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Rates of Reaction

Total questions: 90

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

2.

Grinding a effervescent tablet into powder increases the rate of reaction due to increased

a)

concentration

b)

surface area

c)

temperature

d)

reactants

3.

Adding a catalyst ___________ the activation energy.

a)

Raises

b)

Lowers

c)

Doesn't affect

d)

Inreases

4.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

5.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)
b)
c)
d)
6.
The graph shows how the total volume of a gas given off from a reaction changes with time. In which time interval is least gas given off? 
a)
A
b)
B
c)
C
d)
D
7.
In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulphuric acid. The solid line on the graph shows the volume of gas given off when the 2 g lump is used. Which dotted line is obtained when the zinc is powdered? 
a)
A
b)
B
c)
C
d)
D
8.
A student investigated the rate of reaction of calcium carbonate with dilute hydrochloric acid. Every minute, the student recorded the total volume of carbon dioxide produced, until some time after the reaction was complete.
Which graph shows the correct results? 
a)
A
b)
B
c)
C
d)
D
9.
Order the letters from highest to lowest rate of reaction.
a)
A > B > C > D
b)
A > BC > D (B and C have the same rate)
c)
A > B > CD (C and D have the same rate)
d)
D > C > B > A
10.
Why does a catalyst increase the rate of reaction?
a)
it produces extra energy for the reactants
b)
it increases the speed of the reactant particles
c)
it increases the frequency of particle collisions
d)
it reduces the activation energy of the reaction 
11.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
12.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

13.

The major theory of reaction rate is called

a)

Collision theory

b)

Crash theory

c)

Newton's laws

d)

Thermodynamics

14.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
15.
What does NOT happen when the temperature is increased?
a)
Particles collide more often
b)
Particles collide with more energy
c)
Particles move faster
d)
More particles collide in the correct orientation
16.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
17.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
18.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
19.

Which factors affect the rate of a reaction?

a)

temperature

b)

concentration

c)

surface area

d)

pressure

e)

catalyst

20.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

21.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

22.

Grinding a effervescent tablet into powder increases the rate of reaction due to increased

a)

concentration

b)

surface area

c)

temperature

d)

reactants

23.

Increasing the temperature gives particles more __________.

a)

Time

b)

Energy

c)

Space

d)

Frequency

24.

As the frequency of ______________ increases, the rate of reaction increases.

a)

Time

b)

Reactions

c)

Collisions

d)

Reactants

25.

Adding a catalyst ___________ the activation energy.

a)

Raises

b)

Lowers

c)

Doesn't affect

d)

Inreases

26.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

27.

Substance that changes the rate of a chemical reaction without being consumed in the reaction

a)

bonding

b)

catalyst

c)

chemical reaction

d)

activation energy

28.
What method can NOT be used to collect gas?
a)
Using a gas syringe
b)
Collecting it in a measuring cylinder under water
c)
Measuring the change in mass
d)
Seeing how quickly the solution goes cloudy
29.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)
b)
c)
d)
30.

P, Q, R and S are pieces of apparatus.

Which row describes the correct apparatus for the measurement made?

a)

A

b)

B

c)

C

d)

D

31.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
32.
The graph shows how the total volume of a gas given off from a reaction changes with time. In which time interval is least gas given off? 
a)
A
b)
B
c)
C
d)
D
33.
In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulphuric acid. The solid line on the graph shows the volume of gas given off when the 2 g lump is used. Which dotted line is obtained when the zinc is powdered? 
a)
A
b)
B
c)
C
d)
D
34.

Icing sugar has a greater ______ _____ than a solid cube of

sugar.

a)

Surface Area

b)

Catalyst

c)

