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 determine the number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber's process, we first need to understand the balanced chemical equation for the synthesis of ammonia:

\[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \]

From this equation, we can see that:

- 1 mole of nitrogen (N₂) reacts with 3 moles of hydrogen (H₂) to produce 2 moles of ammonia (NH₃).

Now, we need to find out how many moles of hydrogen are required to produce 20 moles of ammonia.

1. **Determine the ratio of hydrogen to ammonia:**
From the balanced equation, we see that 3 moles of hydrogen are needed to produce 2 moles of ammonia.

\[ \text{Ratio of } H_2 \text{ to } NH_3 = \frac{3 \text{ moles of } H_2}{2 \text{ moles of } NH_3} \]

2. **Set up a proportion to find the moles of hydrogen needed for 20 moles of ammonia:**
We can use a unitary method to find the moles of hydrogen required for 20 moles of ammonia.

\[ \text{If } 2 \text{ moles of } NH_3 \text{ require } 3 \text{ moles of } H_2, \]
\[ \text{Then } 20 \text{ moles of } NH_3 \text{ will require } \left( \frac{3 \text{ moles of } H_2}{2 \text{ moles of } NH_3} \right) \times 20 \text{ moles of } NH_3 \]

3. **Calculate the moles of hydrogen:**
\[ \text{Moles of } H_2 = \frac{3}{2} \times 20 = 30 \text{ moles of } H_2 \]

Thus, the number of moles of hydrogen molecules required to produce 20 moles of ammonia is **30 moles**.

**Final Answer: 30 moles of hydrogen.**

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