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Chemistry - Year 12 > Module 5: Equilibrium and Acid Reactions > Flashcards

Module 5: Equilibrium and Acid Reactions Flashcards

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1
Q

What is entropy?

A

It is the measure of number of possible arrangements of a system

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2
Q

When can entropy increase?

A

When the volume increase, number of particles increases, temperature increases or there is a change in state

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3
Q

What is a spontaneous reaction?

A

Is a reaction that occurs on its own accord

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4
Q

When is a reaction spontaneous?

A

ΔG < 0

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5
Q

When is a reaction not spontaneous?

A

ΔG > 0

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6
Q

When is a reaction at equilibrium?

A

ΔG = 0

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7
Q

How do you calculate gibbs free energy?

A

ΔG = ΔH - TΔS

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8
Q

When is a reaction always spontaneous according to S and H?

A

ΔH < 0 (Exothermic) and TΔS > 0 (increase in entropy)

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9
Q

When is a reaction never spontaneous according to S and H?

A

ΔH > 0 (Endothermic) and TΔS < 0 (decrease in entropy)

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10
Q

When is a reaction spontaneous at high temperatures according to S and H?

A

ΔH > 0 (Endothermic) and TΔS > 0 (increase in entropy)

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11
Q

When is a reaction spontaneous at low temperatures according to S and H?

A

ΔH < 0 (Exothermic) and TΔS < 0 (decrease in entropy)

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12
Q

What are irreversible reactions?

A

Are reactions which occur in one direction

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13
Q

What are some examples of irreversible reactions?

A

Baking a cake
Combustion reactions
Combustion of magnesium and iron wool

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14
Q

What are reversible reactions?

A

Are reactions where the products formed can react again and reform the reactants

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15
Q

What are some examples of reversible reactions?

A

Evaporation and condensation of water
Formation of saturated sugar solution
Reaction between de/hydrated cobalt (II) chloride
Reaction between iron (III) nitrate and potassium thiocyanate

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16
Q

When is equilibrium reached in the evaporation and condensation of water?

A

When the rate of evaporation is equal to the rate of condensation

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17
Q

What colour is dehydrated cobalt (II) chloride?

A

Blue

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18
Q

What colour is hydrated cobalt (II) chloride?

A

Pink

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19
Q

What colour is a solution of iron (III) nitrate?

A

Pale yellow

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20
Q

What colour is a solution of potassium thiocyanate?

A

Colourless

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21
Q

What colour is iron (III) thiocyanate?

A

Deep red

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22
Q

What is chemical equilibrium?

A

When both reactants and products are in concentrations which have no further tendency to change with time

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23
Q

What is dynamic equilibrium?

A

When the rate of forward reaction and the rate of reverse reaction is equal

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24
Q

What is the Haber process?

A

The production of ammonia from hydrogen gas and nitrogen gas

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25
Q

What is the extent of a reaction?

A

It is how much product has been formed when equilibrium is met

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26
Q

What are the three factors which affect collision theory?

A
  1. Frequency of collisions
  2. Orientation of the particles
  3. Whether there is sufficient energy to break chemical bonds
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27
Q

What is static equilibrium?

A

When the rate of forward reaction and reverse reaction is almost zero

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28
Q

What is an example of static equilibrium?

A

carbon (graphite) <—-> carbon (diamond)

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29
Q

What are non-equilibrium systems?

A

Reactions that never reach an equilibrium and are irreversible

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30
Q

What are some examples of non-equilibrium systems?

A

Combustion and photosynthesis

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31
Q

What is Le Chatelier’s principle?

A

If an equilibrium system is subjected to a change or disturbance in conditions, the system will adjust itself to counteract and minimise the effect of change

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32
Q

How does increase in concentration of reactants impact equilibrium?

A

Forward reaction is favoured, equilibrium shifts to the right

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33
Q

How does increase in concentration of products impact equilibrium?

A

Reverse reaction is favoured, equilibrium shifts to the left

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34
Q

How does increase in pressure impact equilibrium?

A

Causes the equilibrium to shift towards the direction with less number of moles

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35
Q

How does decrease in pressure impact equilibrium?

A

Causes the equilibrium to shift towards the direction with more number of moles

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36
Q

How does decrease in volume impact equilibrium?

A

(Increases pressure) Causes the equilibrium to shift towards the direction with less number of moles

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37
Q

How does increase in volume impact equilibrium?

A

(Decrease pressure) Causes the equilibrium to shift towards the direction with more number of moles

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38
Q

When is a reaction exothermic?

A

ΔH = -ve

39
Q

Which side is the energy on for exothermic reactions?

A

Product side

40
Q

When is a reaction endothermic?

A

ΔH = +ve

41
Q

Which side is the energy on for endothermic reactions?

A

Reactant side

42
Q

How does increase of temperature impact equilibrium?

A

Causes the equilibrium to shift towards the direction which does not produce energy to use up the extra energy

43
Q

How does decrease of temperature impact equilibrium?

A

Causes the equilibrium to shift towards the direction which produces energy to make up for the lost energy

44
Q

What does a rate vs time graph look like?

