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11E > 7.4 Rates of Reaction > Flashcards

7.4 Rates of Reaction Flashcards

1
Q

How can you measure the rate of a reaction?

A

The rate at which a reactant is used up, The rate at which a product is formed

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2
Q

Name 2 factors which can affect the rate of a reaction.

A

Temperature/pressure/concentration/SA/ catalysts

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3
Q

What has to happen to particles for a reaction to occur?

A

Collide with enough energy

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4
Q

Define the term activation energy.

A

The amount of energy required for them to react

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5
Q

How can you measure the rate of a reaction when a solid dissolves?

A

Mass of substance used up

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6
Q

How can you measure the rate of a reaction when a gas is given off?

A

Volume of gas given off

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7
Q

What are the units for rate of reaction?

A

g/s orcm3/s or mol/s

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8
Q

Which variable is plotted on the x-axis of a rate graph?

A

Independent / Time

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9
Q

What variable can be found on the y-axis of a rate graph?

A

Dependent / Amount of product formed or amount of reactant used

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10
Q

How can you calculate the average rate across a period of time?

A

Change in Y / Change in X

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11
Q

What is a tangent?

A

A tangent is a straight line drawn on a curve

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12
Q

What information does a tangent provide?

A

The rate of reaction at a specific point

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13
Q

What does it mean when the curve on a rate graph gets steeper?

A

The rate of reaction is increasing

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14
Q

What does it mean when the curve on a rate graph gets shallower?

A

The rate of reaction is decreasing

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15
Q

How can you tell that a reaction has finished from a rate graph?

A

The line becomes constant/ horizontal

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16
Q

What is the rate of reaction?

A

The rate of a reaction is how quickly the products are being made

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17
Q

Name 2 factors that affect the rate of a reaction.

A

Temperature/concentration/SA/pressure

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18
Q

What is the scientific term for movement energy?

A

Kinetic Energy

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19
Q

When temperature is increased what energy store increases in the particles?

A

Thermal Energy

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20
Q

What does the term activation energy mean?

A

The minimum amount of energy that the reactant particles must collide with to cause the reaction to occur

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21
Q

How does increasing temperature increase the rate of a reaction?

A

The particles have more kinetic energy

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22
Q

How does increasing pressure increase the rate of a reaction?

A

The particles are closer together and so more likely to collide

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23
Q

How does increasing surface area increase the rate of a reaction?

A

There are more reactants available to react

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24
Q

Define the term activation energy.

A

The amount of energy needed for a reaction to occur

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25
Q

What does a reaction profile show?

A

The energy changes during a chemical reaction

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26
Q

In an endothermic reaction- which has higher energy, reactants or products?

A

Products

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27
Q

In an exothermic reaction- which has higher energy, reactants or products?

A

Reactants

28
Q

Is energy absorbed or released when new bonds are made?

A

Released

29
Q

Is energy absorbed or released when bonds are broken?

A

Absorbed

30
Q

What decides if a reaction is exothermic or endothermic?

A

The difference in energy needed to break bonds and the energy released when new bonds form

31
Q

What equipment could you use to tell if a reaction is exothermic or endothermic?

A

Thermometer

32
Q

What is a catalyst?

A

A substance which increases the rate of a chemical reaction without being used up itself.

33
Q

How does a catalyst increase the rate of a reaction?

A

Provides an alternate pathway for the reaction to occur

34
Q

What is an enzyme?

A

A biological catalyst

35
Q

What are enzymes made from?

A

Proteins

36
Q

Why is the shape of the active site of an enzyme important?

A

Complimentary to the substrate

37
Q

What is the ‘lock and key’ model?

A

The enzyme and substrate have specific complementary shapes

38
Q

Name 2 factors that can affect the effectiveness of an enzyme.

A

Temperature and pH

39
Q

What are conditions in the human stomach like?

A

Acidic

40
Q

What is a reversible reaction?

A

A reaction that can produce products, but the products can also react to create the reactants

41
Q

What is a dynamic equilibrium?

A

The forward and backward reaction occur at the same rate?

42
Q

HT: In which direction does an equiliubrium shift if temperature is increased?

A

In the endothermic direction

43
Q

HT: In which direction does an equiliubrium shift if temperature is decreased?

A

In the exothermic direction

44
Q

HT: In which direction does an equiliubrium shift if pressure is increased?

A

In the direction of fewer particles

45
Q

HT: In which direction does an equiliubrium shift if pressure is decreased?

A

In the direction of more particles

46
Q

HT: In which direction does an equiliubrium shift if concentration of reactants is increased?

A

In the direction of the products

47
Q

HT: In which direction does an equiliubrium shift if concentration of products is increased?

A

In the direction of the reactants

48
Q

What colour change would you expect to see when iodine is added to starch?

A

From brown to blue - black

49
Q

Why does increasing surface area increase the rate of a chemical reaction?

A

It increases the available particles for the reaction

50
Q

Why does increasing temperature increase the rate of a chemical reaction?

A

It increases the energy of the particles

51
Q

What is a tangent?

A

A straight line drawn on a curve

52
Q

How does a catalyst increase the rate of reaction?

A

Gives the reaction an alternate pathway and increases the rate.

53
Q

What term matches this definition? Energy required to start a reaction

A

Activation energy

54
Q

What term matches this definition? Part of an enzyme where the substrate becomes a product

A

Active site

55
Q

What term matches this definition? The chemical energy stored in the bonds between atoms

A

Bond energy

56
Q

What term matches this definition? Substance which speeds up a reaction

A

Catalyst

57
Q

What term matches this definition? Particles must collide to cause a reaction

A

Collision theory

58
Q

What term matches this definition? Forward and backwards reactions occur at the same rate

A

Dynamic equilibrium

59
Q

What term matches this definition? Reaction which absorbs energy from the surroundings

A

Endothermic

60
Q

What term matches this definition? A biological catalyst

A

Enzyme

61
Q

What term matches this definition? Reaction which releases energy to the surroundings

A

Exothermic

62
Q

HT: What term matches this definition? Dynamic equilibrium can shifts due to external factors

A

Le Chatelier’s principle

63
Q

What term matches this definition? Model which explains how enzymes are specific to their substrate

A

Lock and key model

64
Q

What term matches this definition? Diagram to show the energy changes during a reaction

A

Reaction profile

65
Q

What term matches this definition? Reaction where products can react to produce the reactants

A

Reversible reaction

66
Q

What term matches this definition? The substance an enzyme works on

A

Substrate

67
Q

What term matches this definition? The ratio of surface area to volume

A

Surface area:volume

11E (24 decks)

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