How far

Question 1

How is the equilibrium constant denoted?

Answer 1

K

Question 2

What are the units for concentration?

Answer 2

moldm⁻³

Question 3

What brackets are used in then Kc equation?

Answer 3

[square brackets]

Question 4

How do you work out Kc?

Answer 4

Concentration of products / concentration of reactants

Question 5

How do you work out the power to which a concentration is raised to in the Kc equation?

Answer 5

However many moles are in the overall balanced equation

Question 6

Do you + or X the concentrations of products in the Kc equation?

Answer 6

X

Question 7

Do you + or X the concentrations of reactants in the Kc equation?

Answer 7

X

Question 8

What are the units for Kc if there is one more on the bottom than the top?

Answer 8

dm³mol⁻¹

Question 9

What are the units for Kc if there is one more on the top than the bottom?

Answer 9

mol dm⁻³

Question 10

What are the units for Kc if there is two more on the bottom than the top?

Answer 10

dm⁶ mol⁻²

Question 11

What are the units for Kc if there is two more on the top than the bottom?

Answer 11

mol² dm⁻⁶

Question 12

What is the one thing that affects Kc?

Answer 12

Temperature

Question 13

What happens to the rate of the forward reaction when a reactant is added to a system in equilibrium?

Answer 13

The rate of the forward reaction will increase to use up all the added material and restore equilibrium

Question 14

What happens to the value of K when a reactant is added to a system in equilibrium?

Answer 14

It remains the same

Only temperature can change it

Question 15

What happens to the amount of product produced when a reactant is added to a system in equilibrium?

Answer 15

More product is produced

Question 16

Does the concentration of products and reactants have to be the same for it to be at equilibrium?

Answer 16

No as long as the forward reaction is occuring at the same rate as the backwards reaction it is in equilibrium

Question 17

What does a high value of Kc mean?

Answer 17

The position of equilibrium is further to the right

Question 18

What does a catalyst do in a reversible reaction?

Answer 18

Speeds up the rate of both the backwards and the forwards reaction. Doesn’t effect position of equilibrium but gets to equilibrium quicker

Question 19

If the forward reaction is endothermic what is the backwards reaction?

Answer 19

Exothermic

Question 20

If the forward reaction is exothermic what is the backwards reaction?

Answer 20

Endothermic

Question 21

If the system is heated and the forward reaction is endothermic what happens to the rate of the forward and backward reaction?

Answer 21

Both increase but the forward reaction increases by more because it is endothermic (+ve, takes in heat)

Question 22

How do you work out concentration?

Answer 22

Moles / Volume

Question 23

What isn’t included when working out Kc?

Answer 23

Solids or liquids

Question 24

What is the definition of partial pressure?

Answer 24

The pressure a gas would if it were on it’s own

Partial pressure = total pressure X mole fraction

Question 25

How do you work out the power to which P is in the Kp equation?

Answer 25

It is the same as the number of moles in the overall balanced equation

Question 26

What is partial pressure measured in?

Answer 26

Pa

Question 27

What are the units for Kp if there are 1 more on the top than the bottom?

Answer 27

Pa

Question 28

What are the units for Kp if there are 2 more on the top than the bottom?

Answer 28

Pa²

Question 29

What are the units for Kp if there are 1 more on the bottom than the top?

Answer 29

Pa⁻¹

Question 30

What are the units for Kp if there are 2 more on the bottom than the top?

Answer 30

Pa⁻²

Question 31

How do you work out the mole fraction of a gas?

Answer 31

Number of moles of that gas / Total number of moles of all the gases

Question 32

How do you work out the partial pressure?

Answer 32

Mole fraction X total pressure

Question 33

How do you work out the total pressure?

Answer 33

Add together all the partial pressures

Question 34

How do you work out Kp?

Answer 34

Partial pressure of products / partial pressure of reactants

Question 35

What is a homogeneous equilibria?

Answer 35

When all reactants and products in a reaction are in the same state.

Question 36

What is a heterogeneous equilibria?

Answer 36

When some reactants and products in a reaction are in different states.

Question 37

What does the sum of the mole fractions equal?

Answer 37

1

Question 38

What is Le Chatelier's principle?

Answer 38

When a system in equilibrium is subjected to an external change, the system readjusts itself to oppose/minimise the effects of the change

Question 39

How does increasing pressure affect the position of equilibrium?

Answer 39

Shifts equilibrium to side with fewer moles of gas

Question 40

How does increasing temperature affect the position of equilibrium?

Answer 40

Shifts equilibrium in endothermic (+ve) direction