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Flashcards in Equillibrium Deck (28)
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1
Q

What is the equilibrium?

A

When the rate of the forward reaction is equal to the rate of backwards reaction, the system reaches dynamic equilibrium.

2
Q

Can equilibrium be reached in an open system?

A

No, the system should be closed, where no gaseous products can escape container.

3
Q

What type of reaction would occur on an open system?

A

An irreversable reaction.

4
Q

What is the difference between rate and extent?

A

Rate refers to how quickly reaction proceeds, while extent refers to degrees of conversion.`

5
Q

What 2 factors do manufactures consider when establishing reactions?

A

Rate and yield.

6
Q

What does competing equillibira refer to and what it one example?

A

When reactions occur simultaneously and the outcome of one reaction influences the other.
Eg. oxygen and co competing equilibria

7
Q

Why would small amounts of CO be harmful for someone when there is plenty of O2 around?

A

CO has an extremely high Kc and so its reaction is favoured in comparison to oxygens. CO will be more strongly absorbed by haemoglobin, preventing O2 from binding with HB.

8
Q

Does temperature effect Kc?

A

YES

9
Q

What is Kc a measure of?

A

The yield or extent of reaction.

10
Q

What does a low Kc mean and what does a high Kc mean?

A

Low: reverse reaction is favoured- more reactants
High: forwards reaction is favoured- more products

11
Q

What is the concentration quotient?

A

Q is a form of the equilibrium expression which is a measure of the relative amounts of products and reactants present. It indicates weather reaction is at equilibrium or not.

12
Q

What does a low Q mean and what does a high Q mean?

A

Low: reverse reaction is favoured- more reactants
High: forwards reaction is favoured- more products

13
Q

What is the Q and Kc expression used to identify extent of reaction?

A

Kc < Q < Kc

14
Q

What is the reactionship between Kc and n, where n is the value that the equation is changed by?

A

(kc) ^n

15
Q

What tool should you always use when calculating equillibrium concebtrations?

A

Rice table.

16
Q

What is Le Chatliers principle?

A

When a system in =m, is subjected to change equilibrium will shift in order to favour the reaction that partially oposes the change.

17
Q

How does adding product effect equilibrium?

same as removing reactant

A

System favours net backwards reaction.

18
Q

How does adding reactant effect equilibrium?

same as removing product

A

System favours net forwards reaction.

19
Q

How does diluting reaction effect equillibrium?

A

System favours reaction with most moles in order to increase concentration.

20
Q

How does increasing pressure effect equillibrium?

same as decreasing volume

A

System favours reaction with least moles in order to reduce volume.

21
Q

How does decreasing pressure effect equillibrium?

same as increasing volume

A

System favours reaction with most moles in order to

increase volume.

22
Q

How does increasing temp effect equillibrium of exothermic reaction?

A

System favours net backwards reaction in order to decrease temp.
Kc descreases

23
Q

How does decreasing temp effect equillibrium of exothermic reaction?

A

System favours net fowards reaction in order to increase temp.
Kc increases

24
Q

How does increasing temp effect equillibrium of endothermic reaction?

A

System favours net fowards reaction in order to increase temp.
Kc increases

25
Q

How does decreasing temp effect equilibrium of endothermic reaction?

A

System favours net backwards reaction in order to decrease temp.
Kc descreases

26
Q

How does adding an inert gas to a solution affect the equilibrium?

A

It increases the volume, hence pressure decreases. This means the equilibrium will shift to the side with the most amount of moles.

27
Q

How do you answer equilibrium questions?

A
  1. describe the change
  2. describe Le Chateliers principle
  3. describe the equilibrium
28
Q

Answer the following question:
When more reactant is added, what colour will the solution be?
left= clear right= brown

A

When [O2] increases, the system will adjust to partially oppose the change and favour the reaction that decreases [O2]. Therefore the equilibrium shifts in a net forwards direction, producing more NO2 which increases browness.