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Haber Process - Coggle Diagram
Haber Process
Economic Importance
Produces different types of salts used in chemical reactions
Nitrogen Salt
Phosphorous Salt
Potassium Salt
Nylon
Ammonium Nitrate
Fertilizer
Society is extremely dependent on fertilizer to optimize use of land
Explosives
Household Cleaning Products
Dyes
Water Purification
Refrigerant
Pharmaceuticals
Le Chatelier's Principle
(Change in T, pressure, or [ ] pushes equilibrium to a side of the reaction)
Temperature
Compromise is made
400-450 degrees celcius
Anywhere between
300-500 degrees celcius
Decrease temperature
Increase yield
favours exothermic reaction
Exothermic = forward reaction
Decrease rate of reaction
Increase temperature
Increase rate of reaction
particles collide
Decrease yield
Concentration
High concentration of
H2
favour forward reaction
Produces ammonia
N2
Process
PROCESS
Pressure
Lower pressure
cheaper
Easier
high pressure
expensive
favours reaction
that has fewer gas molecules
2NH3 in this case
therefore, more ammonia produced
The compromise
150-250 atmospheres
High
Dangerous
Expensive
N2(g)+3H2(g)↽⇀2NH3(g) ΔH=−92.4kJ/mol
Avogadros law
1 mol of N2
For 3mol of H2
gases have same mol when
temperature is same
pressure is same
Reactants
N2
Ratio: 1
Extracted from atmosphere
H2
Ratio: 3
Extracted from Methane Ga
300atm
High pressure
breaks Nitrogen bonds
1 more item...
ICE Table
C
-x
-x
+x
E
6-x
20-x
x
I
6 mol
20 mol
0
N2(g)+3H2(g)↽⇀2NH3(g)
Reacting at 50atm
Temperature Issue
The trade-off
Lower temperatures yield more Ammonia
But to increase rate of reaction temperature must be high
The compromise
Solution!
An
Iron(Oxide) Catalyst
removes the need for high temperatures for faster rate of reaction
Increase of pressure yield more Ammonia
But higher pressure is inefficient and expensive(Dangerous too!)
The compromise
150-250 atmospheres
High
Dangerous
Expensive
