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Advanced Higher Chemistry > Unit 2 - Physical Chemistry > Flashcards

Unit 2 - Physical Chemistry Flashcards

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1
Q

What is chemical equilibrium

A

When concentration of reactants and products remains constant over time

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2
Q

Equilibirum must take place in a 1 system

A

Closed

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3
Q

What is a closed system

A

Species in solution can not escape to environment

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4
Q

What is a stable equilibrium

A

Usually minimum E state

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5
Q

Whats a dynamic equilibrium

A

Where concentration of reactants and products remain the same but the individual molecules/ ions are moving from one side of the euqation to the other side

Forward and reverse are equal

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6
Q

K > 1 = (1)

K < 1 = (2)

A

1 product favoured

2 reactant favoured

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7
Q

What happens to Kc when heat is added to an expthermic reaction

A

Decrease

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8
Q

What happens to Kc if heat is added to an endothermic reaction

A

Increase

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9
Q

What reavtion is favoured when heat is added to an exothermic reaction

A

Reverse reaction

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10
Q

What reaction eill be favoured if heat is added to an endothermic reaction

A

Forward reaction

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11
Q

Acids= H+ donors/acceptors

A

Donors

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12
Q

Bases= H+ donor/acceptor

A

Acceptor

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13
Q

For every acid there is a (1)

A

Conjugated base

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14
Q

For every base there is a (2)

A

Conjugated acid

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15
Q

H2O is amphoteric which means..

A

It can accept and donate protons

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16
Q

Why is water a poor conductor of electricity

A

Because it doesnt dissociate very much

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17
Q

What is Kw

A

Ionic product of water

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18
Q

What is Ke dependent on

A

Temperature

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19
Q

In pure water, H+ and OH- are

A

Equal

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20
Q

Do strong bases and acids dissociate completely or partially

A

Completely

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21
Q

Examples of strong acids

A

HCL, HBr, Hl, HNO3, H2SO4

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22
Q

What does ph depend on for strong acids

A

Initial molarity of the acid

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23
Q

What are common strong bases

A

Oxides, hydroxides of group 1 metals

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24
Q

What does [OH-], [H+] and pH depend on for strong bases

A

Initial molarity of base

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25
Q

Is Ka large/small for strong acids

A

Large

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26
Q

Why is Ka large for strong acids

A

Because they dissociate completely

27
Q

Pka for strong acids is

A

Small

28
Q

Pka for wear acids is

A

Large

29
Q

Pka for weak conjugated base is

A

Small

30
Q

Pka for strong conjugated base is

A

Large

31
Q

Strong acids and bases dissociate (1) in awueous solutions

A

Completely

32
Q

Weak acids and bases dissociate (2) in aqueous solutions

A

Partially

33
Q

What does ph in a salt solution depend on

A

Relative strength of parent acid and base

34
Q

Strong acid + strong base =

A

Neutral

35
Q

Weak acid + strong base =

A

Alkaline

36
Q

Strong acid + weak base =

A

Acidic solution

37
Q

Whats a buffer solution

A

A solution in which the ph remains approximately constant when small amounts of water (acid) base are added

38
Q

Whats an acid buffer

A

Solution if weak acid + on eof its salts

39
Q

Whats a basic buffer

A

Solution of weak base + one of its salts

40
Q

What must a buffer be able to do in order to stabalise ph

A

Absorb extra acid or alkali

41
Q

How does an acid buffer work

A

Weak acid provides H+ and when these are removed by the addition of small amounts of base.

The salt of the weak acid provides the conjugated base which can absorb exess H+ produced bt addition of a small amount if acid

42
Q

What are indicators

A

Dyes ehose colours are sensitive to pH

43
Q

What can indicators be used for

A

Determine the end point of an acid - base titration

44
Q

What is thermochemistry

A

The study of chages in E that occur in chemical reactions

45
Q

What does reaction feasibility depend on

A

Enthalpy
Temp
Entropy

46
Q

What is the standard enthalpy of formation

A

Enthalpy change when one mole of substance us formed from its elements un their standard states

47
Q

Whats the standard state of a substance

A

Its most stable state at a pressure of 1 atm and a specific T

48
Q

Whats the standard enthalpy

A

Can be calculated form the standard enthalpies of formation of the reactants and products

49
Q

Whats entropy

A

Degree of disorder of a system

50
Q

Increased disorder= 1 entropy

A

Increased

51
Q

Solids have high/low disorder

A

Low

52
Q

Gases have high/low disorder

A

High

53
Q

Why do gases have a higher entropy than solids

A

Because gases can move more freely while solid particles are limited to vibration

54
Q

What do state changes do to entropy

A

Large changes in entropy

55
Q

Whats the 2nd law of thermodynamics

A

The total entropy of a reaction system and its surroundings always increases for a spontanious process

56
Q

Heat energy released into surroundings

A

Increased S of surroundings

57
Q

Heat energy absorbed from surroundings

A

Decreased S of surroundings

58
Q

Whats the standard entropy of a substance

A

Entropy value for the substance in uts standard state

59
Q

Whats a feasible reaction

A

One that tends towards the product rather than the reactants

60
Q

What needs to happen for a reaction to be feasible at given T

A

Must happen spontaneously

61
Q

What happens when a reaction occurs spontaneously

A

No extra energy needed for reaction to occur

62
Q

What do kinetics describe

A

The rate of chemical reactions

63
Q

What is the rate determining step

A

Step which is the slowesr and therefore contributes the most to the rate

Advanced Higher Chemistry (4 decks)

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