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Kinetics Unit Practice

Total questions: 69

Worksheet time: 1hrs 9mins

Name
Class
Date
1.

The rate of a chemical reaction normally

a)

increases as temperature decreases.

b)

decreases when a catalyst is added.

c)

increases as reactant concentration increases.

d)

decreases as reactant concentration increases.

2.

Crushing a solid into a powder will increase reaction rate because:

a)

the particles will collide with more energy

b)

the orientation of colliding particles will be improved

c)

the activation energy barrier will be lowered

d)

the powdered form has more surface area

3.

A lump of ignited charcoal which is glowing in air burns more vigorously when lowered into a bottle of pure oxygen. This is due to an increase in

a)

surface area

b)

temperature

c)

concentration

d)

volume

4.

What happens to a catalyst in a reaction?

a)

It remains unchanged.

b)

It is incorporated into the reactants.

c)

It is incorporated into the products.

d)

It evaporates.

5.

Which out of the following is NOT a factor that affects the rate of a reaction between a solid and liquid reactant?

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

6.

How does a catalyst work in speeding up a reaction?

a)

by lowering the activation energy (minimum energy needed for the reaction to take place)

b)

by giving the reactants more energy

c)

by increasing the number of reactant particles

d)

by increasing the temperature

7.

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

8.
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.
9.

Which of the following increases the reaction rate?

a)

less surface area

b)

lower temperature

c)

more particle size

d)

increased concentration

10.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
11.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
12.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
13.
A measure of the average kinetic energy of a substance.
a)
heat
b)
temperature
c)
enthalpy
d)
entropy
14.

The potential energy diagram of a reaction is shown. Which represents the enthalpy change for the reaction?

a)

1

b)

2

c)

3

d)

4

15.

In an exothermic process the surroundings looses heat. 

a)
True
b)
False
16.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
17.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
18.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
19.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

20.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

21.
Endothermic reactions feel
a)
warm
b)
cold
22.

What kind of energy is stored in the bonding of atoms?

a)

Potential

b)

Kinetic

c)

None of the above

d)

All of the above

23.

The ____________ states that atoms, ions, or molecules must collide in order to react.

a)

transition state

b)

activation energy

c)

rate law

d)

collision theory

24.

Increasing the ____ causes the particles (atoms

or molecules) of the reactants to move more quickly so that

they collide with each other more frequently and with more

energy.

a)

Catalyst

b)

Surface Area

c)

Temperature

d)

Concentration

25.

________ is the measure of how much area of an

object is exposed.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentration

26.

Grains of sugar have a greater _______ than a solid cube of

sugar of the same mass, and therefore will dissolve quicker in water.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentratrion

27.

The energy needed for substance to initiate reaction is called...

a)

Initiation energy

b)

Propagation energy

c)

Activation energy

d)

Enthalpy

28.

From options below, which one is an exothermic reaction?

a)

Photosynthesis

b)

Melting ice cube

c)

Sublimation

d)

Magnesium Combusting

29.

When the value of ΔH is negative, which one(s) from below is/are true?

a)

The reaction is fast

b)

The reaction releases energy

c)

It is a combustion reaction

d)

The energy of product is lower than reactant

30.

When KNO3 salt is dissolved in water, the water becomes colder. By that information, we know that the solvation of KNO3 is...

a)

Endothermic reaction

b)

Endothermic process

c)

Exothermic reaction

d)

Exothermic process

31.
If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there will be no effect on the
a)
rate of the forward reaction
b)
activation energy of the reaction
c)
heat of reaction
32.
Two reactant particles collide with proper orientation.The collision will be effective if the particles have
a)
high activation energy
b)
high ionization energy
c)
sufficient kinetic energy
d)
sufficient potential energy
33.
When one mole of a certain compound is formed from its elements under standard conditions, it absorbs 85 kiloJoules of heat. A correct conclusion from this statement is that the reaction has a
a)

ΔH is –85 kJ/mole

b)

ΔH is +85 kJ/mole

c)

 ΔS is –85 kJ/mole

d)

 ΔS is +85 kJ/mole

34.
Which interval represents the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
E
35.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
36.

Given the reaction: C6H12O6(s) + 6O2(g) --> 6H2O(l) + 6CO2(g) + energy

What is the ΔH and ΔS?

a)

ΔH is + & ΔS is +

b)

ΔH is + & ΔS is -

c)

ΔH is - & ΔS is +

d)

ΔH is - & ΔS is -

37.

