EQUILIBRIUM - created from Mind Map

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Dynamic equilibrium: a situation in which the composition of a reaction mixture doesn't change because both the forward and backward reactions are proceeding at the same rate.

LE CHATELIER'S PRINCIPLE... if a system at equilibrium is disturbed then the equilibrium shifts in the direction that tends to reduce this disturbance

AMMONIA, NH3

ETHANOL

Equilibrium...

... can only be reached in a closed system

... can be approached from either direction and still reach the same position of final equilibrium

Changing concentrations... increasing the concentration of a reactant tend to favour the forward reaction and so equilibrium shifts to the right.

Changing the overall pressure... only affects gaseous reactions. Equilibrium favours the side of the reaction with the least molecules of gas.

Changing temperature... if you increase temperature, equilibrium favours the reaction which cools the system down (endothermic reaction)

used to make fertilisers (ammonium nitrate, ammonium sulfate and urea) as well as synthetic fibres (nylon), dyes, explosives and plastics

N2(g) + H2(g) 2NH3(g)

Yield depends on temperature and pressure.. low temperature and high pressure gives high yield, and high temperature and low pressure gives a low yield.

is made by the hydration of ethene

H2C=CH2(g) + H2O(g) CH3CH2OH(g)

favours.. high pressure, low temperature, with excess steam. HOWEVER, low temp. reduces reaction rate, high pressure increases costs and too much steam can affect the catalyst

catalyst = phosphoric acid on silica