Practice Test#1
Chapter 1 - Kinetics
Chapter 1 – Kinetics - Practice Test #1
Name - _________________
The answers to this test are posted online
1.
2.
Consider the following reaction mechanism:
step 1:
M
+
X
→
step 2:
MX +
A
→
The chemical species MX is a(n)
A.
catalyst
B.
inhibitor
X
final product
reaction intermediate
2.5 x 10-6 mol/s
5.0 x 10-6 mol/s
C.
D.
Which of the following factors affect the rates of both homogeneous and heterogeneous
reactions.
A.
B.
nature of the reactants
presence of a catalyst
temperature of system
concentration of reactants
I and IV only
II and III only
C.
D.
II, III, and IV only
I, II, III, and IV
Which of the following equations represents an endothermic reaction?
A.
B.
C.
D.
5.
C.
D.
1.0 x 10-5 mol/s
1.3 x 10-6 mol/s
I
II
III
IV
4.
+
Consider the following reaction:
2N2O5(g) → 4NO2(g) + O2(g)
At a certain temperature the rate of decomposition of 2N2O5(g) is 2.5 x 10-6 mol/s. The rate of
formation of NO2 is
A.
B.
3.
MX
D
N2O4(g)
2H2(g)
2BrCl(g)
2H2(g)
+ 59 kJ → 2NO2(g)
+ O2(g) → 2H2O(l) + 572 kJ
-29.3 kJ →Br2(g) + Cl2(g)
+ O2(g) → 2H2O(l)
ΔH
= -572 kJ
Consider the potential energy diagram. The activation energy for the reverse reaction is
A.
B.
30 kJ
140 kJ
PE
(kJ)
C.
170 kJ
D.
200 kJ
170kJ
30kJ
Progress of the reaction
Practice Test#1
6.
Consider the following mechanism: Step 1:
Step 2:
The reaction intermediate is
A.
B.
7.
C.
D.
O3
ClO
fastest and has the lowest activation energy.
fastest and has the highest activation energy.
slowest and has the lowest activation energy.
slowest and has the highest activation energy.
increasing the concentration of reactant(s).
decreasing the concentration of the reactant(s).
increasing the activation energy of the overall reaction.
decreasing the activation energy of the overall reaction.
Which of the following properties could be used to measure the rate of the following reaction in
a open container. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
A.
B.
10.
Cl
O2
+ O2
+ O2
A catalyst increases the rate of a reaction by
A.
B.
C.
D.
9.
Cl + O3 → ClO
O + ClO → Cl
In a reaction mechanism, the rate determining step is the
A.
B.
C.
D.
8.
Chapter 1 - Kinetics
mass of Zn
solubility of HCl
Consider the following potential energy diagram:
PE
(kJ)
Progress of the reaction
The above diagram represents an
A.
B.
C.
D.
exothermic reaction involving one step.
exothermic reaction involving two steps.
endothermic reaction involving one step.
endothermic reaction involving two steps.
C.
D.
concentration of Clcolour of the solution
Practice Test#1
11.
Which of the following are necessary for successful collisions to occur?
I.
II.
III.
A.
B.
12.
Chapter 1 - Kinetics
Favourable geometry
Sufficient energy
Large ΔH
I only
I and II only
Consider the following reaction:
C.
D.
2H2O2(aq) →
II and III only
I, II, and III
2H2O(l) + O2(g)
When 1.0 g of KI is added to the H2O2, bubbles of O2 are produced at an increased rate, The KI
is a
A.
B.
13.
product
catalyst
C.
D.
reactant
intermediate
Consider the following
I.
Frequency of successful collision
II.
Volume of the reaction vessel
III.
Pressure of the system
IV
Mass of the system
To increase the rate of a chemical reaction there must be an increase in
A.
B.
14.
I only
I and III only
Consider the following reaction mechanism:
Step1: ICl + H2 → HI + HCl slow
Step 2: ICl + HI → HCl + I2 fast
The species HCl is a
A.
B.
C.
D.
product
catalyst
reactant
reaction intermediate
C.
D.
