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S4 Chemistry_Review

Total questions: 123

Worksheet time: 2hrs 21mins

Name
Class
Date
1.

Which of the following is true about the formation of bonds between molecules?

a)

Energy is given off when bonds are formed between molecules.

b)

Energy is absorbed by the molecule when bonds are formed.

c)

Energy is neither given off nor absorbed when bonds are formed.

2.

Which of the following statement is true about the breaking of bonds between molecules?

a)

To break a bond between molecules, energy must be released by the molecule

b)

To break a bond between molecules, no energy is needed.

c)

To break a bond between molecules, energy must be absorbed by the molecule.

3.
Which letter corresponds to the energy of the products?
a)
A
b)
B
c)
C
d)
D
4.
If ∆H is negative, the reaction is?
a)
exothermic
b)
endothermic
5.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
6.

The energy level diagram for the reaction between magnesium and hydrochloric acid is shown.

a)

Energy is given out during the reaction

b)

The products are at a lower energy level than the reactants

c)

The reaction is endothermic.

7.

Which reaction is endothermic?

a)

acid neutralising alkali causing a temperature increase

b)

adding magnesium to hydrochloric acid

c)

calcium carbonate decomposing when heated combustion of fossil fuels

8.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
9.
Is photosynthesis an exothermic or endothermic reaction?
a)
Endothermic
b)
Exothermic
c)
Neither
10.

The initial temperature was measured to be 20oC and the final temperature was 10oC. The reaction was

a)

exothermic

b)

endothermic

11.

The initial temperature was measured to be 20oC and the final temperature was 45oC. The reaction was

a)

exothermic

b)

endothermic

12.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
13.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

14.

The graph above is from which type of reaction?

a)

Endothermic reaction

b)

Exothermic reaction

15.
Melting 
a)
exothermic
b)
endothermic
16.

When wood is burnt to keep us warm. This is an example of an ------------ reaction

a)

displacement

b)

exothermic

c)

endothermic

17.

An exothermic change is detected when the temperature ____

a)

stays the same

b)

increases

c)

decreases

18.

The energy taken into a reaction is higher than the energy given out, when the reaction is _____

a)

endothermic

b)

exothermic

19.

Choose the examples of exothermic reactions

a)

dehydration

b)

displacement

c)

nuclear reactions

d)

combustion

e)

photosynthesis

20.

Heat is taken in when ammonium nitrate dissolves in water. This is an example of?

a)

Thermal decomposition

b)

Endothermic change

c)

Exothermic change

d)

Electrolysis

21.

Which of the following energy changes corresponds to the activation energy required for the forward reaction to take place?

a)

A

b)

C

c)

B

d)

E

22.

Which of the following is true about the formation of bonds between molecules?

a)

Energy is given off when bonds are formed between molecules.

b)

Energy is absorbed by the molecule when bonds are formed.

c)

Energy is neither given off nor absorbed when bonds are formed.

23.

The energy level diagram for the reaction between magnesium and hydrochloric acid is shown.

a)

Energy is given out during the reaction

b)

The products are at a lower energy level than the reactants

c)

The reaction is endothermic.

24.

Which is an endothermic process?

a)

Burning hydrogen

b)

Distilling petroleum

c)

Reacting potassium with water

d)

Using petrol in a motor car engine

25.
What is the activation energy?
a)
The energy of the products
b)
The energy of the reactants
c)
The minimum energy needed by the reactants to form the products.
d)
The energy lost in the reaction
26.
If ∆H is negative, the reaction is?
a)
exothermic
b)
endothermic
27.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
28.

Exothermic reactions feel

a)

warm

b)

cold

29.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

30.

The average bond enthalpies for O-O and O=O are 146 and 496 kJ/mol respectively. What is the enthalpy change, in kJ, for the reaction below?

H-O-O-H(g) → H-O-H(g) + ½O=O(g)

a)

-102

b)

+102

c)

+350

d)

+394

31.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

32.

The following equation shows the formation of magnesium oxide from magnesium metal. Which statement is correct for this reaction?

