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Chemistry Module 5 > How far > Flashcards

How far Flashcards

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1
Q

How is the equilibrium constant denoted?

A

K

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2
Q

What are the units for concentration?

A

moldm⁻³

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3
Q

What brackets are used in then Kc equation?

A

[square brackets]

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4
Q

How do you work out Kc?

A

Concentration of products / concentration of reactants

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5
Q

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

A

However many moles are in the overall balanced equation

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6
Q

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

A

X

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7
Q

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

A

X

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8
Q

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

A

dm³mol⁻¹

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9
Q

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

A

mol dm⁻³

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10
Q

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

A

dm⁶ mol⁻²

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11
Q

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

A

mol² dm⁻⁶

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12
Q

What is the one thing that affects Kc?

A

Temperature

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13
Q

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

A

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

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14
Q

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

A

It remains the same

Only temperature can change it

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15
Q

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

A

More product is produced

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16
Q

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

A

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

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17
Q

What does a high value of Kc mean?

A

The position of equilibrium is further to the right

18
Q

What does a catalyst do in a reversible reaction?

A

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

19
Q

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

A

Exothermic

20
Q

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

A

Endothermic

21
Q

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

A

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

22
Q

How do you work out concentration?

A

Moles / Volume

23
Q

What isn’t included when working out Kc?

A

Solids or liquids

24
Q

What is the definition of partial pressure?

A

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

Partial pressure = total pressure X mole fraction

25
Q

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

A

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

26
Q

What is partial pressure measured in?

A

Pa

27
Q

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

A

Pa

28
Q

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

A

Pa²

29
Q

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

A

Pa⁻¹

30
Q

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

A

Pa⁻²

31
Q

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

A

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

32
Q

How do you work out the partial pressure?

A

Mole fraction X total pressure

33
Q

How do you work out the total pressure?

A

Add together all the partial pressures

34
Q

How do you work out Kp?

A

Partial pressure of products / partial pressure of reactants

35
Q

What is a homogeneous equilibria?

A

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

36
Q

What is a heterogeneous equilibria?

A

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

37
Q

What does the sum of the mole fractions equal?

A

1

38
Q

What is Le Chatelier’s principle?

A

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

39
Q

How does increasing pressure affect the position of equilibrium?

A

Shifts equilibrium to side with fewer moles of gas

40
Q

How does increasing temperature affect the position of equilibrium?

A

Shifts equilibrium in endothermic (+ve) direction

Chemistry Module 5 (8 decks)

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