topic 4: chemical equilibrium Flashcards

1
Q

explain what happens in an open chemical system

A

energy and matter move freely between the system and surroundings

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2
Q

explain what happens in a closed chemical system

A

energy can move between the system and surroundings but matter cant

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3
Q

explain what happens in an isolated chemical system

A

neither energy nor matter can move between the system and the surroundings

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4
Q

which of the 3 chemical systems is used in equilibrium reactions

A

closed

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5
Q

explain what is meant by dynamic equilibrium

A

a point where the forward and reverse reactions occur at the same rate

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6
Q

what can be stated about the reactants and products at dynamic equilibrium

A

at this point the concentrations of reactants and products remain constant butt they are rarely equal

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7
Q

explain what is meant by the equilibrium lying to the right

A

the forward reaction is favoured, and more product is made

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8
Q

explain what is meant by the equilibrium lying to the left

A

the reverse reaction is favoured and more reactant remains

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9
Q

what does le chatelier’s principle state

A

“if a system at equilibrium is subjected to change the system reajustes itself to counteract the change”

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10
Q

the three main factors afftecting an equilibriums position

A

•concentration
•temperature
•pressure

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11
Q

consider: A+2B ⇌C+D

what happens if the concentration of A or B is increased

A

•equilibrium shifts to bring [A/B] back down
•more A+B react so forward reaction is favoured
•equilibrium shifts right (more product)

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12
Q

consider: A+2B ⇌C+D

what happens if the concentration of A or B is decreased

A

•equilibrium shifts to bring [A/B] back up
•more C+D react to make more A+B
•reverse reaction is favoured (more reactant)
•equilibrium position shifts left

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13
Q

consider: A+2B ⇌C+D

what happens if the concentration of C or D is increased

A

•equilibrium shifts to bring [C/D] back down
•more C+D is converted back into reactants
•reverse reaction is favoured (more reactant)
•equilibrium position shifts left

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14
Q

consider: A+2B ⇌C+D

what happens if the concentration of C or D is decreased

A

•equilibrium shifts to bring [C/D] back up
•more A+B is converted into products
•forward reaction is favoured (more product)
•equilibrium position shifts right

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15
Q

if the forward reaction us exothermic what will the reverse be

A

endothermic

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16
Q

in an exothermic reaction what happens the the equilibrium when there is temperature increase

A

•system shifts to bring the temp back down
•reverse reaction will be favoured to absorb the additional heat
•equilibrium shifts left, favouring reactants

17
Q

in an exothermic reaction what happens the the equilibrium when there is temperature decrease

A

•system shifts to raise the temp
•favours the reaction that releases heat- the forward exothermic reaction
•equilibrium shifts right, favouring products

18
Q

describe the result of a pressure increase on this equilibrium

A+2B ⇌C+D
3 moles-2 moles

A

•equilibrium shifts to decrease the pressure (less molecules)
•shifts to the right, favouring the forward reaction

19
Q

describe the result of a pressure decrease on this equilibrium

A+2B ⇌C+D
3 moles-2 moles

A

•equilibrium shifts to increase the pressure (more molecules)
•shifts to the left, favouring the reverse reaction

20
Q

explain what happens in an equilibrium with a catalyst

A

a catalyst doesn’t effect the position of an equilibrium it just decreases the time taken for a reaction to reach equilibrium