Temperature

35.
A solution of hydrogen peroxide releases oxygen slowly at room temperature.
 hydrogen peroxide → water + oxygen
 The diagrams show the effect of adding blood to the solution. What could be the reason for the observed change? 
a)
Blood contains an enzyme. 
b)
Blood contains water. 
c)
The hydrogen peroxide becomes more concentrated. 
d)
The hydrogen peroxide is neutralised by blood. 
36.
A liquid X reacts with solid Y to form a gas.
Which two diagrams show suitable methods for investigating the speed of the reaction? 
a)
1 and 3
b)
1 and 4
c)
2 and 3
d)
2 and 4
37.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
38.
A student investigated the rate of reaction of calcium carbonate with dilute hydrochloric acid. Every minute, the student recorded the total volume of carbon dioxide produced, until some time after the reaction was complete.
Which graph shows the correct results? 
a)
A
b)
B
c)
C
d)
D
39.
Identify where the reaction has finished
a)
A
b)
B
c)
C
d)
D
40.
Order the letters from highest to lowest rate of reaction.
a)
A > B > C > D
b)
A > BC > D (B and C have the same rate)
c)
A > B > CD (C and D have the same rate)
d)
D > C > B > A
41.
Identify the part of the graph with the fastest rate of reaction.
a)
A
b)
B
c)
C
d)
D
42.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

43.

Grinding a effervescent tablet into powder increases the rate of reaction due to increased

a)

concentration

b)

surface area

c)

temperature

d)

reactants

44.

Adding a catalyst ___________ the activation energy.

a)

Raises

b)

Lowers

c)

Doesn't affect

d)

Inreases

45.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

46.
The graph shows how the total volume of a gas given off from a reaction changes with time. In which time interval is least gas given off? 
a)
A
b)
B
c)
C
d)
D
47.
Why does a catalyst increase the rate of reaction?
a)
it produces extra energy for the reactants
b)
it increases the speed of the reactant particles
c)
it increases the frequency of particle collisions
d)
it reduces the activation energy of the reaction 
48.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
49.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
50.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

51.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

52.

How is this equipment being used to measure the rate of reaction?

a)

The gas syringe measures how much gas is produced in a certain time

b)

The reaction mixture will increase in volume in a certain time

53.

The rates of some chemical reactions can be measured by using the apparatus shown. For which reaction is this apparatus suitable?

a)

MgCO3 + 2HCl -> MgCl2 + CO2 + H2O

b)

Mg + ZnCl2 -> MgCl2 + Zn

c)

MgCl2 + 2NaOH -> Mg(OH)2 + 2NaCl

d)

MgO + 2HCl -> MgCl2 + H2O

54.

When you react sodium thiosulfate and hydrochloric acid, the solution turns cloudy. This is because...

a)

a sodium precipitate is produced

b)

a sulfur precipitate is produced

55.

Which solution show a higher concentration (left or right)?

a)

left

b)

right

c)

both the same

56.

The more concentrated the sodium thiosulfate solution, the less time is taken for the cross to become no longer visible. Give two reasons why.

a)

Particles are more spread out

b)

Particles collide more frequently

c)

Particles have more energy

d)

Particles move more quickly

e)

There are more particles in a fixed volume

57.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

58.

The rate of a reaction is described as the speed at which the amount of reactants decreases or the amount of ______ increases

a)

reagents

b)

gases

c)

products

d)

metals

59.

The rate of a reaction can be calculated as the change in concentration, volume or mass divided by _________

a)

time

b)

mass

c)

moles

d)

rate

60.

When acid is reacted with calcium carbonate the volume of carbon dioxide released is recorded, what equipment could be used to record the volume of gas? (pick all correct answers)

a)

A pipette

b)

A burette

c)

A gas syringe

d)

A measuring cylinder submerged in water

61.

Which line represents a higher initial rate of reaction?

a)

1

b)

2

c)

They both have the same initial rate

62.

As the reaction progresses both lines plateau, why is this the case?

a)

The rate of reaction is at a constant high rate

b)

The reaction has reached the maximum rate

c)

The reaction has stopped and no more carbon dioxide is produced.

63.

What might cause the difference between line 1 and 2?

a)

Reaction 1 contains a solid with a higher surface area than the solid in reaction 2

b)

Reaction 1 is carried out at a higher temperature than reaction 2

c)

Reaction 1 uses a catalyst and reaction 2 does not.

d)

Reaction 1 has a greater number of moles of reactants than reaction 2.

64.

Substances which are powdered will react faster, this is because...

a)

A smaller surface area of solid will result in more frequent successful collisions

b)

A larger surface area of solid will result in more frequent successful collisions

c)

A larger surface area of solid will result in the particles having higher energy and therefore more particle will have the required activation energy.

d)

A smaller surface area of solid will result in the particles having higher energy and therefore more particle will have the required activation energy.

