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Topic 4: Gases, Equilibria and Ammonia
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Chemistry Mapa Mental sobre Topic 4: Gases, Equilibria and Ammonia, criado por Alice Clayden em 25-04-2013.
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chemistry
chemistry
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Alice Clayden
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Alice Clayden
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Topic 4: Gases, Equilibria and Ammonia
The Harber process
Fritz Harber, 1900's
Uses the reversible reaction of ammonia- the conditions allow the forward reaction to happen faster than the backward reaction as it is in equilibirum
200 atmospheres, 450 ' C, iron catalyst
Molar volume of gases
Avogadro's gas law- 1 mole of any gas at room temperature and normal atmospheric pressure has a volume of 24dm'3
using the idea of molar volume we can calculate volumes of gases needed for reactions
e.g. how much methane (CH4) is burned completely in oxygen if 11g of CO2 is produced?
1. balanced symbol equation, 2. work out number of moles in 11g of CO2, 3. work out molar ratio of methane to CO2,4 . number of moles x molar volume
volume (dm'3) = number of moles x molar volume of gas (dm'3)
Reversible reactions
A + B <> C + D
The products of a reaction will react to give the original reactants back
ammonium chloride + HEAT <<>> Ammonia + Hydrogen Chloride
Equilibrium
The forward and backward reactions happen at the same rate.
decreasing the temperature for the ammonia reaction will result in an increase of the rate of forward reaction because it is exothermic - heats up
'equilibirum has shifted to the right'
increasing pressure results in a higher yield of ammonia as the equilibrium again shifts to the right. This is to expensive, it is done at 200 at
Fertilisers
Over-use of nitrate fertilisers leads to Eutrophication
contain soluble nitrogen compounds which plants need to make proteins
Ammonia is a raw material used to make nitrogenous fertilisers
advantages of manmade- easy to store, distribute and handle, produced to match requirements, increase yield of crops
disadvantages of over use- high nitrate levels are dangerous in drinking water, eutrophication
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