Question
How many moles of nitrogen monoxide are produced when 1 mole of ammonia reacts with 2 moles of oxygen? Identify the limiting reactant.
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 in the reaction between ammonia (NH₃) and oxygen (O₂), we can analyze the balanced chemical equation given:
\[
2 \text{NH}_3(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g) + 3 \text{H}_2(g)
\]
From the balanced equation, we can summarize the stoichiometric relationships:
- 2 moles of NH₃ react with 1 mole of O₂ to produce 2 moles of NO.
### Step 1: Determine the limiting reactant
You have 1 mole of NH₃ and 2 moles of O₂. Let's consider how much of each reactant is required to react completely.
From the stoichiometry of the balanced equation:
- For 1 mole of NH₃, we need \(\frac{1}{2} = 0.5\) moles of O₂ (since 2 NH₃ react with 1 O₂).
- You have 2 moles of O₂ available.
### Step 2: Identify the limiting reactant
- NH₃ is the limiting reactant because it can only react with 0.5 moles of O₂ (and you have more than enough O₂: 2 moles).
### Step 3: Calculate how many moles of NO are produced
From the stoichiometry in the equation:
- 2 moles of NH₃ produce 2 moles of NO.
- Therefore, 1 mole of NH₃ will produce 1 mole of NO (because it's a 1:1 ratio in terms of NH₃ to NO).
Thus, since you have 1 mole of NH₃, it will produce:
\[
1 \text{ mole of NO}
\]
### Conclusion
- The limiting reactant is ammonia (NH₃).
- The reaction produces 1 mole of nitrogen monoxide (NO).
\[
2 \text{NH}_3(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g) + 3 \text{H}_2(g)
\]
From the balanced equation, we can summarize the stoichiometric relationships:
- 2 moles of NH₃ react with 1 mole of O₂ to produce 2 moles of NO.
### Step 1: Determine the limiting reactant
You have 1 mole of NH₃ and 2 moles of O₂. Let's consider how much of each reactant is required to react completely.
From the stoichiometry of the balanced equation:
- For 1 mole of NH₃, we need \(\frac{1}{2} = 0.5\) moles of O₂ (since 2 NH₃ react with 1 O₂).
- You have 2 moles of O₂ available.
### Step 2: Identify the limiting reactant
- NH₃ is the limiting reactant because it can only react with 0.5 moles of O₂ (and you have more than enough O₂: 2 moles).
### Step 3: Calculate how many moles of NO are produced
From the stoichiometry in the equation:
- 2 moles of NH₃ produce 2 moles of NO.
- Therefore, 1 mole of NH₃ will produce 1 mole of NO (because it's a 1:1 ratio in terms of NH₃ to NO).
Thus, since you have 1 mole of NH₃, it will produce:
\[
1 \text{ mole of NO}
\]
### Conclusion
- The limiting reactant is ammonia (NH₃).
- The reaction produces 1 mole of nitrogen monoxide (NO).