2Mg(s) + O2(g) → 2MgO(s) ΔH = -1204 kJ

a)

1204 kJ of energy are released for every mole of magnesium reacted

b)

602 kJ of energy are absorbed for every mole of magnesium oxide formed

c)

602 kJ of energy are released for every mole of oxygen reacted

d)

1204 kJ of energy are released for every two moles of magnesium oxide formed

33.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

34.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

35.

How can we figure out if an overall reaction is endo- or exo-thermic? It is the difference between _______ and __________.

a)

hot and cold temperatures

b)

energy to break and energy to form bonds.

c)

time to form a bond versus time to break a bond

36.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

37.
Rate of chemical reaction means
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
38.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
39.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
40.
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 
41.
You make a space much smaller hoping to increase the reaction rates.
a)
temperature
b)
concentration
c)
catalyst
d)
pressure
42.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
43.
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
44.
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
45.
B represents
a)
energy absorbed
b)
energy released
c)
activation energy
46.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
47.
The picture shows a reversible chemical reaction taking place. How can equilibrium be reached?
a)
Stopper the flask.
b)
Add more reactants.
c)
Add more products.
d)
Cool the contents.
48.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
49.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
50.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
51.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
52.
A substance that increases speed of chemical reaction without being changed is called:
a)
Catalyst
b)
Acid
c)
Base
d)
pressure
53.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the reaction rate
54.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
55.
Identify where the reaction has finished
a)
A
b)
B
c)
C
d)
D
56.
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
57.
Identify the part of the graph with the fastest rate of reaction.
a)
A
b)
B
c)
C
d)
D
58.
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
59.
How does the energy in a reversible reaction in one way compare with the opposite direction?
a)
more energy going forward
b)
more energy going back
c)
the same
d)
no difference
60.
Which of these statements about rate of reaction graphs is NOT true?
a)
the steeper the slope, the faster the rate of reaction
b)
a flat slope means there is no reaction
c)
the shallower the slope, the faster the reaction
d)
as the reaction slows, the slope gets more shallow
61.

A ______ is a substance that speeds up the rate of a

chemical reaction without being used up in the reaction itself.

a)

Concentration

b)

Catalyst

c)

surface area

62.

When we investigate the rate of reaction we are looking at the...

a)

amount of product formed

b)

speed of reaction

c)

concentration of reacting particles

d)

combining reactants with products

63.
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 
64.

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

65.

Creating fossils is a very _____ chemical reaction

a)

Fast

b)

Slow

c)

It is not a chemical reaction

66.

Hydrogen gas burns in air to form water.

2H2 (g) + O2 (g) → 2H2O(I) ΔH= - 572 kJ

How much heat energy (in kJ) is given off if a rocket carrying 200.0 kg of hydrogen gas is burnt in excess oxygen?

a)

1.43 x 106

b)

1.43 x 107

c)

2.86 x 107

d)

4.92 x 107

67.

The gaseous oxides of nitrogen such as NO, N2O, NO2 and N2O4 have positive enthalpies of formation because

a)

oxygen has high electron affinity.

b)

the atomisation enthalpy of nitrogen is very high.

c)

the nitrogen atom has a high electronegativity.

d)

nitrogen has an extra stability due to its half-filled p orbitals.

68.

The standard enthalpy of combustion of 2-methylbut-1-ene, C5H10 is -3114 kJ mol-1. Which of the following compounds is expected to have the same enthalpy of combustion?

a)

Cyclopentane, C5H10

b)

Cyclopentene, C5H8

c)

Pent-2-ene, C5H10

d)

Methylcyclobutane, C5H10

69.

When an unknown mass of ethanol was burnt, the temperature of 1 dm3 water contained in a copper beaker increased by 7.2 °C. If the enthalpy of combustion

of ethanol is -1350 kJ mol-1, determine the mass of ethanol burnt. [Specific heat capacity of solution = 4.20 J g-1 °C-1; density of solution = 1.0 g cm-3; Mr of ethanol = 46]

a)

1.03 g

b)

1.55 g

c)

1.88 g

d)

2.25 g

70.

The following table shows the change in the enthalpy of combustion (kJ mol-1) of a hydrocarbons.

