Grade 10 – CHM 51
Topic 5 – Practice Questions – AK
 Subtopic 5.1 – Describing Chemical Reactions

2. The reactants in the reaction above are
____________.
Use the following information to answer
questions 1 – 4.
The diagram below represents the reaction
between grey iron metal, Fe, and
hydrochloric acid solution, HCl, where
hydrogen gas and yellow iron (II) chloride
solution, FeCl2, are produced.
√
A.
hydrogen and hydrochloric acid
B.
iron (II) chloride and hydrogen
C.
iron and hydrochloric acid
D.
iron and hydrogen
3. The products in the reaction above are ______.
√
√
I only
B.
II only
C.
I and II only
D.
I, II and III
hydrogen and hydrochloric acid
B.
iron (II) chloride and hydrogen
C.
iron and hydrochloric acid
D.
iron and hydrogen
4. What is the word equation for the above
chemical reaction?
1. What is/are the sign(s) that a chemical
reaction has taken place in the above
experiment?
I.
Release of gas
II.
Change of color
III.
Release of heat
A.
A.
√
A.
Hydrogen reacts with hydrochloric
acid to form iron (II) chloride
solution and iron
B.
Iron reacts with hydrochloric acid to
form iron (II) chloride and hydrogen
C.
Iron (II) chloride reacts with
hydrogen to form iron and
hydrochloric acid
D.
Iron and hydrogen gas combine to
form iron chloride and hydrochloric
acid
______________________________________________________
Topic 5 – Practice Questions
1
Grade 10 – CHM 51
5. The ____________ in a chemical equation
represent the relative amounts of reactants
and products.
√
A.
subscripts
B.
coefficients
C.
superscripts
D.
Both A and C
8. What does the symbol (s) in a chemical
equation indicate?
√
A.
Gas
B.
Solid
C.
Liquid
D.
Dissolve in water
9. What does the symbol (l) in a chemical
equation indicate?
6. What evidence of a chemical reaction is
represented in the figure below?
√
A.
Gas
B.
Solid
C.
Liquid
D.
Dissolve in water
10. What does the symbol (g) in a chemical
equation indicate?
√
A.
Change in color
B.
Formation of a gas
C.
A solid changed to liquid
D.
A solid dissolved in water
√
√
I only
B.
II only
C.
III only
D.
I and II only
Topic 5 – Practice Questions
Gas
B.
Solid
C.
Liquid
D.
Dissolve in water
11. What does the symbol (aq) in a chemical
equation indicate?
7. Which quantitative information is/are
revealed by a chemical equation?
I.
Number of molecules of each
compound
II.
Number of atoms of each element
III.
The state of each reactant
A.
A.
√
2
A.
Gas
B.
Solid
C.
Liquid
D.
Dissolve in water
Grade 10 – CHM 51
12. In a chemical equation, the state symbol
(aq) stands for ________.
√
A.
dissolved in acid
B.
dissolved in water
C.
reversible reaction
D.
gas being produced
16. In the reaction below the reactant(s) is/are
__________.
Magnesium + Sulfuric acid ⟶
Magnesium Sulfate + Hydrogen
√
13. Which of the symbols in a chemical
equation does not match its description?
A.
(l)
Liquid state
B.
(s)
Solid state
C.
(g)
Gas state
(aq)
Substance dissolved in oil
√ D.
A.

B.
△
C.
+
D.
Both A and B
√
√
I only
B.
II only
C.
I and II only
D.
I, II and III
Topic 5 – Practice Questions
B.
magnesium and sulfuric acid
C.
magnesium sulfate and hydrogen
D.
magnesium and magnesium
sulfate
A.
solids
B.
catalyst
C.
reactants
D.
products
18. It is important to balance a chemical
equation in order to _________.
I.
satisfy the law of conservation of
mass
II.
conserve the mass on both sides of
the chemical equation
III.
conserve the number of atoms on
both sides of the chemical equation
15. Which of the following is/are type of
product(s) produced by reactions that
occur in aqueous solutions?
I.
Solid
II.
Water
III.
Gas
A.
magnesium only
17. In a chemical equation, the ________________
are found on the right side of the equation.
14. Which of the following symbols is used to
separate reactants from products and
specify direction?
√
A.
√
3
A.
I only
B.
II only
C.
I and II only
D.
I, II and III
Grade 10 – CHM 51
19. Chemical equations must be balanced
because in a chemical reaction the _____.
√
A.
mass is conserved
B.
volume is conserved
C.
D.
22. Which of the following sets of coefficients
correctly balance the chemical equation
below?
___Zn(s) +__CuCl2 (𝑎𝑞) →__ZnCl2 (𝑎𝑞) +__Cu(s)
state of reactants is
conserved
√
atoms are destroyed and
recreated
A.
balanced
balanced
energy
C.
reversible
mass
D.
reversible
energy
√
A.
CaO(𝑠) +CO2 (𝑔) → CaCO3 (𝑠)
B.
CO2 (𝑔) + CaCO3 (𝑠) → CaO(𝑠)
C.
CaCO3 (𝑠) → CaO(𝑠) +CO2 (𝑔)
D.
2 : 1 : 2 : 1
C.
1 : 1 : 1 : 1
D.
2 : 1 : 1 : 1
A.
2
B.
3
C.
4
D.
6
24. Which of the following is true about a
skeleton equation?
I.
It shows the states of matter of each
formula
II.
It uses words to indicate reactants and
products
III.
It uses formulas to identify the reactants
and the products.
21. Solid calcium oxide reacts with carbon
dioxide gas to form solid calcium carbonate.
The chemical equation for the reaction
occurring is __________.
√
B.
CH4 (g) +____O2 (g) ⟶ ___ CO2 (g) +___ H2O (g)
mass
B.
1 : 2 : 1 : 1
23. For the following reaction to be balanced,
the coefficient of oxygen needs to be _______.
