4NH₃ + 5O₂ → 6H₂O + 4NO
When 1 mole of ammonia (NH₃) reacts with 1 mole of oxygen (O₂), which of the following

Question

4NH₃ + 5O₂ → 6H₂O + 4NO
When 1 mole of ammonia (NH₃) reacts with 1 mole of oxygen (O₂), which of the following outcomes occurs regarding the consumption of the reactants?

Accepted Answer

1. **Analyze Stoichiometry:** From the balanced chemical equation, $4	ext{ mol of NH}_3$ require $5	ext{ mol of O}_2$ to react completely.
2. **Calculate Required Amounts:**
   - For $1	ext{ mol of NH}_3$, the required amount of $O_2$ is $\frac{5}{4} 	imes 1 = 1.25	ext{ mol}$.
3. **Compare with Given Amounts:**
   - We are given only $1	ext{ mol of O}_2$, which is less than the required $1.25	ext{ mol}$.
   - Therefore, Oxygen ($O_2$) is the **limiting reagent** and will be completely consumed before the ammonia is used up.
4. **Check Excess Reagent:**
   - Amount of $NH_3$ consumed for $1	ext{ mol O}_2$ = $\frac{4}{5} 	imes 1 = 0.8	ext{ mol}$.
   - Remaining $NH_3$ = $1 - 0.8 = 0.2	ext{ mol}$. Thus, ammonia is in excess.

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