Equilibrium

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What direction is the endothermic direction
backward
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what direction is the exothermic
forward
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if temperature is increased what direction does the equilibrium shift
It goes in the endothermic direction to oppose change as it does this it absorbs the heat
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if temperature is decreased what direction does the equilibrium shift
It shifts in the exothermic direction and it tries to give out heat
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Why do lower temperatures produce more product yield
Because equilibrium shifts to oppose the change by moving in the exothermic direction and trying to give out heat
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what will an increase in pressure do to the equilibrium
the equilibrium will shift to favour the side with less molecules
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what will an decrease in pressure do to the equilibrium
it will shift the equilibrium to the side with more molecules
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what happens if the concentration is increases in a reaction
the concentration will move to oppose the increase in concentration and try and decrease the concentration
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what effect will a catalyst have on the equilibrium
a catalyst does not effect the equilibrium it will only speed up the rate at which equilibrium is achieved.
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CO (g) + 2H2(g) ------------>CH3OH (g) in this equation why is a high pressure and low temp used
There is a high pressure to favour the side with less molecules which is the RHS also a low compromised temperature is used because the equilibrium will shift in the exothermic direction meaning heat is given out.
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CH2=CH2 (g) + H2O (g)-------> CH3CH2OH(l) Why is a high pressure used in the production of ethanol
so equilibrium shifts to the right to favour the side with less molecules also to stop the unwanted polymerisation of polyethene
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What does Kc mean
Equilibrium constant
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how do you calculate moles of reactant at equilibrium
initial moles - moles reacted
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how do you calculate moles of product at equilibrium
initial moles + moles formed
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if the Kc value is larger what does that mean
it favours the products more
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What does kc only change with
temperature
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if temperature is increased what does this do to the Kc value
Equilibrium shifts left in the endothermic direction meaning less products produced and more reactants produced
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if there are more moles on the right side of a reaction what happens to the Kc value if pressure is increased
The equilibrium will shift left because there are less moles and because pressure is increased however the Kc value is not altered as pressure has no effect on Kc only temperature
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brown I2 + 2OH------->I - + IO- + H2O colourless what happens if concentration of OH- increased
Equilibrium shifts in the exothermic direction to oppose the change in concentration meaning the amount of I- and IO- increases turning the product brown to colourless
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Other cards in this set

Card 2

Front

what direction is the exothermic

Back

forward

Card 3

Front

if temperature is increased what direction does the equilibrium shift

Back

Preview of the front of card 3

Card 4

Front

if temperature is decreased what direction does the equilibrium shift

Back

Preview of the front of card 4

Card 5

Front

Why do lower temperatures produce more product yield

Back

Preview of the front of card 5
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