Question

In the Haber’s process, 30 L of hydrogen and 30 L of nitrogen were taken for the reaction, which yielded only 50% of the expected product. What will be the composition of the gaseous mixture under the aforementioned condition after reaction is completed?

• A. 20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
• B. 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
• C. 20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen
• D. 20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen

Answer 1

The correct option is B 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen

Given: $N_2+3H_2\to 2N{H}_3$
1 L of nitrogen reacts with 3 L of hydrogen.
30 L of nitrogen will react with $\frac{3}{1}\times 30=90$ L of hydrogen.
But we are given only 30 L of hydrogen (according to the question)
Therefore, hydrogen is the limiting reagent.
3 L of hydrogen produce 2 L of ammonia.
With 100% efficiency, 30 L of hydrogen will produce 20 L of ammonia
But with 50% efficiency, only 10 L of ammonia is produced.
Therefore, only 15 L of hydrogen reacted.
3 L of hydrogen react with 1 L of nitrogen,
So, 15 L of hydrogen will react with 5 L of nitrogen
Composition of the gaseous mixture in the end will be:
Hydrogen remaining = 30 L - 15 L = 15 L
Nitrogen remaining = 30 L - 5 L = 25 L
Ammonia produced = 10 L