Question

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

• A. 10
• B. 20
• C. 30
• D. 40

Answer 1

The Correct Option is C

To solve this problem, we need to consider the chemical reaction involved in the production of ammonia through the Haber process. The balanced chemical equation for this reaction is:

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

This equation tells us that 1 mole of nitrogen gas reacts with 3 moles of hydrogen gas to produce 2 moles of ammonia. Thus, the stoichiometric ratio between hydrogen and ammonia is 3:2.

Given in the problem, we need to produce 20 moles of ammonia. Let's calculate the number of moles of hydrogen required:

According to the stoichiometric ratio, 2 moles of ammonia require 3 moles of hydrogen. Therefore, to find out how many moles of hydrogen are needed for 20 moles of ammonia, we set up the proportion:

\frac{3 \text{ moles of } H_2}{2 \text{ moles of } NH_3} = \frac{x \text{ moles of } H_2}{20 \text{ moles of } NH_3}

Cross-multiplying gives us:

2x = 20 \times 3

2x = 60

Dividing each side by 2 to solve for x gives:

x = \frac{60}{2} = 30

Therefore, 30 moles of hydrogen gas are required to produce 20 moles of ammonia.

Hence, the correct answer is 30.