Question
4NH3 + 3O2 = 2N2 + 6H20
products: 2 N2, 6 H20
leftovers: 0 NH3, 2 O2
what are the reactants?
products: 2 N2, 6 H20
leftovers: 0 NH3, 2 O2
what are the reactants?
Answers
Answered by
GPT-4o mini
In the given reaction:
\[ 4 \text{NH}_3 + 3 \text{O}_2 \rightarrow 2 \text{N}_2 + 6 \text{H}_2\text{O} \]
the reactants are ammonia (NH₃) and oxygen (O₂).
From the stoichiometry of the reaction:
- **Reactants**: \( 4\text{NH}_3\) (ammonia) and \(3\text{O}_2\) (oxygen).
Since you mentioned that there are "leftovers: 0 NH₃, 2 O₂", it implies that all 4 moles of NH₃ were consumed, and only 1 mole of O₂ was used, leaving 2 moles of O₂ unreacted. Therefore, the specific amounts of the reactants would have started at \(4 \text{NH}_3\) and \(3 \text{O}_2\), with only 1 mole of O₂ reacting due to the consumption of NH₃.
So the complete answer:
- Reactants used were \(4 \text{NH}_3\) and \(3 \text{O}_2\), but only \(1 \text{O}_2\) was consumed in the reaction.
\[ 4 \text{NH}_3 + 3 \text{O}_2 \rightarrow 2 \text{N}_2 + 6 \text{H}_2\text{O} \]
the reactants are ammonia (NH₃) and oxygen (O₂).
From the stoichiometry of the reaction:
- **Reactants**: \( 4\text{NH}_3\) (ammonia) and \(3\text{O}_2\) (oxygen).
Since you mentioned that there are "leftovers: 0 NH₃, 2 O₂", it implies that all 4 moles of NH₃ were consumed, and only 1 mole of O₂ was used, leaving 2 moles of O₂ unreacted. Therefore, the specific amounts of the reactants would have started at \(4 \text{NH}_3\) and \(3 \text{O}_2\), with only 1 mole of O₂ reacting due to the consumption of NH₃.
So the complete answer:
- Reactants used were \(4 \text{NH}_3\) and \(3 \text{O}_2\), but only \(1 \text{O}_2\) was consumed in the reaction.