IDNLearn.com is the perfect place to get answers, share knowledge, and learn new things. Explore a wide array of topics and find reliable answers from our experienced community members.
Sagot :
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%.
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%.
Your participation means a lot to us. Keep sharing information and solutions. This community grows thanks to the amazing contributions from members like you. Your questions deserve reliable answers. Thanks for visiting IDNLearn.com, and see you again soon for more helpful information.