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are chemical reactions reversible
yes - the sign is ā
the direction of some reversible reactions can be altered by changing the reaction conditions
forward reaction = left to right
backward reaction = right to left
dynamic equilibrium
forward and backward reactions are occurring at the same rate, so the amount of reactant and product doesnāt change
position of equilibrium
ālies to the leftā = more reactant than product at equilibrium
ālies to the rightā = more product than reactant at equilibrium
how can equilibrium be affected
if there is a change is the surroundings, equilibrium moves to counteract the change
e.g. if the temperature increases, the opposing action will be to decrease temperature and shift towards the endothermic side of the reaction
if pressure increases, the opposing action will be to decrease pressure and shift to the side with less gas molecules
same works with increasing reactant/product concentration
how can rate of attainment of equilibrium be affected
catalysts increase speed at which equilibrium is reached (but not equilibrium position)
changing temperature/pressure/concentration can also shift the position of equilibrium and so change how long it takes to achieve it
haber process
reversible reaction (so it can obtain equilibrium) between nitrogen and hydrogen to form ammonia
3H2 + N2 ā> 2NH3
nitrogen = extracted from air
hydrogen = obtained from natural gas
conditions for haber process
iron catalyst
temperature 450 degrees C
pressure 200 atmospheres
explain temperature for haber process
ideal = lower temperature would favour forward reaction as it is exothermic so the equilibrium would shift to the right to increase temperature, increasing the yield of ammonia
however, this would mean that the rate of reaction is very slow at low temperatures
450 degrees C is a compromise; reduces yield but increases rate of reaction
explain pressure of haber process
ideal = high pressure would favour forward reaction as the equilibrium would shift to the right to decrease pressure as there are less gas molecules, increasing the yield of ammonia
however high pressures can be very dangerous and expensive to maintain, buy equipment for, and contain
so 200 atm is a compromise between a lower yielf of products being made more safely and economically
fertilisers
may contain nitrogen (found in soluble ions such as ammonium and nitrate), phosphorus, and potassium compounds to promote plant growth
ammonia being used for fertiliser:
ammonia + nitric acid ā> ammonium nitrate
making ammonium sulfate in the laboratory
preparing ammonium sulfate by titration:
add exact volume of ammonia to conical flask placed on the white tile
add a few drops of indicator and swirl - should turn yellow
add sulfuric acid to flask solution drop by drop, swirling the falsk in between
continue until the colour turns red sharply and record the titre
repeat by adding exactly the same amount of acid but this time without the indicator (is an impurity(
pour reaction mixture in an evaporating dish, gently heat in water bath to remove some water
leave in dry place so remaining water evaporates, allowing crystallisation to occur
after a few days ammonium sulfate crystals should appear
industrial preparation of ammonium sulfate
large scale operation
hugely expensive and complex
ammonia prepared by haber process, sulfuric acid by contact process
comparing industrial and laboratory productions of ammonium sulfate
in laboratory more simple equipment needed, industrial is hugely expensive and complex
in laboratory lower concentrations, industrial high concentrations
laboratory less heat given off, industrial highly exothermic
in laboratory product separated by crystallisation which is a very slow process, industrial heat produced is used to evaporate water from the reaction mixture to make very concentrated ammonium sulfate