C2H6 = -1560 ; C4H10 = -2880 ; C7H16 = -4848

The complete combustion of 0.05 mol of a hydrocarbon W releases 176.5 kJ. What could be the molecular formula of W if W is also an alkane?

a)

C3H8

b)

C5H12

c)

C6H14

d)

C8H18

71.

In Thermite Reaction, a reactive metal such as aluminium is used to reduce iron(lll) oxide to iron. What is the enthalpy change when 2.0 moles iron(lll) oxide is reduced by 3.0 moles aluminium? [ΔHf (Al2O3) = -1676 kJ mol-1 ; ΔHf (Fe2O3) = -825 kJ mol-1]

a)

-855.0 kJ

b)

-1276.5 kJ

c)

-1702.2 kJ

d)

-3404.8 kJ

72.

The standard enthalpies of combustion of graphite and hydrogen are -394 kJ mol-1 and -286 kJ mol-1 respectively. If the standard enthalpy of formation of ethane is -20.0 kJ mol-1, what is the standard enthalpy of combustion of ethane in kJ mol-1?

a)

-1 220

b)

-1 305

c)

-1 537

d)

-1 626

73.

The standard heats of combustion per mole of butane, C4H10(g), hydrogen, H2(g), and 1,3-butadiene, C4H6(g) are -2878 kJ, -286 kJ and -2540 kJ respectively. What is the heat of hydrogenation of 1,3-butadiene?

C4H6(g) + 2H2(g) → C4H10(g)

a)

-234 kJ mol-1

b)

-325 kJ mol-1

c)

-370 kJ mol-1

d)

-408 kJ mol-1

74.

When heated strongly, potassium chlorate(V) decomposes to form potassium chloride and oxygen.

2KCIO3(s) →- 2KCI(s) + 3O2(g)

If the heat of formation of KCIO3 and KCI are -391.2 kJ mol-1 and -436.7 kJ mol-1 respectively, what is the enthalpy change when 20 g KCIO3 is heated?

[Relative atomic mass: O = 16; Cl = 35.5; K = 39]

a)

6.88 kJ

b)

7.42 kJ

c)

8.15 kJ

d)

8.80 kJ

75.

When 28.0 g of nitrogen reacts with oxygen to form nitric oxide, NO, and nitrogen dioxide, NO2, 103.0 kJ of heat was required. If no nitrogen remained, calculate the mass of nitric oxide, NO formed.

[ΔHf (NO) = 90.3 kJ mol-1, ΔHf (NO2) = 33.2 kJ mo-1]

a)

4.8 g

b)

9.6 g

c)

19.2 g

d)

24.3 g

76.

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

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

77.

Which of the following is true about the formation of bonds between molecules?

a)

Energy is given off when bonds are formed between molecules.

b)

Energy is absorbed by the molecule when bonds are formed.

c)

Energy is neither given off nor absorbed when bonds are formed.

78.

Which of the following statement is true about the breaking of bonds between molecules?

a)

To break a bond between molecules, energy must be released by the molecule

b)

To break a bond between molecules, no energy is needed.

c)

To break a bond between molecules, energy must be absorbed by the molecule.

79.
Which letter corresponds to the energy of the products?
a)
A
b)
B
c)
C
d)
D
80.
If ∆H is negative, the reaction is?
a)
exothermic
b)
endothermic
81.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
82.

The energy level diagram for the reaction between magnesium and hydrochloric acid is shown.

a)

Energy is given out during the reaction

b)

The products are less stable than the reactants

c)

The reaction is endothermic.

83.

Which reaction is endothermic?

a)

acid neutralising alkali causing a temperature increase

b)

adding magnesium to hydrochloric acid

c)

calcium carbonate decomposing when heated combustion of fossil fuels

84.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
85.
Is photosynthesis an exothermic or endothermic reaction?
a)
Endothermic
b)
Exothermic
c)
Neither
86.

The initial temperature was measured to be 20oC and the final temperature was 10oC. The reaction was

a)

exothermic

b)

endothermic

87.

The initial temperature was measured to be 20oC and the final temperature was 45oC. The reaction was

a)

exothermic

b)

endothermic

88.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
89.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

90.