A

Forward rate decreases, reverse rate increases until they meet in the middle

45
Q

What does an amount vs time graph look like?

A

Reactants and products increase and decrease until they are both straight lines

46
Q

What does a sharp peak on one chemical mean on a concentration equilibrium graph?

A

Change in concentrations

47
Q

What does a sharp peak of all chemicals mean on a concentration equilibrium graph?

A

Change in pressure or volume

48
Q

What does a smooth peak of all chemicals mean on a concentration equilibrium graph?

A

Change in temperature

49
Q

How do you remember the equilibrium constant equation?

A

PORK
product over reactant = Keq

50
Q

What is the symbol of equilibrium constant?

A

Keq

51
Q

What does the Keq indicate?

A

The equilibrium position

52
Q

What does it mean if the Keq is greater than 1?

A

Equilibrium tends towards the products (right)

53
Q

What does it mean if the Keq is smaller than 1?

A

Equilibrium tends towards the reactants (left)

54
Q

What does it mean if the Keq is very large?

A

The reaction is near completion

55
Q

What does it mean if the Keq very small?

A

The forward reaction hardly occurs

56
Q

What is the only thing that can impact Keq?

A

Temperature

57
Q

When is the Keq accurate?

A

When a system is at equilibrium

58
Q

What is reaction quotient?

A

When the equilibrium expression is different to Keq

59
Q

What is the symbol for the reaction quotient?

A

Q

60
Q

What reaction favoured if Q>Keq?

A

The reverse reaction

61
Q

What reaction favoured if Q<Keq?

A

The forward reaction

62
Q

What reaction favoured if Q=Keq?

A

The system is at equilibrium

63
Q

What are the only things considered when calculating Q?

A

Gases and aqueous solutions

64
Q

How does an increase of temp impact Keq of endothermic reactions?

A

Favours forward reaction hence Keq value increases

65
Q

How does a decrease of temp impact Keq of endothermic reactions?

A

Favours reverse reaction hence Keq value decreases

66
Q

How does an increase of temp impact Keq of exothermic reactions?

A

Favours reverse reaction hence Keq value decreases

67
Q

How does a decrease of temp impact Keq of an exothermic reactions?

A

Favours forward reaction hence Keq value increases

68
Q

What is the structure of water?

A

2 hydrogen bonds covalently bond to an oxygen atom

69
Q

Are the covalent bonds in water polar or non-polar?

A

Polar

70
Q

What bonds exist between water molecules?

A

Hydrogen bonds

71
Q

When is a substance soluble?

A

When more than 0.1 mol of it will dissolve in 1L of water at 25*C

72
Q

When is a substance insoluble?

A

When less than 0.01 mol of it will dissolve in 1L of water at 25*C

73
Q

When is a substance slightly soluble?

A

When 0.01-0.1 mol of it will dissolve in 1L of water at 25*C

74
Q

What does SNAAP stand for?

A

Sodium
Nitrate
Ammonium
Acetate
Potassium

75
Q

What are the SNAAP salts?

A

Salts which are soluble

76
Q

What is the solubility product?

A

Is the product of the concentration of ions in a saturated solution of a insoluble salt

77
Q

What does Ksp include?

A

Only aqueous solutions

78
Q

What is the ionic product?

A

The product of the concentration of ions in any solution

79
Q

When is a solution saturated?

A

When the ionic product = Ksp

80
Q

How does Ksp show solubility?

A

The bigger the Ksp the more soluble it is

81
Q

When will a precipitate not form?

A

Ionic product < Ksp

82
Q

When will a precipitate form?

A

Ionic product > Ksp

83
Q

Why is the undissolved solid not included in the Ksp calculation?

A

As it remains constant and there is no change in concentration

84
Q

What is Kc?

A

It is like the Keq

85
Q

What happens to the Kc when all moles are halved, doubled, tripled etc?

A

Kc to the power of what happened
eg if halved Kc to the power of half

86
Q

What happens to the Kc when the reaction is reversed?

A

It will be Kc to the power of a negative

87
Q

What is Kp and how do you calculate it?

A

It is the equilibrium constant based on pressure and it is calculated the same way as Keq but with the pressures

88
Q

How to calculate Ksp from molar solubility?

A
  1. Write balanced equation A ⇌ B + C
  2. Ksp = [B][C]
  3. Substitute molar solubility in and if required multiply by the number of ions produced
89
Q

What is a homogeneous equilibrium?

A

Is a reaction where all of the products and reactants are the same state

90
Q

What is a heterogeneous equilibrium?

A

Is when there are different states in the reaction

91
Q

Is the self-ionisation of water exothermic of endothermic?

A

Endothermic

92
Q

How do you find concentration from Ksp?

A

Use a rice table and solve for x

93
Q

Is the statement [H3O+] = [OH-] always true?

A

Yes at all temperatures pure water will always have [H3O+] = [OH-]

94
Q

How does the addition of a catalyst affect a reversible reaction?

A

It decreases the activation energy of both the forward and reverse reaction

Chemistry - Year 12 (5 decks)

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