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To solve this problem, we will address each part (a, b, and c) individually using stoichiometry and relevant chemical principles.

### Given Data and Reaction
**Reaction:** 
\[
\text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3
\]

**Data provided:**
- **Nitrogen (N₂)**: 4202 lb per hour
- **Hydrogen (H₂)**: 1046 lb per hour
- **Ammonia (NH₃)** produced: 3060 lb per hour

### Molar Masses
- **Molar mass of N₂**: \( 28 \, \text{g/mol} \)
- **Molar mass of H₂**: \( 2 \, \text{g/mol} \)
- **Molar mass of NH₃**: \( 17 \, \text{g/mol} \)

### Step 1: Convert Given Masses to Moles
1. **Convert nitrogen (N₂) to moles:**
   \[
   \text{Moles of N}_2 = \frac{4202 \, \text{lb} \times 453.592 \, \text{g/lb}}{28 \, \text{g/mol}}
   \]

2. **Convert hydrogen (H₂) to moles:**
   \[
   \text{Moles of H}_2 = \frac{1046 \, \text{lb} \times 453.592 \, \text{g/lb}}{2 \, \text{g/mol}}
   \]

### Step 2: Determine the Limiting Reactant
From the reaction, 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃. We’ll use the mole ratios and calculated moles to find the limiting reactant.

### Step 3: Calculate Percent Excess Reactant
Using the limiting reactant, we can determine how much of the other reactant is in excess and then calculate the percent excess.

### Step 4: Calculate Percent Conversion (Based on Limiting Reactant)
Percent conversion will be based on the actual yield (3060 lb of NH₃ produced) compared to the theoretical yield calculated from the limiting reactant.

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I will now go through each part in detail to provide the final answers.

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### Follow-Up Questions
1. What is the purpose of identifying the limiting reactant in a reaction?
2. How does calculating the percent excess help in optimizing chemical reactions?
3. Why is it necessary to calculate theoretical yield before determining percent conversion?
4. How would the calculations change if the reactor efficiency were considered?
5. Can this method be applied to other types of reactions with different stoichiometries?

### Tip
When working with stoichiometry, always start by balancing the equation and identifying molar masses for accurate conversions.

The synthesis of ammonia proceeds according to the following reaction: N₂ + 3 H₂ → 2 NH₃. In a given plant, 4202 lb of nitrogen and 1046 lb of hydrogen are fed to the synthesis reactor per hour. Production of pure ammonia from this reactor is 3060 lb per hour. Calculate: (a) the limiting reactant, (b) the percent excess reactant, and (c) the percent conversion obtained based on the limiting reactant.

Solve a stoichiometry problem involving ammonia synthesis: identify the limiting reactant, calculate the percent excess reactant, and determine the percent conversion based on the limiting reactant. Given data includes 4202 lb of nitrogen, 1046 lb of hydrogen, and 3060 lb of ammonia produced per hour. Suitable for Grades 11-12 chemistry students.

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