The graph above is from which type of reaction?

a)

Endothermic reaction

b)

Exothermic reaction

91.
Melting 
a)
exothermic
b)
endothermic
92.

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

93.

What is the instantaneous rate of reaction

a)

Is the reaction time instantly

b)

Is the rate of reaction at any one particular time during the reaction

c)

Is the rate of reaction at multiple times during the reaction

d)

Is the rate of reaction initially during the reaction

94.

2 factors affecting the rate of a reaction are

a)

Particle size

b)

Time

c)

Temperature

d)

Solubility

95.

the nature of reactants affects the rate of reaction. Which has a faster reaction rate

a)

Covalent bonds

b)

Ionic bonds

96.

Why do covalent bonds have a slower reaction rate?

a)

Double bonds need to be broken first

b)

Electron transfer must occur

c)

Single bonds need to be made first

d)

They aren't slower than ionic

97.

Particle size affects rate of reaction how

a)

Large the particle size, the quicker the reaction due to a large surface area

b)

Dust particles have a very slow reaction

c)

Smaller the particle size, the quicker the reaction due to a large surface area

d)

Cutting potatoes up into smaller pieces doesn't help it cook faster

98.

For a dust explosion to occur, which of the following must be present?

a)

Oxygen

b)

Methane

c)

Enclosed space

d)

Open space

99.

This image indicates what about concentration?

a)

Decreasing concentration, decreases the rate of a reaction

b)

Having equal amounts of both increases rate of reaction

c)

Increasing concentration, increases the rate of a reaction

d)

Increasing concentration, decreases the rate of a reaction

100.

This image tells you what about higher temperature in terms of rate of reaction

a)

Increase temperature, increase collisions as the particles have less energy and so collide more

b)

Increase temperature, decrease collisions

c)

Increase temperature, increase collisions as the particles have more energy and so collide more

d)

Decrease temperature which increases collisions so the rate of reaction increases

101.

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

102.

Which of these are enzymes

a)

Catalase

b)

Brollase

c)

Protease

d)

Treease

103.

The reaction of hydrogen peroxide and manganese dioxide is an example of

a)

Homogeneous catalysis

b)

Heterogeneous catalysis

c)

Biological catalysis

d)

Catalyst poision

104.

The surface adsorption theory involves

a)

Hydrogen and oxygen

b)

Oxygen and carbon dioxide

c)

Lead

d)

Platinum

105.

It converts pollutants from the exhaust gases into less harmful substances

a)

Car engine

b)

Car exhaust

c)

Catalytic converter

d)

Catalytic poison

106.

Catalytic converter is an example of a

a)

Catalyst poison

b)

Heterogeneous catalysis

c)

Homogeneous catalysis

d)

Biological catalyst

107.

Lead compounds are an example of

a)

Catalyst

b)

Catalyst poison

c)

Catalytic converter blocker

d)

Heterogeneous cataylst

108.

Reactants have more energy than products in which type of reaction

a)

Endothermic

b)

Exothermic

109.

When we investigate the rate of reaction we are looking at the...

a)

amount of product formed

b)

speed of reaction

c)

concentration of reacting particles

d)

combining reactants with products

110.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
111.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
112.
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 
113.
You add more bodies into a "mosh pit" to hope for more collisions.  You have increased-
a)
temperature
b)
concentration
c)
pressure
d)
catalyst
114.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
115.
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
116.
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
117.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
118.

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

119.

Creating fossils is a very _____ chemical reaction

a)

Fast

b)

Slow

c)

It is not a chemical reaction

120.

What does the M after a concentration value stand for?

a)

meters

b)

music

c)

Molarity

d)

moles

121.

Which is the highest concentration?

a)

10m

b)

2M

c)

25 mmol

d)

0.5M

122.

The major theory of reaction rate is called

a)

Collision theory

b)

Crash theory

c)

Newton's laws

d)

Thermodynamics

123.

When surface area is decreased the rate of reaction...

a)

Decreases, because there are LESS possible sites for correct collisions

b)

Increases, because there are LESS possible sites for correct collisions

c)

Decreases, because there are MORE possible sites for correct collisions

d)

Increases, because there are MORE possible sites for correct collisions

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