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Assessment| Chemistry Revision

Total questions: 100

Worksheet time: 1hrs 15mins

Name
Class
Date
1.

Which statement explains why ammonia gas, NH3, diffuses at a faster rate than

hydrogen chloride gas, HCl ?

a)

Ammonia expands to occupy all of the space available.

b)

Ammonia has a smaller relative molecular mass than hydrogen chloride.

c)

Ammonia is an alkali and hydrogen chloride is an acid.

d)

Ammonia molecules diffuse in all directions at the same time.

2.

2.00 g of powdered calcium carbonate is added to 50.0 cm3 of hydrochloric acid.

Which apparatus is used to measure the calcium carbonate and the hydrochloric acid?

a)

calcium carbonate- balance; hydrochloric acid-burette

b)

calcium carbonate-balance; hydrochloric acid-thermometer

c)

calcium carbonate-pipette; hydrochloric acid-burette

d)

calcium carbonate-pipette; hydrochloric acid-thermometer

3.

The measurements from a chromatography experiment using substance F are shown. The diagram is not drawn to scale.

What is the Rf value of F?

a)

0.55

b)

0.61

c)

0.90

d)

1.64

4.

Which statement describes the structure of an ionic compound?

a)

It is a giant lattice of oppositely charged ions.

b)

It is a giant lattice of positive ions in a ‘sea’ of electrons.

c)

It is a giant molecule of oppositely charged ions.

d)

It is a simple molecule of oppositely charged ions.

5.

Propane burns in oxygen.

C3H8 + xO2 → 3CO2 + yH2O

Which values of x and y balance the equation?

a)

x:5, y:4

b)

x:7, y:4

c)

x:10, y:8

d)

x:13, y:8

6.

Magnesium reacts with sulfuric acid.

What are the formulae of the products formed in this reaction?

a)

MgSO4 and H2

b)

MgSO4 and H2O

c)

Mg(SO4)2 and H2

d)

Mg(SO4)2 and H2O

7.

Which statement explains why graphite is used as a lubricant?

a)

All bonds between the atoms are weak.

b)

It conducts electricity.

c)

It has a low melting point.

d)

Layers in the structure can slide over each other.

8.

Ethanol is used as a fuel.

ethanol + oxygen --> carbon dioxide + water


Which statements are correct?

1 The reaction is endothermic.

2 The products have more energy than the reactants.

3 The oxygen for this reaction comes from the air.

4 The temperature of the reaction mixture rises during this reaction.

a)

1 and 2

b)

1 and 3

c)

2 and 4

d)

3 and 4

9.

Which metal has variable oxidation states?

a)

aluminium

b)

calcium

c)

copper

d)

sodium

10.

What is the catalyst in the Haber process?

a)

Fe

b)

Ni

c)

Pt

d)

V2O5

11.

Which calcium compound does not neutralise an acid soil?

a)

calcium oxide

b)

calcium sulfate

c)

calcium hydroxide

d)

calcium carbonate

12.

Which type of linkage joins the amino acids in a protein?

a)
b)
c)
d)
13.

In which molecule are all the outer shell electrons from each atom used to form covalent bonds?

a)

CH4

b)

Cl2

c)

H2O

d)

NH3

14.

The diagram shows a section of an overhead power cable.

Which statement explains why a particular substance is used?

a)

Aluminium has a low density and is a good conductor of electricity.

b)

Ceramic is a good conductor of electricity.

c)

Steel can rust in damp air.

d)

Steel is more dense than aluminium.

15.

Which row describes an endothermic reaction?

a)
b)
c)
d)
16.

Some metal nitrates and carbonates decompose when heated strongly.

Metal Q has a nitrate that decomposes to give a salt and a colourless gas only.

The carbonate of metal Q does not decompose when heated with a Bunsen burner.

What is metal Q?

a)

calcium

b)

copper

c)

sodium

d)

zinc

17.

Aluminium is extracted from its ore by electrolysis.

