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rates of reaction

Total questions: 50

Worksheet time: 2hrs 40mins

Name
Class
Date
1.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

2.

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

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

3.

Which of the following increase the reaction rate?

a)

less surface area

b)

lower temperature

c)

increased concentration

4.

What is the rate of reaction?

a)

How fast a reaction is

b)

How big a reaction is

c)

How loud a reaction is

5.

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

sugar.

a)

Surface Area

b)

Catalyst

c)

Temperature

6.
Why does breaking up a solid reactant increase the rate of reaction?
a)
it creates more solid
b)
it creates more energy
c)
it increases the surface area
d)
it increases the concentration
7.

The word for a substance that you react at the start of a chemical reaction...

a)

Reaction

b)

Reactant

c)

Product

d)

The result

8.

The word for a substance created in a chemical reaction...

a)

Reaction

b)

Reactant

c)

Product

d)

Mass

9.

Objects hitting each other

a)

Collision

b)

Catalyst

c)

Explosion

d)

Reaction

10.

The speed at which a chemical reaction occurs

a)

Fast

b)

Slow

c)

Rate

d)

Ratio

11.

The amount of something; how many particles in a volume of a mixture

a)

Rate

b)

Collision

c)

Catalyst

d)

Concentration

12.

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

13.

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

14.

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

15.

Increasing the temperature gives particles more __________.

a)

Time

b)

Energy

c)

Space

d)

Frequency

16.

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

a)

Time

b)

Reactions

c)

Collisions

d)

Reactants

17.

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

a)
b)
c)
d)
18.
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
19.
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
20.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
21.
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
22.
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
23.
Identify the part of the graph with the fastest rate of reaction.
a)
A
b)
B
c)
C
d)
D
24.

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

25.
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
26.
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
27.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

28.
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.
29.
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
30.
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
31.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
32.

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

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

33.

What is the rate of a reaction?

a)

How fast something happens

b)

How slow something happens

c)

When two chemicals mix together and make something new

d)

change in concentration per unit time of any one reactant or product

34.

2 factors affecting the rate of a reaction are

a)

Particle size

b)

Time

c)

Temperature

d)

Solubility

35.

What is a catalyst according to chemistry

a)

A substance that speeds up the rate of a reaction without being used up in the reaction

b)

A substance that slows down the rate of a reaction without being used up in the reaction

c)

A substance that alters the rate of a reaction without being used up in the reaction

d)

A substance that slows down the rate of a reaction and is used up in the reaction

36.

Increasing the temperature gives particles more __________.

a)

time

b)

energy

c)

space

d)

frequency

37.

You make a space much smaller by increasing the ________________ hoping to increase the reaction rates.

a)

temperature

b)

concentration

c)

catalyst

d)

pressure

38.

which curve applies for the same gas at a lower temperature?

a)
b)
c)
d)
39.

Which solid-line curve most accurately represents the distribution of molecular energies in a gas at 500K if the dotted-line represents the corresponding distribution for the same gas at 300K ?

a)
b)
c)
d)
40.

Which pair of statements is correct when a catalyst is used

a)

Ea1, catalysed reaction and fewer effective collisions

Ea2, uncatalysed reaction and more effective collisions

b)

Ea1, uncatalysed reaction and fewer effective collisions

Ea2, catalysed reaction and more effective collisions

c)

Ea1, catalysed reaction and more effective collisions

Ea2, uncatalysed reaction and fewer effective collisions

d)

Ea1, uncatalysed reaction and more effective collisions

Ea2, catalysed reaction and fewer effective collisions

41.

Which of the following is FALSE for Maxwell Boltzmann distribution curve?

a)

Area under curve represent number of particles

b)

Increase in temperature will shift the curve to right

c)

High temp, fraction of molecules with energy > Ea increases

d)

At higher temp, area under curve is greater than at low temp

42.

Which of the curves indicates the fastest reaction?

a)

A

b)

B

c)

C

43.

Which of the curves indicates the slowest reaction?

a)

A

b)

B

c)

C

44.

A liquid X reacts with a solid Y to form a gas. Which two diagrams show suitable methods for investigating the rate (speed) of the reaction.

a)

1 and 3

b)

1 and 4

c)

2 and 3

d)

2 and 4

45.

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

46.

Powdered marble reacts with hydrochloric acid using the apparatus shown. The gas syringe fills in 36 seconds. The experiment is repeated using marble chips in place of powdered marble. How long does it take to fill the gas syringe in this experiment.

a)

9 seconds

b)

18 seconds

c)

36 seconds

d)

72 seconds

47.

Which of the following changes decreases the rate of the reaction between magnesium and dilute hydrochloric acid?

a)

1, 2 and 3

b)

1 and 2 only

c)

1 and 3 only

d)

2 and 3 only

48.

A student investigates the rate of reaction between marble chips and hydrochloric acid. The mass of the reaction flask is measured. The graph shows the results of two experiments, P and Q.

Which change explains the difference between P and Q?

a)

A catalyst is added in P.

b)

A higher temperature is used in P.

c)

Bigger marble chips are used in Q.

d)

Hydrochloric acid is more concentrated in Q.

49.

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

a)

A

b)

B

c)

C

d)

D

50.

Which of these represent the activation enthalpy of a reaction?

a)

A

b)

B

c)

C

d)

D

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