20. All chemical equations must be __________ to
satisfy the Law of conservation of
____________.
√
A.
√
A.
I only
B.
II only
C.
I and III only
D.
I, II and III
CO2 (𝑔) → CaO(𝑠) + CaCO3 (𝑠)
Topic 5 – Practice Questions
4
Grade 10 – CHM 51
25. Which of the following is a correct
balanced chemical equation?
I.
II.
III.
√
28. To be balance the above reaction, the
coefficient of HCl should be ________________.
2Cu (s) + O2(g) → 2CuO (s)
2H2S (g) + 3O2(g) → 2SO2(g) + 2H2O(g)
6CO2(g) + 6H2O(l) → C6H12O6 (s) + 6O2(g)
A.
I only
B.
II only
C.
III only
D.
I, II and III
√
√
N2 + NH3 ⟶ H2
B.
NH3 + H2 ⟶ N2
C.
N2 ⟶NH3 + H2
D.
N2 + H2 ⟶ NH3
1
B.
2
C.
3
D.
4
______________________________________________________

Use the following information to answer
questions 29 and 30.
Iron, Fe, rusts when it reacts with oxygen gas,
O2, to form solid iron (III) oxide, Fe2O3.
26. Which of the following is the skeletal
equation for the production of ammonia,
NH3, from the reaction between nitrogen,
N2 and hydrogen, H2?
A.
A.
29. The reactant(s) for the above reaction
is/are ______.
√
__________________________________________________
 Use the reaction below to answer questions
27 and 28.
A.
Fe only
B.
O2 only
C.
Fe and O2 only
D.
O2 and Fe2O3 only
30. The unbalanced equation for the reaction
is:
Fe + O2  Fe2O3
HCl (aq) + Mg (s) ⟶ MgCl2 (aq) + H2 (g)
When the above equation is balanced, the
coefficient for O2 is ______.
27. The products in the above reaction are
_______.
√
A.
HCl and Mg
B.
MgCl2 and H2
C.
MgCl2 and Mg
D.
MgCl2 and HCl
Topic 5 – Practice Questions
√
5
A.
1
B.
2
C.
3
D.
4
Grade 10 – CHM 51

33. The ratio of coefficients needed to balance
the equation below is ______________.
Use the following information to answer
questions 31 and 32.
Magnesium ribbon, Mg, burns in oxygen gas,
O2, to form solid magnesium oxide, MgO.
31. The product(s) for the reaction is/are ______.
√
A.
Mg only
B.
MgO only
C.
MgO and O2 only
D.
Mg and MgO only
√
A.
1:1:1
B.
2:3:1
C.
2:1:3
D.
2:2:3
32. The equation for the reaction is
Mg + O2  MgO
When the above equation is balanced, the
coefficient for MgO is ______.
√
A.
2
B.
3
C.
4
D. 5
_____________________________________________________
34. Which of the following word equations represents the reaction described in the box below?
Iron rusts in the presence of oxygen to produce Iron oxide
√
A.
Iron + Iron oxide ⟶ Oxygen
B.
Iron + oxygen ⟶ Iron oxide
C.
Oxygen+ Iron oxide ⟶ Iron
D.
Iron + Iron oxide ⟶ di Iron oxide
Topic 5 – Practice Questions
6
Grade 10 – CHM 51

Consider the following reaction. Answer questions 35 and 36.
When solid aluminum is added to bromine gas, solid aluminum bromide is produced
35. The correct word equation for the reaction above is ___________________.
√
A.
aluminum bromide → aluminum + bromine
B.
aluminum bromide (s)→ aluminum(s) + bromine (g)
C.
aluminum bromide (s) + bromine (g) → aluminum (s)
D.
aluminum (s) + bromine (g) → aluminum bromide (s)
36. Which of the following is the correct skeleton equation for the reaction above?
√
A.
AlBr3 (s) →Al (s) + Br2 (g)
B.
Al (s) + Br2 (g) → AlBr3 (s)
C.
Al (s) + AlBr2 (s) → Br2 (g)
D.
Al (s) → AlBr2 (s) + Br2 (g)
_________________________________________________________________________________________________________________
37. Which of the following is an example of a chemical reaction?
I.
II.
III.
√
A.
I only
B.
II only
C.
I and III only
D.
I, II and III
Topic 5 – Practice Questions
7
Grade 10 – CHM 51
38. Consider the following reaction to answer questions a and b.
Hydrogen iodide gas breaks down into hydrogen gas and iodine gas
a) Write the word equation for the reaction above.
Hydrogen Iodide (g) → Hydrogen (g) + Iodine (g)
b) Write a skeleton equation for the reaction above.
HI (g) → H2 (g) + I2 (g)
_____________________________________________________________________________________________________________________
39. Write a balanced chemical equation with state symbols for the reaction below.
Sulfur dioxide gas reacts with oxygen gas to produce sulfur trioxide gas
2 SO2 (g) + O2 (g) → 2 SO3 (g)
40. Balance each of the following chemical equations.
a) ___NH3(g) + __O2 (𝑔) → __NO(g) + __H2 O(g)
4, 5, 4, 6
b) __Fe2 O3(g) + __H2 (𝑔) → __ Fe(s) + __H2 O(g)
1, 3, 2, 3
Topic 5 – Practice Questions
8
Grade 10 – CHM 51
 Subtopic 5.2 – Types of Chemical Reactions
41. The equation below is an example of a
_________ reaction.
44. Which of the following reactions produces
heat in the presence of oxygen?
2 C3H7OH(g) + 9O2(g)  6CO2(g) + 8H2O(g)
√
A.
synthesis
B.
combustion
C.
decomposition
D.
single replacement
√
√
B.
combustion
C.
decomposition
D.
single replacement
√
√
√
3 H2 (g) + N2 (g) → 2NH3 (g)
2 H2 (g) + O2 (g) → 2 H2 O(g)
CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2 O(g)
A.