I, III and IV only
I, II, III, and IV
Practice Test#1
15.
Chapter 1 - Kinetics
Consider the following potential energy diagram:
125
PE
(kJ)
100
75
50
25
Progress of the reaction
The activation energy in the forward direction is
A.
B.
16.
C.
D.
75 kJ
125 kJ
Consider the following reactions:
I.
N2 + O2(g) → 2NO(g)
II.
Mg(s) + O2(g) → 2MgO(s)
III.
CaCO3(s) + 2H+(aq) → Ca2+ (aq) + H2O(l) + CO2(g)
Increasing the surface area will increase the reaction rate in
A.
B.
17.
25 kJ
50 kJ
II only
I and III only
C.
D.
II and III only
I, II, and III
C.
D.
V3+
Fe3+
Consider the following reaction mechanism:
Step 1: V3+ + Cu2+ → V4+ + Cu+
Step 2: Cu+ + Fe3+→ Cu2+ + Fe2+ slow
The reaction intermediate is
A.
B.
18.
Cu+
Cu2+
The rate of a chemical reaction can be expressed in
A.
B.
C.
D.
grams per mole
energy consumed per mole
volume of gas per unit time
mole formed per litre of solution
Practice Test#1
19.
Consider the following reaction:
2MnO4-(aq) + 5C2O42-(aq) 16H+(aq) → 2Mn2+(aq) + 10CO2(g) + 8H2O(l)
The rate of decomposition of the oxalate ion is increased by
A.
B.
20.
adding NaOH.
removing CO2
C.
D.
adding a catalyst
decreasing the pressure
The minimum amount of energy needed to start a reaction is called the
A.
B.
21.
Chapter 1 - Kinetics
activation energy.
energy of reaction.
C.
D.
entropy of reaction
reaction mechanism energy
An 8.00g piece of magnesium was placed into 6.0 M HCl. After 25 s, 3.50 g of unreacted
magnesium remained. The average rate at which magnesium was consumed is
A.
B.
C.
D.
0.14 g/s
0.18 g/s
0.32 g/s
4.50 g/s
22.
In general rates double when the temperature is increased by 10 oC. The temperature of a
reaction is increased by 40 oC. The rate will increase by a factor of
A.
2
C.
8
B.
4
D.
16
23.
Consider the following factors
I.
reactant particles collide
II.
sufficient kinetic energy is present
III.
a favourable geometry exists
IV.
catalysts are present
Which combination of the above factors is required for all successful collisions?
A.
B.
24.
C.
D.
I, II and III only
I, II, III, and IV
Consider the following reaction at constant temperature in an open system:
MgCO3(s) + 2HCl(aq) → CO2(g) + H2O(l) + MgCl2(aq)
Which of the following properties could be used to determine the reaction rate.
A.
B.
25.
I only
II and III only
mass of the system
pressure of the gas
C.
D.
concentration of H2O
concentration of MgCO3
Which combination of factors will affect the rate of the following reaction?
MgCO3(s) + 2HCl(aq) → CO2(g) + H2O(l) + MgCl2(aq)
A.
temperature and surface area only
B.
temperature and concentration only
C.
concentration and surface area only
D.
temperature, concentration, and surface area only
Practice Test#1
26.
Chapter 1 - Kinetics
As reactant molecules approach each other
A.
B.
C.
D.
heat is released
a reaction intermediate forms
kinetic energy changes into potential energy
potential energy changes into kinetic energy
Consider the following potential energy diagram for the next three five questions.
2
PE
4
1
3
Progress of reaction
27.
The interval representing ΔH for the reverse reaction is
A.
B.
28.
1
2
C.
D.
3
4
1
2
C.
D.
3
4
C.
D.
3
4
The interval representing Ea for the forward reaction is
A.
B.
31.
3
4
The interval representing Ea for the reverse reaction is
A.
B.
30.
C.
D.
The interval representing ΔH for the forward reaction is
A.
B.
29.
1
2
1
2
The interval representing the energy of the activated complex is
A.
B.
1
2
C.
D.
3
4
Practice Test#1
32.
When a catalyst is added to a reaction, ΔH will
A.