Which equation represents the reaction that occurs at the anode during the electrolysis?

a)

Al3+ + 3e– ----> Al

b)

Al3+ ---> Al + 3e–

c)

2O2– ---> O2 + 4e–

d)

2O2– + 2e– ---> O2

18.

a)

A

b)

B

c)

C

d)

D

19.

a)

A

b)

B

c)

C

d)

D

20.

a)

A

b)

B

c)

C

d)

D

21.

a)

A

b)

B

c)

C

d)

D

22.

a)

A

b)

B

c)

C

d)

D

23.

a)

A

b)

B

c)

C

d)

D

24.

a)

A

b)

B

c)

C

d)

D

25.

a)

A

b)

B

c)

C

d)

D

26.

a)

A

b)

B

c)

C

d)

D

27.

a)

A

b)

B

c)

C

d)

D

28.

a)

A

b)

B

c)

C

d)

D

29.

a)

A

b)

B

c)

C

d)

D

30.

a)

A

b)

B

c)

C

d)

D

31.

a)

A

b)

B

c)

C

d)

D

32.

a)

A

b)

B

c)

C

d)

D

33.

a)

A

b)

B

c)

C

d)

D

34.

a)

A

b)

B

c)

C

d)

D

35.

a)

A

b)

B

c)

C

d)

D

36.

a)

A

b)

B

c)

C

d)

D

37.

a)

A

b)

B

c)

C

d)

D

38.

a)

A

b)

B

c)

C

d)

D

39.

a)

A

b)

B

c)

C

d)

D

40.

a)

A

b)

B

c)

C

d)

D

41.

a)

A

b)

B

c)

C

d)

D

42.

a)

A

b)

B

c)

C

d)

D

43.

a)

A

b)

B

c)

C

d)

D

44.

a)

A

b)

B

c)

C

d)

D

45.

a)

A

b)

B

c)

C

d)

D

46.

a)

A

b)

B

c)

C

d)

D

47.

a)

A

b)

B

c)

C

d)

D

48.

a)

A

b)

B

c)

C

d)

D

49.

a)

A

b)

B

c)

C

d)

D

50.

a)

A

b)

B

c)

C

d)

D

51.

a)

A

b)

B

c)

C

d)

D

52.

a)

A

b)

B

c)

C

d)

D

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 rate.
54.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
55.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
56.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
57.

Smaller clumps allow for a _________ surface area to be exposed for the reaction.

a)
larger
b)
smaller
58.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
59.
Which of these will NOT speed up the rate of reaction between a strip of magnesium and hydrochloric acid?
a)
tightly coil up the strip of magnesium
b)
cut up the strip of magnesium
c)
increase the concentration of the hydrocholoric acid
d)
increase the temperature of the hydrocholoric acid
60.
Products will form faster if____________
a)

the surface area of the reactants are smaller.

b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
61.

Na2S + 2 HCl → 2NaCl + H2S

What would happen if we increased the volume of the container where the reaction occurred?

a)

More NaCl would be produced

b)

Less H2S would would be produced

c)

More reactions would occur

d)

More HCl would be needed

62.

(NH4)2SO4 + Ba(NO3)2 → 2NH4NO3 + BaSO4

What would happen if we increased the concentration of (NH4)2SO4?

a)

More product would be produced

b)

Less (NH4)2SO4 would participate in the reactions

c)

There would be less collisions between

(NH4)2SO4 and Ba(NO3)2

d)

There would be more Ba(NO3)2 particles to react

63.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
64.

Which of the following would increase the number of collisions that occur? Choose all that appy.

a)

Increase Surface Area

b)

Decrease Concentration

c)

Increase Temperature

d)

Increase Volume

65.

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

66.

AgNO3 + NaCl → AgCl + NaNO3

What would you expect to happen if we decrease the temperature of this reaction container?

a)

The energy of the reactants would decrease.

b)

The would be more product produced.

c)

The number of particles of

AgNO3 and NaCl would decrease.

d)

The number of collisions in the reactants would increase.

67.

More collisions (in the correct orientation) results in... (choose all that apply)

a)

a slower reaction rate

b)

an increased reaction rate

c)

more product being produced

d)

less volume of the reaction container

68.