I only
B.
II only
C.
I and II only
D.
II and III only
Topic 5 – Practice Questions
Combustion
C.
Decomposition
D.
Single replacement
A.
Synthesis
B.
Decomposition
C.
Single replacement
D.
Double replacement
46. Using the reactivity series identify which of
the following reactions will occur.
43. Which of the following is a combustion
reaction?
I.
II.
III.
B.
AX + BY → AY + BX
Ba(s) + 2 HCl(aq) BaCl2(aq) + H2(g)
synthesis
Synthesis
45. What type of chemical reaction is
represented by the equation below?
42. The equation below is an example of a
_________ reaction.
A.
A.
9
A.
Ca + CuBr2
B.
Cu + CaBr2
C.
Ag + NaCl
D.
Zn + NaCl
Grade 10 – CHM 51
47. Which of the following is true for the single
replacement reaction below?
49. The following particulate diagram
represents a __________ reaction.
MQ + Z → ZQ + M
√
A.
Element Q is more reactive
than element Z
B.
Element Z is more reactive
than element M
C.
Element M is more reactive
than element Z
D.
√
Elements M and Z have the
same reactivity
√
I only
B.
II only
C.
I and II only
D.
II and III only
Topic 5 – Practice Questions
synthesis
B.
decomposition
C.
single replacement
D.
double replacement
50. What type of chemical reaction is
represented by the particulate diagram
below?
48. What are the possible products of a
decomposition reaction?
I.
Two or more simple compounds
II.
Two or more elements
III.
One complex compound
A.
A.
√
10
A.
Synthesis
B.
Decomposition
C.
Double replacement
D.
Single replacement
Grade 10 – CHM 51
51. What is the type of reaction represented
below?
√
A.
Synthesis
B.
Decomposition
C.
Single replacement
D.
Double replacement
54. What is the type of the reaction below?
Zn(s) + CuSO4 (aq) → ZnSO4 (aq) + Cu(s)
√
√
synthesis
B.
combustion
C.
decomposition
D.
double replacement
√
53. Which of the following is a combustion
reaction?
I.
2Cu (s) + O2(g) → 2CuO (s)
II.
2H2S (g) + 3O2(g) → 2SO2(g) + 2H2O(g)
III.
6CO2(g) + 6H2O(l) → C6H12O6 (s) + 6O2(g)
√
A.
I only
B.
II only
C.
I and II only
D.
I, II and III
Topic 5 – Practice Questions
Hydrolysis
B.
Synthesis
C.
Single replacement
D.
Double replacement
55. What is the type of the reaction below?
2K + 𝐙𝐧𝐂𝐥𝟐(𝐚𝐪)  𝐙𝐧(𝐬) + 𝟐𝐊𝐂𝐥(𝐚𝐪)
52. A chemical reaction in which a single
compound breaks down to form two or
more new compounds or elements is known
as a ___________ reaction.
A.
A.
A.
Hydrolysis
B.
Synthesis
C.
Single replacement
D.
Double replacement
56. What happens when chlorine gas, Cl2(g) is
mixed with aqueous sodium iodide, NaI(aq) ?
I.
No visible reaction occurs
II.
Aqueous sodium chloride is produced
III.
Chlorine gas is released during the
reaction
A.
I only
√
B.
II only
C.
I and II only
D.
II and III only
57. A reaction in which two substances react to
form a single product is known as ________.
√
11
A.
synthesis
B.
combustion
C.
decomposition
D.
double replacement
Grade 10 – CHM 51
58. What is the type of the chemical reaction
given below?
Cl2 (g) + 2KBr (aq) ⟶ 2KCl (aq) + Br2 (l)
√
A.
Synthesis
B.
Precipitation
C.
Single replacement
D.
Double replacement
60. The reaction between copper metal, Cu, and
hydrochloric acid solution, HCl, __________
take place because _________.
59. When Zinc metal, Zn, is mixed with
hydrochloric acid, HCl, a reaction ________
because ____________.
√
A.
takes place
zinc is more
reactive than
hydrogen
B.
takes place
zinc is less
reactive than
hydrogen
C.
D.
√
A.
will
hydrogen is more reactive
than copper
B.
will
hydrogen is less reactive
than copper
C.
will not
hydrogen is less reactive
than copper
D.
will not
hydrogen is more reactive
than copper
61. The reaction between zinc metal, Zn, and
hydrochloric acid solution, HCl, __________
take place because _________.
√
does not take
place
zinc and hydrogen
have the same
reactivity
does not take
place
zinc is less
reactive than
hydrogen
A.
will
zinc is more reactive
than hydrogen
B.
will
zinc is less reactive
than hydrogen
C.
will not zinc and hydrogen
have the same
reactivity
will not zinc is less reactive
than hydrogen
D.
62. The reaction below is an example of a
_________ reaction.
HCl (aq) + Mg (s) ⟶ MgCl2 (aq) + H2 (g)
√
Topic 5 – Practice Questions
12
A.
combustion
B.
decomposition
C.
single replacement
D.
double replacement
Grade 10 – CHM 51
63. Using the reactivity series, predict whether each of the following reactions will occur or not. If a
reaction will occur, write (R), if the reaction does not occur write (NR).
a) Cu + MgCl2 →
________________________
NR
b) Cl2 + 2 HBr →
________________________
R
c) Mg + AgNO3 →
________________________
R
_____________________________________________________________________________________________________________________
64. Using the reactivity series, predict whether each of the following reactions will occur or not. If a
reaction will occur, write (R), if the reaction does not occur write (NR).
a) Mg + HCl →
________________________
R
b) Br2 + HCl →
________________________
NR
c) Cu + NaNO3 →
________________________
NR
_____________________________________________________________________________________________________________________
65. Using the given reactivity series, predict whether each of the following reactions will occur or not.
If a reaction will occur, write (R), if the reaction does not occur write (NR).
a) Ca + CuCl2 →
________________________
R
b) Cl2 + 2 NaF →
________________________
NR
c) Zn + AgNO3 →
________________________
R
_____________________________________________________________________________________________________________________
66. Using the given reactivity series, predict whether each of the following reactions will occur or not.
If a reaction will occur, write (R), if the reaction does not occur write (NR).
a) Cu + NaCl →
________________________
NR
b) Ca + H2SO4 →
________________________
R
c) I2 + 2 KCl →
________________________
NR
Topic 5 – Practice Questions
13
Grade 10 – CHM 51
67. For the following chemical reaction, identify the reactant(s), the product(s), the type of reaction
and write the word equation.