65.

Collision theory states that for a reaction to take place the the particles must collide with sufficient energy for the collision to result in a reaction. This amount of energy is called the...

a)

collision energy

b)

frequency energy

c)

activation energy

d)

success energy

66.

The reaction profile digram is shown for an exothermic reaction, which arrow represents the activation energy?

a)

A

b)

B

c)

C

67.

The reaction between an acid and calcium carbonate was carried out (reaction 1) it was repeated at a higher temperature. Which line (or lines) could represent the reaction?

a)

1

b)

2

c)

3

d)

4

68.

The reaction between an excess of acid and calcium carbonate was carried out (reaction 1) it was repeated but the concentration of the acid was reduced but still remained in excess. Which line (or lines) could represent the reaction?

a)

1

b)

2

c)

3

d)

4

69.

The reaction between an excess of acid and calcium carbonate was carried out (reaction 1) it was repeated but the mass of the calcium carbonate was halved. Which line (or lines) could represent the reaction?

a)

1

b)

2

c)

3

d)

4

70.

Reactions taking place at a higher temperature have a higher rate of reaction because...

a)

The particle move faster and so there are more frequent collisions.

b)

Higher temperatures break the particles down into smaller parts and so they have a greater surface area resulting in more frequent collisions.

c)

The particles have more energy and so more of the collisions exceed the activation energy and so there are more frequent successful collisions.

d)

Higher temperatures cause the water to evaporate and the solutions to become more concentrated, this means there will be more frequent collisions.

71.

Catalysts are...

a)

Substances that speed up the rate of a reaction

b)

Substances that are chemically unchanged at the en of a reaction

c)

Always solids

d)

Often (but not always) transition metal compounds.

72.

Catalysts work by...

a)

Providing an alternative route for a reaction with a lower activation energy. This results in less frequent successful collisions.

b)

Providing an alternative route for a reaction with a lower activation energy. This results in less frequent successful collisions.

c)

Providing an alternative route for a reaction with a higher activation energy. This results in more frequent successful collisions.

d)

Providing an alternative route for a reaction with a lower activation energy. This results in more frequent successful collisions.

73.

What does rate of reaction tell us?

a)

How fast products turn into reactants

b)

How fast reactants turn into products

c)

If a reaction happens or not

d)

What happens during a reaction

74.

What factors affect rate of reaction?

a)

Surface area

b)

Catalysts

c)

Temperature

d)

Concentration

e)

Time

75.

What is activation energy?

a)

Energy needed to make chemicals spontaneously split apart

b)

Energy to activate chemicals

c)

Largest amount of energy particles have

d)

Smallest amount of energy particles need before they react

76.

What is needed for particles to react?

a)

They must collide

b)

They must have enough energy

c)

They must be elements

d)

They must be compounds

77.

If we increase the temperature, what happens to the rate of reaction?

a)

Nothing

b)

Decreases

c)

Increases

78.

Particles that are at a higher temperature move (a)   then particles with a low temperature

79.

Why does increasing concentration increase rate of reaction?

a)

Less particles moving around so more collisions

b)

More particles moving around so more collisions

c)

More particles moving around so less collisions

d)

Less particles moving around so less collisions

80.

A higher surface area means....

a)

nothing

b)

higher rate of reaction

c)

lower rate of reaction

81.

Which has the biggest surface area?

a)

Small particles

b)

Large particles

c)

elements

d)

compounds

82.

What is the name of a special substance which can be added to a reaction to increase the rate of reaction?

(a)  

83.

What happens to a catalyst during a reaction

a)

It is used up and needs to be replaced every reaction

b)

It is used up

c)

It isnt used up but cant be used again

d)

It isn't used up and can be used again

84.

True or false: There is only one type of catalyst which can be used for every reaction

a)

True

b)

False

85.

How can we measure the rate of reaction?

a)

Time the bubbles

b)

Measure how quickly reactants are used up

c)

Measure rate at which products are made

d)

Just look and see what is happening

86.

Why is it important to control the rate of reaction in the body?

a)

Otherwise you will die

b)

So your cells can get exactly what they need

87.

A temperature increase causes the particles to ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

88.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

89.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
90.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

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