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Reversible Reactions and Le Chatelier's Principle (reversible…
Reversible Reactions and Le Chatelier's Principle
equilibrium
- when the forwards reaction is going at exactly the same rate as the backwards one
reversible reactions
as the forwards reactants react their
concentrations fall
so it will slow down but as more and more products are made their
concentrations rise
, the backwards reaction will speed up
after a while the system will be at
eqilibrium
at equilibrium both reactions are still happening but there is
no overall effect
as they have reached a
balance
and wont change
equilibrium can only be reached if the reversible reaction takes place in a closed system
position of equilibrium
when a reaction is at equilibrium it doesn't mean the amount of reactants and products are equal
lies to the
right
- concentration of
products is greater
than the reactants
lies to the
left
- concentration of
reactants is greater
than the products
the position depends on:
temperature
pressure
concentration
endo / exothermic
in reversible reactions if it is
endothermic
one way it will be
exothermic
in the other
energy transferred
from the surrounds by
endothermic reaction
=
energy transferred
to the surrounding during the
exothermic reaction
Le Chatelier's Principle
the idea that if you
change the conditions
of a reversible reaction at
equilibrium
the system will try to
counteract that change
temperature
if you
decrease the temperature
the equilibrium will move in the exothermic direction to
produce more heat
. This means you get
more
products for the
exothermic
reaction and
fewer
products for the
endothermic
reaction
pressure
if you
increase
the pressure the equilibrium tries to reduce it - it
moves
in the direction where there are
fewer molecules of gas
if you
decrease
the pressure the equilibrium tries to increase it - it
moves
in the direction where there are
more molecules of gas
concentration
if you change the concentration of either of the reactants or products the
system will no longer be at equilibrium
if you
increase
the concentration of the reactants the system tries to
decrease
it by
making more products
if you
decrease
the concentration of products the system tries to
increase
it again by
reducing the amount of reactants