Topic 11 - 11.2 - Reactions of Ammonia

Question 1

Haber Process equation?

Answer 1

nitrogen + hydrogen ⇌ ammonia
N₂+3H₂ ⇌ 2NH₃
* makes use of an iron catalyst to speed up the reaction
* catalyst can be reused = saves money

Question 2

Describe how ammonia is made industrially

Answer 2

• Made through the Haber process
• Haber process is reversible, it never goes to completion

Question 3

• Describe the problem with the Haber process
• Explain why a lower temp and higher pressure is NOT used

Answer 3

• Impossible for all the nitrogen and hydrogen to be turned into 100% ammonia, since the reaction is being broken down at the same time, so a low yield is produced
• Lower temp = slower rate of reaction
• Higher pressure = more expensive for the companies

Question 4

Describe the condtions needed to complete the Haber process EFFICIENTLY, referring to ats and temp.

Answer 4

• 200 ats - used because both reactants are gases so molecules need to collide to react together, which is why pressure is used
• 450°C - used because at room temp = rate of reaction is too slow, but if temp is too high, ammonia breaks down.