Question
2NO + 1O2 = 2NO2
products: 4NO2
leftovers: 0NO, 3O2
what are the numbers of reactants?
products: 4NO2
leftovers: 0NO, 3O2
what are the numbers of reactants?
Answers
GPT-4o mini
To determine the numbers of reactants, we first need to analyze the given chemical reaction:
\[ 2 \text{NO} + \text{O}_2 \rightarrow 2 \text{NO}_2 \]
From this equation, we see that 2 moles of NO (nitric oxide) react with 1 mole of O₂ (oxygen gas) to produce 2 moles of NO₂ (nitrogen dioxide).
You provided that the products are 4 moles of NO₂ and that there are leftovers of 0 moles of NO and 3 moles of O₂.
### Understanding the Stoichiometry:
1. Since you produced 4 moles of NO₂, we can determine how many moles of reactants were needed based on the stoichiometry of the reaction.
- According to the balanced equation, 2 moles of NO yield 2 moles of NO₂. Therefore, for 4 moles of NO₂:
\[ 4 \text{NO}_2 \text{ would require } 4 \text{NO} \text{ (since } 2 \text{NO} \rightarrow 2 \text{NO}_2 \text{)} \]
2. For each mole of O₂ used, 2 moles of NO are needed to produce 2 moles of NO₂. If we produced 4 moles of NO₂, we already calculated that you would need 4 moles of NO, which would essentially mean:
- Using 2 moles of O₂ is necessary for the reaction; this is because:
\[ 2 \text{NO} + 1 \text{O}_2 \rightarrow 2 \text{NO}_2 \]
- To produce 4 moles of NO₂, you would need to double the amount of both reactants:
\[ 4 \text{NO} + 2 \text{O}_2 \rightarrow 4 \text{NO}_2 \]
### Conclusion:
Thus, in terms of the reactants based on the products produced (4 moles of NO₂) and the leftovers (0 moles of NO and 3 moles of O₂), you started with 4 moles of NO and 2 moles of O₂, but ended up with leftover O₂ after the reaction:
- **Reactants used**: 4 moles of NO and 1 mole of O₂
- **Leftovers**: 0 moles of NO and 3 moles of O₂ (implying only 1 total mole of O₂ was actually used)
So to summarize:
- **Initial amounts before the reaction** should have been:
- Reactants: **4 moles of NO, 2 moles of O₂**
- **Reactants used**: **4 NO, 1 O₂** (yielding 4 NO₂)
- **Leftovers**: **0 NO, 3 O₂** (indicating that still more O₂ remains)
\[ 2 \text{NO} + \text{O}_2 \rightarrow 2 \text{NO}_2 \]
From this equation, we see that 2 moles of NO (nitric oxide) react with 1 mole of O₂ (oxygen gas) to produce 2 moles of NO₂ (nitrogen dioxide).
You provided that the products are 4 moles of NO₂ and that there are leftovers of 0 moles of NO and 3 moles of O₂.
### Understanding the Stoichiometry:
1. Since you produced 4 moles of NO₂, we can determine how many moles of reactants were needed based on the stoichiometry of the reaction.
- According to the balanced equation, 2 moles of NO yield 2 moles of NO₂. Therefore, for 4 moles of NO₂:
\[ 4 \text{NO}_2 \text{ would require } 4 \text{NO} \text{ (since } 2 \text{NO} \rightarrow 2 \text{NO}_2 \text{)} \]
2. For each mole of O₂ used, 2 moles of NO are needed to produce 2 moles of NO₂. If we produced 4 moles of NO₂, we already calculated that you would need 4 moles of NO, which would essentially mean:
- Using 2 moles of O₂ is necessary for the reaction; this is because:
\[ 2 \text{NO} + 1 \text{O}_2 \rightarrow 2 \text{NO}_2 \]
- To produce 4 moles of NO₂, you would need to double the amount of both reactants:
\[ 4 \text{NO} + 2 \text{O}_2 \rightarrow 4 \text{NO}_2 \]
### Conclusion:
Thus, in terms of the reactants based on the products produced (4 moles of NO₂) and the leftovers (0 moles of NO and 3 moles of O₂), you started with 4 moles of NO and 2 moles of O₂, but ended up with leftover O₂ after the reaction:
- **Reactants used**: 4 moles of NO and 1 mole of O₂
- **Leftovers**: 0 moles of NO and 3 moles of O₂ (implying only 1 total mole of O₂ was actually used)
So to summarize:
- **Initial amounts before the reaction** should have been:
- Reactants: **4 moles of NO, 2 moles of O₂**
- **Reactants used**: **4 NO, 1 O₂** (yielding 4 NO₂)
- **Leftovers**: **0 NO, 3 O₂** (indicating that still more O₂ remains)