The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber's process is :

Options

A. 40
B. 10
C. 20
D. 30

Explanation

To solve the problem of how many moles of hydrogen molecules are required to produce 20 moles of ammonia through the Haber process, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Haber Process Reaction**:
The Haber process can be represented by the balanced chemical equation:
\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]
This indicates that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.

2. **Determine the Ratio of Hydrogen to Ammonia**:
From the balanced equation, we can see that:
- 2 moles of ammonia (NH₃) are produced from 3 moles of hydrogen (H₂).
- Therefore, the ratio of hydrogen to ammonia is:
\[ \frac{3 \text{ moles of } H_2}{2 \text{ moles of } NH_3} \]

3. **Calculate Hydrogen Required for 20 Moles of Ammonia**:
We need to find out how many moles of hydrogen are required to produce 20 moles of ammonia. Using the ratio derived from the balanced equation:
\[ \text{Hydrogen required} = 20 \text{ moles of } NH_3 \times \frac{3 \text{ moles of } H_2}{2 \text{ moles of } NH_3} \]
Simplifying this gives:
\[ \text{Hydrogen required} = 20 \times \frac{3}{2} = 20 \times 1.5 = 30 \text{ moles of } H_2 \]

4. **Final Answer**:
Therefore, the number of moles of hydrogen molecules required to produce 20 moles of ammonia is **30 moles**.