In Table i the reaction of hydrogen and oxygen to form water is best described as

a)
exothermic, because energy is released
b)
endothermic, because energy is released
c)
exothermic, because energy is absorbed
d)
endothermic, because energy is absorbed
38.

Which numbered intervals on the diagram would change when a catalyst is added?

a)
B & C
b)

A & E 

c)

A & D

d)

E & D 

39.

Which term refers to the difference between the potential energy of the products and the potential energy of the reactants for any chemical change?

a)
heat of deposition
b)
heat of fusion
c)
heat of reaction
d)
heat of vaporization
40.
Which picture shows how a catalyst would change the rate? 
a)
Option 3
b)
Option 2
c)
Option 1
41.

What is the symbol for entropy?

a)

H

b)

G

c)

S

d)

E

42.

Which represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

43.

Which represents a -ΔS?

a)

ice melting

b)

salt dissolving

c)

water boiling

d)

none of these

e)

wood burning

44.

Which of the following scenarios describes a process with a negative entropy change?

a)

Building a skyscraper

b)

A clean room becomes cluttered

c)

An igloo melting

d)

salt dissolving in water

45.

Which of these have a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

N2(g) and 3H2(g) → 2NH3(g)

c)

C6H6(l) → 6C(s)+ H2(g)

46.

The entropy can be thought of as

a)

the amount of disorder and spread

b)

the amount of order and organization

c)

the amount of heat energy

47.

Which combination of ΔH and ΔS always has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

48.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

49.

Ammonium nitrate dissolves in water. The solution becomes colder as it dissolves. It is a spontaneous endothermic process in the chemistry room because there is

a)

a decrease in enthalpy and the temperature of the room is high enough

b)

an increase in entropy and the temperature of the room is high enough

c)

an increase in enthalpy and of the room the temperature is cold enough

d)

a decrease in entropy and the temperature of the room is cold enough

50.

What is a spontaneous process ?

a)

slow process

b)

fast process

c)

process that needs an external intervention to occur

d)

process that does not need external intervention to occur / keep happening

51.
Spontaneity is determined by....
a)
enthalpy only
b)
entropy only
c)
enthalpy, entropy, and temperature
52.
Spontaneous reactions may be extremely slow.
a)
True
b)
False
53.
Reactions tend to be spontaneous if they are exothermic.
a)
True
b)
False
54.
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
55.
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
56.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
57.

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

58.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

59.

Predict the signs of ΔH , ΔS and spontaneity of the melting of iron:

Fe(s) + energy --> Fe(l)

a)

Δ H = - , Δ S = + and spontaneous at all temperature

b)

Δ H = + , Δ S = + and spontaneous at high temperature

c)

Δ H = + , Δ S = + and never spontaneous

d)

Δ H = - , Δ S = - and spontaneous at all temperature

60.

Which factor can only affect the rate of reaction when gases are one of the reactants?

a)

Concentration of reactants

b)

Pressure

c)

Temperature

d)

Size of reactants

61.

A catalyst only changes...

a)

the speed of the reaction

b)

the ΔH of the reaction

c)

the amount of product produced when the reaction is finished

d)

The ΔS of the reaction

62.

If ΔH is negative, heat would be shown on the _____ side of the thermochemical equation.

a)
Reactant
b)
Product
63.

In an exothermic process the system looses heat. 

a)
True
b)
False
64.

In an endothermic reaction the surroundings are losing energy.

a)
True
b)
False
65.

ΔH value in an exothermic reaction is a positive number.

a)
True
b)
False
66.

Which interval represents the PE of the Products?

a)
A
b)
B
c)
D
d)
E
67.

Which represents a +ΔS?

a)

water freezing

b)

water condensing

c)

photosynthesis

d)

none of these

e)

wood burning

68.

According to table i, which two of the following will feel colder when dissolving into room temperature water?

a)

NaOH(s)

b)

NH4Cl(s)

c)

LiBr(s)

d)

KNO3(s)

69.

According to table i, which two of the following will feel hotter when dissolving into room temperature water?

a)

NaOH(s)

b)

NaCl(s)

c)

LiBr(s)

d)

KNO3(s)

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