Which of the following is true?

a)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of greater surface area.

b)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of lesser surface area.

c)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of greater surface area.

d)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of lesser surface area.

69.

In which container would you expect a higher reaction rate, and why? (Note: The number of particles is the same in both containers.)

a)

The left would have a higher reaction rate because it has a greater volume and more collisions will happen.

b)

The right would have a higher reaction rate because it has a greater volume and more collisions will happen.

c)

The left would have a higher reaction rate because it has a lesser volume and more collisions will happen.

d)

The right would have a higher reaction rate because it has a lesser volume and more collisions wil happen.

70.

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

71.

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

72.

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

73.

For the reaction 2H2(g) + O2(g) → 2H2O(g) the bond enthalpies (in kJ/mol) are

H-H = x, O=O = y, O-H = z

Which calculation will give the value, in kJ/mol, of ΔH for the reaction?

a)

2x + y - 2z

b)

4z - 2x - y

c)

2x + y - 4z

d)

2z - 2x - y

74.
Which statement is true regarding endothermic reactions?
a)
a) Temperature change is positive and enthalpy change is positive
b)
b) Temperature change is positive and enthalpy change is negative
c)
c) Temperature change is negative and enthalpy change is positive
d)
d) Temperature change is negative and enthalpy change is negative
75.
Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....
a)
+ 160 kJ
b)
-63 kJ
c)
- 160 kJ
d)
-217 kJ
76.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

77.

What kind of energy change happens in the photosynthesis reaction in plant leaves?

a)

Endo

b)

Exo

c)

No change

78.

Burning leaves and burning a fuel provide a(n) _______ change.

a)

endothermic

b)

exothermic

c)

physical

79.

When new chemical bonds form, energy ____________.

a)

is taken into the system.

b)

is released from the system.

c)

stays the same in the system.

80.

In a reaction old bonds _______ and new bonds _______.

a)

form , break

b)

break, form

c)

stay, added

81.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) → PCl5 (s) + energy

a)

endothermic

b)

exothermic

82.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy → 2KNO2 (s) + O2 (g)

a)

endothermic

b)

exothermic

83.

Is this reaction endo- or exo-thermic?

NH4NO2 + energy → N2 (g) + 2H2O (g)

a)

endothermic

b)

exothermic

84.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
85.
What element is being Reduced?
a)
N
b)
H
c)
O
d)
S
86.
What are the coefficients when the equation is balanced?
a)
2 + 3 --> 2 + 3 + 4
b)
1 + 3 --> 1 + 3 + 2
c)
2 + 4 --> 2 + 3 + 2
d)
1 + 1 --> 1 + 1 + 1
87.
What element is being Oxidized?
a)
I
b)
H
c)
S
d)
O
88.
What are the coefficients when the equation is balanced?
a)
1 + 1 + 1 --> 2 + 1 + 3
b)
2 + 2 + 2 --> 4 + 2 + 3
c)
1 + 2 + 1 --> 2 + 2 + 3
d)
1 + 1 + 1 --> 1 + 1 + 1
89.
What element is being reduced?
a)
I
b)
H
H
c)
S
S
d)
O
O
90.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
91.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
92.
What is oxidation number of H in CaH2?
a)
+1
b)
-1
c)
0
d)
+2
93.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
94.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
95.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
96.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
97.

In the reaction 2Ca(s) + O2(g) → 2CaO(s), calcium is

a)

Reduced

b)

Synthesized

c)

Oxidized

d)

None of the above

98.

In the reaction Zn + H2O → ZnO2 + H2  which element, if any, is oxidized? 

a)

Zinc

b)

Hydrogen

c)

Oxygen

d)

None

99.

What substance is oxidized in the following reaction?

4Fe + 3O2 → 2Fe2O3

a)

Iron

b)

Fluorine

c)

Oxygen

d)

Iron oxide

100.
Oxygen always has an oxidation number of...
a)
-1
b)
1
c)
2
d)
-2

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