harbor process Flashcards
full equations
N2(g)+3H2(g) ⇌ 2NH3(g)
stage one
obtain reactants and mix in 3:1 ratio
stage two
set the conditions in a sealed container
stage 3
cool mixture so ammonia can condense and be collected.
stage 4
the hydrogen gas and nitrogen gas are recycled back into the reaction vessel
what happens if the forward reaction is favored
The equilibrium will shift to the right and the yield of products will increase
what happens if the backwards reaction is favored
The equilibrium will shift to the left and the yield of products will decrease
what can ammonia be used for
fertilisers,explosivesand dyes
Complete the missinf information for the harer process
nitrogen from the air
hydrogen from CH4
nitrogen and hydrogen 3:1 ratio
400-500 200atm iron catalyst
unreacted gases recycled
gases are cooled and and condense into liquids
why is 450 degrees used in the haber process
temp lower= eaction too slow but high production yield
temp high= reaction is fast but lower yield
450= reaction and yield reasonable
why is 200atm used in haber process
too high pressure = dangerous + expensive
the forward reaction is
exothermic (releases energy in the form of hea)
the backwards reaction is
endothermic ( absorbs energy from surroundings)
If reaction mixture is cooled
the equilibrium will shift to exothermic to heat the surroundings.
if the reaction mixture is heated
the equilibrium will shift to endothermix to decrease the temperature