∆
K2CO3 (s) → K2O (s) + CO2 (g)
Reactant(s):
________________________
K2CO3
Product(s):
________________________
K2O and CO
Type of reaction:
________________________
Decomposition
Word equation:
_________________________________________________________________________________
Solid potassium carbonate breaks down or decomposes by heat to solid
potassium oxide and carbon dioxide gas
_____________________________________________________________________________________________________________________
68. For the following chemical reaction, identify the reactant(s), the product(s), the type of reaction
and write the word equation.
CaO (s) + CO2 (g) → CaCO3 (s)
Reactant(s):
________________________
CaO and CO2
Product(s):
________________________
CaCO3
Type of reaction:
________________________
Synthesis
____________________________________________________________________________________
Word equation:
Solid calcium oxide reacts with carbon dioxide gas to produce solid
calcium carbonate
_____________________________________________________________________________________________________________________
69. Balance and identify the type of each of the following chemical reactions.
Chemical equation
i)
Type of reaction
_2_ Na + _1_ Cl2 → _2_ NaCl
Synthesis
ii)
_1_ AgNO3 + _1_ NaCl → _1_ AgCl + _1_ NaNO3
iii)
_1_ C5H12 + _8_ O2 → _5_ CO2 + _6_ H2O
Topic 5 – Practice Questions
14
Double replacement
Combustion
Grade 10 – CHM 51
70. Identify the type of the chemical reaction given in the table below.
Chemical equation
Type of Chemical Reaction
C2H4 (g) + 3O2 (g) ⟶ 2CO2 (g) + 2H2O (g)
Combustion
Zn (s) + CuSO4 (aq) ⟶ ZnSO4 (aq) + Cu(s)
Single replacement
CaCO3 (s) ⟶ CaO (s) + CO2 (g)
Decomposition
H2 (g) + F2 (g) ⟶ 2 HF (g)
Synthesis
Ca(OH)2 (aq) + 2HCl (aq) ⟶ CaCl2 (aq) + 2H2O (l)
Double replacement
_____________________________________________________________________________________________________________________
71. Consider the following diagram to answer questions a – c.
a) Identify the type of reaction occurring.
Decomposition reaction
b) List two signs for a chemical reaction that can be inferred from the above diagram.
Production of a gas
Change of color
c) Write the balanced chemical equation for the reaction occurring.
CuCO3 (s) → CuO(s) + CO2 (g)
Topic 5 – Practice Questions
15
Grade 10 – CHM 51
72. A student carried out an experiment where he heated some solid ammonium carbonate,
(NH4)2CO3 (s), in a sealed test tube. The student observed the experiment and noticed that bubbles
of gas were produced. When the bubbles of gas were passed through lime water for a short time,
the lime water turned milky which proved that carbon dioxide gas, CO2 (g), was produced. The
students also noticed that a pungent smelling gas was produced, which he identified as ammonia
gas, NH3 (g). Water vapor, H2O(g), was also a product of the reaction. Answer questions a – c.
a) Identify the reactant(s), product(s) and type of reaction that occurred in the experiment.
________________________________
Ammonium carbonate
or (NH4)2CO3
Products (s):
________________________________
Ammonia, carbon dioxide and water
vapor
NH3, CO2 and H2O
Type of reaction:
________________________________
Decomposition
Reactant(s):
b) List one observation that indicates that a chemical reaction has taken place.
Bubbles of gas formed
c) Write balanced chemical equation for the reaction between magnesium and hydrochloric acid.
Include physical states for reactants and products.
(NH4)2CO3 (g) → 2 NH3 (g) + CO2 (g) + H2O (g)
Topic 5 – Practice Questions
16
Grade 10 – CHM 51
73. Consider the following diagram to answer questions a – c.
a) Identify the type of reaction occurring.
Synthesis reaction
b) Write word equation for the reaction occurring.
Iron reacts with sulfur to produce iron (II) sulfide
c) Write the balanced chemical equation for the reaction occurring.
Fe (s) + S (s)→ FeS
_____________________________________________________________________________________________________________________
74. Consider the reaction described in the box below to answer questions a – d.
Solid calcium (Ca) reacts with hydrochloric acid solution (HCl) to produce calcium
chloride solution (CaCl2) and hydrogen gas (H2)
a) Write the word equation for the above reaction.
Calcium + Hydrochloric acid ⟶ Calcium chloride + Hydrogen
b) Name the reactants and products in the above reaction.
Reactants:
Calcium and Hydrochloric acid
Products:
Calcium chloride and Hydrogen
c) Write a balanced chemical equation for the above reaction including the state symbols.
Ca (s) + 2HCl (aq) ⟶ CaCl2 (aq) + H2 (g)
d) Name the type of the above chemical reaction.
Single replacement
Topic 5 – Practice Questions
17
Grade 10 – CHM 51
75. A student carried out an experiment to test the reactivity of two metals: copper, Cu, and
magnesium, Mg, with dilute hydrochloric acid, HCl. He used 4 g of each metal and added each
separately to 100 mL of HCl as shown in the figure below. Answer questions a and b.
a) By referring to the figure above, identify the two metals X and Y. Explain your answer using the
reactivity series.
