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Year 12 > Chemistry Unit 3 > Flashcards

Chemistry Unit 3 Flashcards

1
Q

Chemical equilibrium

A

when the rate of forward reaction = rate of reverse reaction and the concentration of reactants remain unchanged

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2
Q

Dynamic equilibrium

A

rate of forward reaction = rate of reverse reaction

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3
Q

Extent of reaction

A

how much of a product is formed when a system reaches equilibrium

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4
Q

(⇌)

A

a reversible process

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5
Q

Reversible reactions occur

A

simultaneously in both directions

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6
Q

Relative ratio of reactants to products at equilibrium

A

different for different reactions

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7
Q

Rate of reaction

A

a measure of the change in concentration of reactants over time

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8
Q

In a closed system

A

only energy is exchanged with surroundings

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9
Q

In an open system

A

both energy and matter are exchanged with surroundings

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10
Q

Irreversible reaction

A

products cannot react together to be converted back into reactants

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11
Q

Position of equilibrium can be modified by

A

adding or removing a product/reactant, change in pressure, concentration or temperature

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12
Q

Le Chatelier’s Principle

A

when a stress is applied to a system in a state of equilibrium, the system reacts in a way to reduce the stress

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13
Q

At equilibrium, the concentrations of products and reactants

A

remain the same unless a stress is applied to the system

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14
Q

Examples of added stress to a system:

A

add/remove a chemical, increase/decrease in pressure or temperature

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15
Q

If a chemical added to a system

A

the system shifts away from the chemical and vice versa

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16
Q

If pressure is added to a system

A

the system will shift to the side with the least number of gas particles and vice versa

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17
Q

Heating an exothermic reaction

A

system shifts to the left, favouring the reactants as high energy, and giving more energy to product particles to overcome activation barriers

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18
Q

Heating an endothermic reaction

A

system shifts to the right, favouring the products as high energy, and giving more energy to reactant particles to overcome activation barriers

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19
Q

Pressure (Pa) =

A

force (N) / area (m^2)

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20
Q

Higher temperatures

A

more particle movement and increased collisions

21
Q

Lower temperatures

A

less particle movement and decreased collisions

22
Q

Increased pressure

A

increased collisions and faster forward rate of reactions

23
Q

Increasing pressure by adding an inert gas

A

The concentration of reactants and products is not changed nor is equilibrium affected

24
Q

Increasing concentration in collision theory

A

Equal to increasing pressure

25
Q

Diluting a liquid

A

spreading out particles to decrease pressure

26
Q

Adding water particles

A

reduces the number of particles per volume, lowering the concentration and shifting the equation left

27
Q

Adding dilute

A

the concentration drops, but will rise again as the products are broken down faster than they can be formed

28
Q

Decreasing concentration

A

decreases number of collisions and slows the forward rate of reaction

29
Q

Catalysts do not

A

change the position of equilibrium or ratio of products to reactants

30
Q

Catalysts do

A

help achieve equilibrium faster

31
Q

Bronsted-Lowry Model of Acids and Bases

A

explains the relationship between acids and bases in equilibrium systems

32
Q

Acid (Bronsted-Lowry)

A

the proton (hydrogen-ion) donor

33
Q

Base (Bronsted-Lowry)

A

the proton (hydrogen-ion) recipient

34
Q

Conjugates (Bronsted-Lowry)

A

the base will always have a conjugate acid and vice versa

35
Q

Conjugate Acid

A

the particle formed when a base gains a hydrogen-ion

36
Q

Conjugate Base

A

the particle formed when an acid has donated a hydrogen-ion

37
Q

Conjugate Acid-Base Pair

A

two substances that are related by the loss/gain of a single hydrogen-ion

38
Q

Hydronium Ion

A

the positive ion formed when a water molecule gains a hydrogen-ion

39
Q

Amphoteric

A

a substance that can act as an acid and a base

40
Q

Monoprotic acids

A

any acid that contains one ionizable proton

41
Q

Diprotic acids

A

any acid that contains two ionizable protons

42
Q

Triprotic acids

A

any acid that contains three ionizable protons

43
Q

Strength of an acid or base

A

depends on how much it ionizes in water

44
Q

Concentration of an acid of base

A

depends on how many moles per volume

45
Q

Strong acids

A

completely ionise in aqueous solution, fully dissociate, 100% ionised

46
Q

Weak acids

A

slightly ionise in aqueous solution, partially dissociate, 1% ionised

47
Q

Buffer solutions

A

resist changes in pH when an acid or base is added to it

48
Q

Strong bases

A

fully dissociate

49
Q

Weak bases

A

partially dissociate

Year 12 (1 decks)

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