Question
How many moles of nitrogen monoxide are produced when 1 mole of ammonia reacts with 2 moles of oxygen?
2NH3(g) + O2(g) -----> 2NO(g) + 3H2(g)
2NH3(g) + O2(g) -----> 2NO(g) + 3H2(g)
Answers
GPT-4o mini
To determine how many moles of nitrogen monoxide (NO) are produced when 1 mole of ammonia (NH₃) reacts with 2 moles of oxygen (O₂), we can refer to the balanced chemical equation:
\[ 2 \text{NH}_3(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g) + 3 \text{H}_2(g) \]
From the equation, we can see that:
- 2 moles of NH₃ produce 2 moles of NO.
This means that for every 2 moles of NH₃ consumed, 2 moles of NO are produced.
If you are starting with 1 mole of NH₃, you can set up a proportion based on the balanced equation:
\[
\frac{2 \text{ moles NO}}{2 \text{ moles NH}_3} = \frac{x \text{ moles NO}}{1 \text{ mole NH}_3}
\]
From this proportion, we can find that:
\[
x = 1 \text{ mole NO}
\]
Thus, when 1 mole of ammonia reacts with 2 moles of oxygen, 1 mole of nitrogen monoxide (NO) is produced.
\[ 2 \text{NH}_3(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g) + 3 \text{H}_2(g) \]
From the equation, we can see that:
- 2 moles of NH₃ produce 2 moles of NO.
This means that for every 2 moles of NH₃ consumed, 2 moles of NO are produced.
If you are starting with 1 mole of NH₃, you can set up a proportion based on the balanced equation:
\[
\frac{2 \text{ moles NO}}{2 \text{ moles NH}_3} = \frac{x \text{ moles NO}}{1 \text{ mole NH}_3}
\]
From this proportion, we can find that:
\[
x = 1 \text{ mole NO}
\]
Thus, when 1 mole of ammonia reacts with 2 moles of oxygen, 1 mole of nitrogen monoxide (NO) is produced.