Metal X is copper (Cu)
Metal Y is magnesium (Mg)
Copper is below hydrogen in the reactivity series and cannot displace it thus a reaction does
not occur (and bubbles are not observed)
OR
Magnesium is above hydrogen in the reactivity series and can displace it thus a reaction occurs
(and bubbles are observed)
b) Write a balanced chemical equation for the reaction occurring.
Mg + 2 HCl → MgCl2 + H2
Topic 5 – Practice Questions
18
Grade 10 – CHM 51
76. A student carried out an experiment where he placed three pieces of magnesium ribbon, Mg(s), in a
beaker containing hydrochloric acid solution, HCl (aq). The student observed the experiment and
noticed that bubbles of gas were produced and a colorless solution of magnesium chloride MgCl2
is formed. When the bubbles of gas were tested with a lighted splint, they produced a pop sound,
which proved that the gas is hydrogen. Answer questions a – c.
a) Identify the reactant(s), product(s) and the type of reaction that occurred in the experiment.
Reactant(s):
________________________________
Mg and HCl
or
Magnesium and hydrochloric acid
Products (s):
________________________________
MgCl2 and H2
Magnesium chloride and hydrogen
________________________________
Single replacement reaction
(Must mention Single and
replacement)
Type of reaction:
b) List one observation that indicates that a chemical reaction has taken place.
Bubbles of gas formed
c) Write a balanced chemical equation for the reaction between magnesium and hydrochloric
acid. Include physical states symbols for reactants and products.
Mg (s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
Topic 5 – Practice Questions
19
Grade 10 – CHM 51
77. A student carried out an experiment where he heated some solid ammonium chloride, NH4Cl (s), in
a test tube. The student observed the experiment and noticed that bubbles of gas were produced.
The student identified the gases as ammonia gas, NH3 (g), and hydrogen chloride gas, HCl(g). Answer
questions a – c.
a) Identify the reactant(s), product(s) and type of reaction that occurred in the experiment.
(10 marks)
Reactant(s):
________________________________
Ammonium chloride
or NH4Cl
Products (s):
________________________________
NH3 and HCl
Ammonia and hydrogen chloride
Type of reaction:
________________________________
Decomposition
b) List one observation that indicates that a chemical reaction has taken place.
Bubbles of gas formed
c) Write a balanced chemical equation for the reaction above. Include physical states for
reactants and products.
NH4Cl (s) → NH3 (g) + HCl (g)
Topic 5 – Practice Questions
20
Grade 10 – CHM 51
78. Use the diagram below to answer question a and b.
a) In which experiment does a reaction take place? Explain your answer.
Experiment 1 because the color has changed and a new substance is formed
b) Is magnesium more or less reactive than silver? Justify your answer.
Magnesium is more reactive than silver because it can displace copper in solution while silver
cannot
_____________________________________________________________________________________________________________________
79. Use the diagram below to answer questions a and b.
a) In which of the above experiments did a chemical reaction take place? Justify your answer.
Experiment 1 because bubbles of gas are produced
b) Which metal is more reactive, X or Y? Justify your answer.
Metal X because it reacted with nitric acid while Y did not
Topic 5 – Practice Questions
21
Grade 10 – CHM 51
 Subtopic 5.3 – Reactions in Aqueous Solutions

4. Which of the following is the correct net
ionic equation for the above equation?
Na+(aq) + Cl−
A.
(aq) → NaCl(aq)
Use the following chemical equation to
answer question 1 – 4.
__NaOH(aq)+__CuCl2 (aq)→__NaCl(?)+__Cu(OH)2 (?)
1. Which of the following coefficients should be
used to correctly balance the above
chemical equation?
A.
√ B.
C.
D.
2
2
1
2
2
1
2
3
2
2
1
2
1
1
1
3
−
Na+(aq) + OH(aq)
→ NaOH(aq)
C.
−
Cu2+
(aq) + 2OH(aq) → Cu(OH)2(s)
−
Cu2+
D.
(aq) + 2Cl(aq) → CuCl2(aq)
____________________________________________________
5. Which of the following reactions is/are not a
net ionic equation(s)?
I.
H + (aq) + OH − (aq) ⟶ H2O (l)
II.
Zn2+ (aq) + S 2− (aq) ⟶ ZnS (s)
III.
2 Na(s) + Cl2 (g) ⟶ 2 NaCl (s)
2. Which of the following is a precipitate for
the above equation?
√
√
B.
√
A.
I only
B.
III only
A.
NaCl
B.
Cu(OH)2
C.
I and III only
C.
Both A and B
D.
II and III only
D.
There is no precipitate in the
above reaction
6. Which of the following reactions result in
the formation of a precipitate?
3. Which of these is/are the spectator ion(s) in
the above chemical equation?
I.
Cu2+
(aq)
II.
Na+(aq)
III.
Cl−
(aq)
I.
II.
III.
√
A. I only
B. II only
C.
III only
NaNO3 (aq) and CaCl2 (aq)
BaCl2 (aq) and Na2SO4 (aq)
NaNO3 (aq) and MgSO4 (aq)
A.
I only
B.
II only
C.
I and II only
D.
II and III only
√ D. II and III only
Topic 5 – Practice Questions
22
Grade 10 – CHM 51
7. The _______________ equation contains all
dissolved ionic compounds and highly
ionized molecular compounds shown as
ions.
√
A.
net ionic
B.
chemical
C.
skeletal
D.
complete ionic
10. The coefficient of NaNO3 is _____.
√
√
I and II only
B.
I and III only
C.
II and III only
D.
I, II and III
√
√
√
Ag+ and NO3ˉ
C.
Na+
D.
Na+ and NO3-
and
√
D.
4
A.
gas
B.
solid
C.
water
A.
K+ only
B.
K+ and Cl-
C.
K+ and NO3-
D.
Pb2+ and NO3-
A.
1
B.
2
C.
3
D.
4
14. The type of product in the above reaction
is/are ______.
