Lesson 9: The Harber Process

Question 1

What can the ammonia ,manufactured by The Harber process, be used for?

Answer 1

• The ammonia can be used to produce nitrogen-based fertilisers.

Question 2

What are the 2 raw materials/ reactants for The Harber Process?

Answer 2

• Nitrogen
• Hydrogen

Question 3

What is the source of nitrogen (for Harber Process?)

Answer 3

• The air.

Question 4

What is the source of hydrogen (for the Harber process?)

Answer 4

• Methane.

Question 5

At what temperature and pressure does The Harber Process take place? What catalyst is used in this reaction?

Answer 5

• 450 degrees.
• 200 atmospheres.
• Iron catalyst.

Question 6

TRUE OR FALSE….

450 degrees and 200 atmospheres are considered to be a LOW temperature and a LOW pressure.

Answer 6

• FALSE!!
• 450 degrees and 200 atmospheres are considered to be a high temperature and a high pressure.

Question 7

What are the 4 steps to The Harber process reaction?

Answer 7

1.) Nitrogen and hydrogen pass over an iron catalyst and react in a reactor.
2.) Some of the nitrogen and hydrogen react to form ammonia - some of the ammonia produced breaks down into hydrogen and nitrogen (as reaction is reversible.)
3.) Ammonia is cooled in a condenser and liquefies.
4.) The remaining hydrogen and nitrogen are recycled/ go back to the reactor where they will react again.

Question 8

What compromise needs to be made in this reaction?

Answer 8

• Compromise between RATE OF REACTION and yield (due to equilibrium position.)

Question 9

Why is a VERY high temperature not used in The Harber Process?

Answer 9

• Forward reaction is exothermic so would reduce yield of ammonia further - by shifting equilibrium position to the left.
• High energy costs.

Question 10

What is the issue with having an extremely high pressure (even though it would increase both the yield/ the rate of reaction?)

Answer 10

• It is expensive and dangerous to work with very high pressures.

Question 11

TRUE OR FALSE

The use of a catalyst affects the position of equilibrium in the reaction.

Answer 11

• False.
• Only affects rate (by decreasing activation energy.)