Industrial Equilibrium & The Haber Process
Call Kai
Learn
Practice Test
Spaced Repetition
Match
Flashcards
Knowt Play1/19
There's no tags or description
Looks like no tags are added yet.
Name | Mastery | Learn | Test | Matching | Spaced | Call with Kai | Chat |
|---|
No analytics yet
Send a link to your students to track their progress
20 Terms
What is the Haber process?
The industrial process used to produce ammonia from nitrogen and hydrogen.
What is the balanced symbol equation for the Haber process?
N₂(g) + 3H₂(g) ⇌ 2NH₃(g).
Where is nitrogen obtained for the Haber process?
From the air.
Where is hydrogen commonly obtained for the Haber process?
From natural gas, through industrial processing.
Is the forward Haber reaction exothermic or endothermic?
Exothermic.
Why does increasing pressure favour ammonia production?
There are four moles of gas on the left and two on the right, so equilibrium shifts towards ammonia.
Why does decreasing temperature favour ammonia production?
The forward reaction is exothermic, so lower temperature favours products.
Why is a very low temperature not used?
The reaction would be too slow to be economically viable.
What temperature is typically used in the Haber process?
Approximately 450°C.
What pressure is typically used in the Haber process?
Approximately 200 atmospheres.
What catalyst is used in the Haber process?
Iron.
Why is an iron catalyst used?
It increases reaction rate by lowering activation energy.
Does iron increase the equilibrium yield of ammonia?
No, it only helps equilibrium be reached faster.
Why is a compromise temperature used?
To balance reaction rate and equilibrium yield.
Why is a compromise pressure used?
To balance ammonia yield, reaction rate, equipment cost and safety.
How is ammonia separated from the reaction mixture?
The mixture is cooled so ammonia condenses.
What happens to unreacted nitrogen and hydrogen?
They are recycled back into the reactor.
Why is recycling unreacted gases useful?
It reduces waste and increases overall conversion into ammonia.
What is ammonia mainly used for?
Producing fertilisers and other nitrogen-containing chemicals.
Why is the Haber process an example of industrial compromise?
Conditions balance yield, rate, energy costs and equipment costs.