S2-
√
Topic 5 – Practice Questions
3
13. The coefficient of KNO3 is _____.
9. The spectator ion(s) is/are ______.
B.
C.
12. The spectator ion(s) is/are ______.
Na2S (aq) + 2 AgNO3(aq) → Ag2S(s) + _____ NaNO3(aq)
Na+ only
2
2KCl (aq) + Pb(NO3)2 (aq) → PbCl2(s) + ____ KNO3(aq)
Consider the following equation to answer
questions 9 – 11.
A.
B.
D. colloid
______________________________________________________
 Consider the following equation to answer
questions 12 – 14.
______________________________________________________

1
11. The type of product in the above reaction is
______.
8. When silver nitrate solution, AgNO3, is
mixed with potassium bromide solution,
KBr, the products are ____.
I.
H2O
II.
KNO3
III.
AgBr
A.
A.
23
A.
gas
B.
solid
C.
water
D.
all of the above
Grade 10 – CHM 51
15. The _______________ equation includes only the particles that take part in the reaction.
√

A.
net ionic
B.
chemical
C.
skeletal
D.
complete ionic
Use the following reactions to answer questions 16 and 17.
Pb(NO3)2 (aq) + 2 KI (aq) ⟶ PbI2 (s) + 2 KNO3 (aq)
16. The net ionic equation for the following chemical equation is ___________.
√
A.
B.
C.
D.
Pb2+
(aq) +
−
2I(aq)
→ PbI2(s)
−
K+
(aq) + NO3 (aq) → KNO3(aq)
−
Pb2+
(aq) +2 NO3 (aq) → Pb(NO3 )2 (aq)
−
K+
(aq) + I (aq) → KI(aq)
17. The spectator ions in the reaction below are ______.
√
A.
K+ and I⁻
B.
Pb2+ and I⁻
C.
K+ and NO3⁻
D.
Pb2+ and NO3⁻
_____________________________________________________________________________________________________________________
18. The complete ionic equation for the reaction below is ________________________.
Ba(NO3)2 (aq) + Na2CO3 (aq) ⟶ BaCO3(s) + 2NaNO3 (aq)
√
A.
Ba2+ (aq) + CO2−
3 (aq) ⟶ BaCO3 (s)
B.
2−
−
+
+
Ba2+ (aq) + 2 NO−
3 (aq) + 2 Na (aq) + CO3 (aq) ⟶ BaCO3 (s)+ 2 Na (aq) + 2 NO3 (aq)
C.
+
Ba2+ (aq) + 2 NO−
3 (aq) + 2 Na
D.
+
2−
2−
−
2+
+
Ba2+ (aq) + 2 NO−
3 (aq) + 2 Na (aq) + CO3 (aq) ⟶ Ba (s) + CO3 (s) + 2 Na (aq) + 2 NO3 (aq)
Topic 5 – Practice Questions
(aq)
2−
2+
+ CO2−
3 (aq) ⟶ Ba (aq) + 2 CO3 (aq) + 2NaNO3 (s)
24
Grade 10 – CHM 51
19. The net ionic equation for the reaction below is ___________________________.
LiOH (aq) + HCl (aq) ⟶ LiCl (aq) + H2O (l)
√
A.
O2− (aq) + H + (aq) ⟶ H2O (l)
B.
Li+ (aq) + Cl− (aq) ⟶ LiCl (aq)
C.
OH − (aq) + H + (aq) ⟶ H2O (l)
D.
2OH − (aq) + 2H + (aq) ⟶ 3H2O (l)
20. The products of the reaction between Pb(NO3)2 (aq) and Li2SO4 (aq) are _________________
√
A.
PbSO4 (s) and LiNO3 (aq)
B.
PbLi (s) and SO4NO3 (aq)
C.
PbSO4 (aq) and LiNO3 (s)
D.
PbSO4 (aq) and LiNO3 (aq)
____________________________________________________________________________________________________________________
 Consider the following net ionic equation to answer questions 21 and 22.
𝟐−
𝐏𝐛𝟐+
(𝐚𝐪) + 𝐒(𝐚𝐪) → 𝐏𝐛𝐒(𝐬)
21. Which of the following is the complete ionic equation for the above net ionic equation?
√
A.
−
2−
+
Pb2+
(aq) + 2NO3 (aq) + S(aq) + 2Na(aq)
→ PbS(s) +2NO3− (aq) + 2Na+(aq)
B.
−
2−
+
Pb2+
(aq) + 2NO3 (aq) + S(aq) + 2Na (aq) → 2NaNO3(aq) + PbS(s)
C.
2−
2Na+(aq) + S(aq)
+ Pb(N𝑂3 )2 (𝑎𝑞)
D.
2−
Pb(N𝑂3 )2 (𝑎𝑞) + 2Na+(aq) + S(aq)
2−
+
−
→ Pb2+
(aq) + S(aq) + 2Na(aq) + 2NO3 (aq)
2−
→ 2NaNO3(aq) + Pb2+
(aq) + S(aq)
22. What is/are the product(s) of the above reaction?
√
A.
Pb(NO3)2 only
B.
NaNO3 only
C.
Na2 S and Pb(NO3)2
D.
PbS and NaNO3
Topic 5 – Practice Questions
25
Grade 10 – CHM 51
23. The state symbol for each product for the double replacement reaction below is ___________.
CuCl2 (aq) + Na2SO4 (aq) → CuSO4 (x) + 2 NaCl (y)
√
A.
B.
C.
D.
(x)
(s)
(aq)
(aq)
(s)
(y)
(aq)
(s)
(aq)
(s)
24. The net ionic equation for the reaction below is ___________________________.
CaCO3 (s) + 2HCl (aq) ⟶ CaCl2 (aq) + CO2 (g) + H2O (l)
√
A.
Ca2+ (aq) + 2Cl− (aq) ⟶ CaCl2 (aq)
B.
