U3-4-1 - Equilibria Flashcards

Part of the Equilibria and Industrial Processes topic from Unit 3 of Higher Chemistry, Chemistry in Society

1
Q

At equilibrium, the
_____ of forward and reverse reactions are equal.

A

rates

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2
Q

At equilibrium, the
_____ of forward and reverse reactions are constant.

A

concentrations

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3
Q

State the effect a catalyst has on the equilibrium position

A

None
(rates of forward/reverse reactions are increased by the same amount)

but equilibrium is reached faster

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4
Q

If pressure is increased, which reaction will be favoured:
forward or reverse?

A

Forward

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5
Q

The forward reaction is favoured if pressure is increased.
Why?

A

Fewer gas moles on product side

so favouring forward reaction helps decrease pressure

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6
Q

If pressure is increased, which reaction will be favoured:
forward or reverse?

A

Reverse

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7
Q

Pressure has no effect on this equilibrium. Why?

A

Same no. of gas moles on both sides

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8
Q

Would you increase or decrease temperature to maximise product yield?

A

Decrease

Reaction is exothermic

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9
Q

Would you increase or decrease temperature to maximise product yield?

A

Increase

Reaction is endothermic

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10
Q

Why does an increase in temperature favour reactants?

A

Reaction is exothermic

(so reverse reaction will be favoured to reduce heat)

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11
Q

State Le Chatelier’s principle

A

If a system at equilibrium is subjected to any change, the system readjusts itself to counteract the applied change.

E.g. increased T = endothermic reaction favoured to lower it again

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12
Q

Why does adding OH ions increase the rate of the reverse reaction?

A

Because OH reacts with H+, and the reverse reaction is favoured to replace the H+ used up

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13
Q

Suggest one way to maximise profit in an industrial process.

A

Any of:
*recycle/sell by-products
*use catalysts
*run reactions at low temperatures if possible
*use cheap feedstocks if possible.

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