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inorganic chemistry
module 3
equilibrium
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Created by
Maryam Mirza
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Cards (18)
Chemical equilibrium
All
reversible
reactions reach a
dynamic
equilibrium state
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Dynamic equilibrium
1. Forward and
backward
reactions are occurring at
equal
rates
2. Concentrations of reactants and products stays
constant
3. Reaction is
continuous
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Position of equilibrium
Describes the
composition
of the
equilibrium
mixture
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Position of equilibrium favouring reactants
Equilibrium mixture
will contain mostly
reactants
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Le Chatelier's principle
If an external condition is changed the equilibrium will shift to
oppose
the change (and try to
reverse
it)
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If temperature is increased
Equilibrium will shift in the
endothermic
direction to try to
reduce
the temperature
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If temperature is
decreased
Equilibrium will shift in the
exothermic
direction to try to
increase
the temperature
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Low
temperatures may give a
higher
yield of product but will also result in slow rates of reaction
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If pressure is
increased
Equilibrium will shift towards the side with
fewer
moles of gas to try to
reduce
the pressure
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If pressure is
decreased
Equilibrium will shift towards the side with more
moles
of gas to try to
increase
the pressure
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If the number of
moles
of
gas
is the same on both sides of the equation then changing pressure will have no effect on the position of equilibrium
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Increasing the concentration of OH- ions
Equilibrium shifts in the
forward
direction to remove
OH-
ions
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Adding
H+
ions
Equilibrium shifts back to the
left
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A
catalyst
has no effect on the position of equilibrium, but it will
speed up
the rate at which the equilibrium is achieved
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Industrial processes using equilibrium
Haber
process
Contact
process
Hydration
of
ethene
Production of
methanol
from
CO
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Recycling unreacted reactants back into the
reactor
can improve the overall
yields
of these processes
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High
pressure leads to too
high
energy costs for pumps and too high equipment costs
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Catalysts
speed up the rate, allowing
lower
temperatures to be used but have no effect on equilibrium
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