+
CO2−
3 (aq) + 2H (aq) ⟶ CO2 (g) + H2O (l)
C.
−
CO2−
3 (aq) + 2Cl (aq) ⟶ CO2 (g) + H2O (l)
D.
Ca2+ (aq) + 2H + (aq) ⟶ CO2 (g) + H2O (l)
25. The spectator ions in the reaction between BaCl2 (aq) and Na2SO4 (aq) are _______________________.
√
A.
Na+ and Cl−
B.
Ba2+ and Cl−
C.
Na+ and SO2−
4
D.
Ba2+ and SO2−
4
26. What are the products for the ionic equation given below?
2𝐀𝐠 + (aq) + 2𝐍𝐎𝟑− (aq) + 𝐂𝐚𝟐+ (aq) + 2𝐁𝐫 − (aq) ⟶ ______________________ + _____________________
√
A.
2 AgBr (aq)
Ca(NO3)2(aq)
B.
2 AgCa (s)
Br2(NO3)2(aq)
C.
2 AgBr(s)
Ca(NO3)2(aq)
D.
Ca(NO3)2(s)
2AgBr (aq)
Topic 5 – Practice Questions
26
Grade 10 – CHM 51
27.
I
The complete ionic equation is
different from the net ionic
equation
28.
I
Generally, the complete ionic
equation is the same as the net ionic
equation
Because
Because
II
The complete ionic equation has all
dissolved ionic compounds and highly
ionized molecular compounds shown
as ions.
II
The complete ionic equation includes
only the particles that take part in the
reaction.
_____________________________________________________________________________________________________________________
29. For the following reaction, write the complete ionic equation and net-ionic equation with state
symbols.
AgNO3 (aq) + NaCl (aq) → NaNO3 (aq) + AgCl (s)

Complete ionic equation
Ag+(aq) + NO3⎼ (aq) + Na+(aq) + Cl⎼(aq) → AgCl (s) + Na+(aq) + NO3⎼ (aq)

Net-ionic equation
Ag+(aq) + Cl⎼(aq) → AgCl (s)
Topic 5 – Practice Questions
27
Grade 10 – CHM 51
30. For the following reaction, write the complete ionic equation and net-ionic equation and type
of product formed in each of the following reactions.
2 NaOH (aq) + CuCl2 (aq) → 2NaCl (aq) + Cu(OH)2 (s)

Complete ionic equation
2 Na+(aq) + 2 OH⎼ (aq) + Cu2+(aq) + 2Cl⎼(aq) → Cu(OH)2 (s) + 2 Na+(aq) + 2Cl⎼(aq)

Net-ionic equation
Cu2+(aq) + 2 OH⎼(aq) → Cu(OH)2 (s)
____________________________________________________________________________________________________________________
31. Identify the spectator ions and the write the net ionic equation including state symbols for the
reaction between NaCl (aq) and AgNO3 (aq).
Spectator ions:
Na+ and NO−
3
Net ionic equation:
Ag + (aq) + Cl− (aq) ⟶ AgCl (s)
_____________________________________________________________________________________________________________________
32. Consider the reaction between copper (II) sulfate solution, CuSO4, and barium nitrate solution,
Ba(NO3)2, to answer questions a – c.
a) Write the balanced chemical equation with state symbols for the above reaction.
CuSO4 (aq) + Ba(NO3)2 (aq) ⟶ Cu(NO3)2 (aq) + BaSO4 (s)
b) Write the complete ionic equation for the above reaction.
−
−
2+
2+
Cu2+ (aq)+ SO2−
(aq) + 2NO3 (aq) ⟶ BaSO4 (s) + Cu
(aq) + 2NO3 (aq)
4 (aq) + Ba
c) Write the net ionic equation for the above reaction
Ba2+ (aq) + SO2−
4 (aq) ⟶ BaSO4 (s)
Topic 5 – Practice Questions
28
Grade 10 – CHM 51
33. Use the table below to identify the spectator ions and write the net ionic equation with state
symbols for each of the given reacting solutions.
Reactants
Spectator ions
Net ionic equation
KI (aq) and AgNO3 (aq)
K + and NO−
3
Ag + (aq) + I − (aq) ⟶ AgI (s)
CaCl2(aq) and Na2SO4 (aq)
Na+ and Cl−
Ca2+ (aq) + SO42― (aq) ⟶ CaSO4 (s)
_____________________________________________________________________________________________________________________
34. A student was given three different bottles X, Y and Z. The bottles lost their labels. The student
was informed by the teacher that the bottles contain three chemicals in no specific order:
“Potassium carbonate, K2CO3, hydrochloric acid, HCl, and calcium nitrate, Ca(NO3)2”
The student performed different experiments and recorded the results in the table below.
Solution
X
X
Y
Precipitate
Z
No reaction
Y
Z
Precipitate
No reaction
Gas produced
Gas produced
Identify the contents of each bottle.
X:
___________________
Ca(NO3)2
Y:
___________________
K2CO3
Z:
___________________
HCl
Topic 5 – Practice Questions
29
Grade 10 – CHM 51
35. Consider the following two solutions. Answer questions a – d.
a) Name the solute and solvent in the calcium chloride solution.
Solute:
___________________
Calcium chloride
Solvent:
___________________
water
b) Write the complete balanced chemical equation with state symbols for the above
reaction.
CaCl2 (aq) + K2CO3 (aq) ⟶ CaCO3 (s) + 2KCl (aq)
c) Write the complete ionic equation for the above reaction
Ca2+ (aq)+2Cl−
(aq)
−
+
+ 2K + (aq) + CO2−
3 (aq) ⟶ CaCO3 (s) + 2K (aq) + 2Cl
(aq)
d) Write the net ionic equation for the above reaction.
