefficiency in the process is detected. The correct answer choice is not listed; hence the yield is 100%.
