Topic 5- Dynamic equilibria Flashcards
What is the Haber process?
-Reversable reaction
-Nitrogen and hydrogen into ammonia (fertilisers)
How does the haber process work?
1) Gasses passed into reaction vessel
2) Iron catalyst used to speed up
3) They react to form products and reactants
4) Ammonia has lower BP so we condense it
How does equilibrium shift in higher temp?
-Endothermic (normally reactants)
How does equilibrium shift in higher pressure?
-Less molecules (forced together to fuse/ collide more)
How does equilibrium shift in higher concentration?
-The other is made more
How does equilibrium shift in use of a catalyst?
-Stays the same but faster rate
What are conditions related to in industry?
-Cost effectve:
to get materials e.g nittrogen and hydrogen (for their concentration)
-To have a high temp (not for haber)
-To have a high pressure (for haber)
Conditions:
-Lower temp (prevent endothermic)
-Higher pressure (more collisions)
-Catalyst (iron, to speed)
What do fertilisers contain?
-Nitrogen
-Phosphorus
-Potassium
Ammonia + Oxygen + Water
Nitric acid
Nitric acid + ammonia
-Neutralisation
-Soluable ammonium nitrate (salt)
-Used for fertilisers
Describe the lab method to make ammonium sulfate?
1)Slowly add ammonia solution
2)Add dilute sulfuric acid to beaker (titration, phenolphthalein)
3)Evaporate water for salt crystals
titration –> crystalsation
Problems with lab method of producing ammonium sulfate?
-Small scale
-Batch process
only titration –> crystalsation
Describe the industrial process to produce ammonium sulphate?
-Haber process
- Nitrogen and hydrogen reacted to make ammonia
- Added to Sulphuric acid
fractional distillation of air, and coal gasification
Positives of Industrial process to produce ammonia sulfate
-Lager scale
-Continuous
but several stages