Ca2+ (aq) + CO2−
3 (aq) ⟶ CaCO3 (s)
Topic 5 – Practice Questions
30
Grade 10 – CHM 51
36. A student mixed aqueous solutions of iron (III) chloride, FeCl3, and sodium hydroxide, NaOH. He
noticed that a precipitate was formed and a colorless solution. The student sketched the diagram
below. Answer questions a and b.
a) Write the balanced chemical equation with state symbols.
FeCl3(aq) + 3 NaOH(aq) → Fe(OH)3 (s) + 3 NaCl(aq)
b) Write the net ionic equation for the reaction occurring.
−
Fe3+
→ Fe(OH)3(s)
(aq) + 3 OH(aq)
_____________________________________________________________________________________________________________________
37. A student mixed aqueous solutions of iron (II) chloride, FeCl2, and potassium hydroxide, KOH. He
noticed that a precipitate was formed and a colorless solution. The student sketched the diagram
below. Answer questions a and b.
a) Write the balanced chemical equation with state symbols.
FeCl2(aq) + 2 KOH(aq) → Fe(OH)2 (s) + 2 KCl(aq)
b) Write the net ionic equation for the reaction occurring.
−
Fe2+
(aq) + 2 OH(aq)
Topic 5 – Practice Questions
→ Fe(OH)2(s)
31
Grade 10 – CHM 51
38. A student carried out an experiment where he mixed barium chloride solution, BaCl2, and sodium
sulphate solution, Na2SO4. The student observed that a precipitate was formed and a colorless
solution. The student sketched the diagram below. Answer questions a and b.
a) Write the balanced chemical equation with state symbols.
BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2 NaCl(aq)
b) Write the net ionic equation for the reaction occurring.
2−
Ba2+
(aq) + SO4 (aq)
Topic 5 – Practice Questions
→ BaSO4(s)
32
Grade 10 – CHM 51
39. Using the given solubility rules, complete each of the following chemical equations by writing the
formula of each product and its state symbol.
a) 2 NaOH (aq) + FeCl2 (aq) → ____________________ + ____________________
2 NaCl (aq) and Fe(OH)2 (s)
b) 2 AgNO3 (aq) + Na2S (aq) → ____________________ + _____________________
2 NaNO3 (aq), Ag2S (s)
c) CaCl2 (aq) + MgSO4 (aq) → ____________________ + ____________________
MgCl2 (aq), CaSO4 (s)
d) AgNO3 (aq) + NaI (aq) → ____________________ + ____________________
AgI(s) , NaNO3 (aq)
_____________________________________________________________________________________________________________________
40. A student mixed solutions of calcium chloride, CaCl2 (aq), and sodium carbonate, Na2CO3 (aq). He
noticed that a white precipitate was formed and a colorless solution was produced. Answer
questions a – d.
a) Write a balanced chemical equation with state symbols for the reaction that occurred.
CaCl2 (aq) + Na2CO3 (aq) → 2 NaCl (aq) + CaCO3 (s)
b) Write complete ionic equation for the reaction that occurred.
Ca2+(aq) + 2 Cl―(aq) + 2 Na+(aq) + CO32―(aq) → 2 Na+(aq) + 2 Cl― (aq) + CaCO3 (s)
c) Write the net ionic equation for the reaction that occurred.
Ca2+(aq) + CO32― (aq) → CaCO3 (s)
d) Identify the spectator ion(s).
Na+(aq) and Cl― (aq)
Topic 5 – Practice Questions
33
Grade 10 – CHM 51
41. A student mixed solutions of sodium sulfate, Na2SO4 (aq) and barium nitrate, Ba(NO3)2 (aq). He
noticed that a white precipitate was formed and a colorless solution. Answer questions a – d.
a) Write a balanced chemical equation with state symbols for the reaction that occurred.
Na2SO4 (aq) + Ba(NO3)2 (aq) → 2 NaNO3 (aq) + BaSO4 (s)
b) Write the net ionic equation for the reaction that occurred.
Ba2+(aq) + SO42― (aq) → BaSO4 (s)
c) Identify the spectator ion(s).
Na+(aq) and NO3― (aq)
d) Write the word equation for the reaction that took place.
Sodium sulfate + barium nitrate → sodium nitrate + barium sulfate
Topic 5 – Practice Questions
34
Grade 10 – CHM 51
 Subtopic 5.4 – Combustion Reactions
1. The combustion of hexane, C6H14, would
____________.
√
A.
require 10 O2 (g)
B.
produce 6 CO2 (g)
C.
D.
3. If two moles of butane, C4H10, undergo
complete combustion, ____________.
A.
8 CO is produced
B.
8 CO2 is produced
produce 8 H2O (g)
C.
9 O2 is a reactant
All of the above
D.
2 O2 is a reactant
√
2. The complete combustion of two moles of
octane, C8H18, would ____________.
I.
require 25 O2 (g)
II.
produce 16 CO2 (g)
III.
produce 18 H2O (g)
√
4. The correct balanced chemical equation
for the complete combustion of carbon, C,
is _________.
√
A.
C (s) + O2 (g) ⟶ CO2 (g)
B.
CO2 (g) + O2 (g) ⟶ C (s)
A.
I only
B.
II only
C.
CO2 (g) ⟶ C (s) + O2 (g)
C.
I and III only
D.
C (s) + O2 (g) ⟶ CO3 (g)
D.
I, II and III
_____________________________________________________________________________________________________________________
5. Consider the chemical reaction described below to answer questions a – c.
Ethane (C3H8) burns in the presence of oxygen to produce carbon dioxide
(CO2), water vapor (H2O), light and heat
a) Write the word equation for the above reaction.
Ethane + Oxygen ⟶ Carbon dioxide + Water vapor
b) Write the balanced chemical equation for the above reaction including all state symbols.
C3H8 (g) + 5 O2 (g) ⟶ 3 CO2 (g) + 4 H2O (g)
c) Name the type of the chemical reaction.
Combustion
Topic 5 – Practice Questions
35
Grade 10 – CHM 51