B.
C.
D.
33.
Chapter 1 - Kinetics
increase slowly
remain constant
decrease slowly
increase rapidly due to the alternate pathway
Consider the following reaction: Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
Data for the reaction is shown below:
Time
Mass of Zn (g)
Volume of H2 (mL)
Temperature (oC)
4.65
4.50
4.35
0
50
100
20
21
22
0
2
4
The rate of the reaction can be measured in units of
A.
B.
34.
min/mL
g/(mL)(oC)
behaves as a catalyst
supplies the activation energy
is part of the rate determining step
lowers the activation energy barrier
Consider the following reaction: 2NO(g) + O2(g) → 2NO2(g) + 112 kJ
ΔH for the above reaction is:
A.
B.
C.
D.
36.
C.
D.
When a lit match is touched to the wick of a candle, the candle begins to burn. When the match
is removed, the candle continues to burn, the match,
A.
B.
C.
D.
35.
g/min
g/mL
positive and the reaction is exothermic
negative and the reaction is exothermic
positive and the reaction is endothermic
negative and the reaction is endothermic
Consider the following reaction: 2S(s) + 3O2(g) → 2SO2(g) + heat
The rate of this reaction could be increased by
A.
B.
C.
D.
decreasing the temperature
adding a catalyst
increasing the concentration of S
decreasing the surface area of the S
Practice Test#1
Chapter 1 - Kinetics
37.
Consider the following reaction: ½H2 + ½I2 → HI ΔH = +28 kJ
The activation energy for the formation of HI is 167 kJ. The activation energy for the
decomposition of HI is
A.
28 kJ
C.
167 kJ
B.
139 kJ
D.
195 kJ
38.
Some reactants are more reactive than others because of their activation energy Ea. What graph
shows the relationship between Ea and rate.
A.
B.
Ea
Ea
Rate
C.
D.
Ea
Rate
39.
Ea
Rate
The activated complex is a chemical species that is
A.
B.
40.
Rate
stable and has low PE.
stable and has high PE.
As an activated complex changes into products,
A.
B.
C.
D.
potential energy changes into kinetic energy.
kinetic energy changes into potential energy.
kinetic energy changes into activation energy.
potential energy changes into activation energy.
C.
D.
unstable and has low PE.
unstable and has high PE.
Practice Test#1
Chapter 1 - Kinetics
Long Answer – Written response Questions
PE
Progress of the reaction
1.
On the potential energy diagram above, clearly label the activation energy, heat of the reaction
(∆H), and the energy of the activated complex.
2.
Is the above reaction endothermic or exothermic in the forward direction?
3.
On the graph below, draw the potential energy diagram for an exothermic reaction and label the
activation energy.
PE
Progress of the reaction
4.
a)
Nitric oxide (NO) is involved in the decomposition of ozone by the following mechanism:
Step 1: O3 + sunlight → O2 + O
Step 2: O3 + NO → NO2 + O2
Step 3: NO2 + O → NO + O2
Write the net equation for the decomposition reaction
b)
Identify a catalyst
c)
Identify a reaction intermediate
Practice Test#1
Chapter 1 - Kinetics
d)
What is the function of sunlight in this reaction?
5.
Consider the following reaction:
a)
Explain why the reaction is likely to involve more than one step.
b)
A proposed mechanism for the above reaction is:
Step 1: NO + H2 → N + H2O
Step 2:
?
Step 3: N2O + H2 → N2 + H2O
2NO + 2H2 → 2H2O + N2
Write the equation for step 2.
6.
Define the term activation energy.
7.
The combustion of coal, C, produces carbon dioxide and water according to the following
equation: C(s) + O2(g) → CO2(g) + 394 kJ
a)
What is ∆H for this reaction?
b)
Using the collision theory, explain why a lump of coal does not react with oxygen at
room temperature and pressure.
c)
Many coalmine disasters have resulted when a spark ignites coal dust in the air. Explain using
the collision theory.
8.
State two reasons why some collisions may not result in a chemical reaction.
Practice Test#1
9.
Chapter 1 - Kinetics
A student wishes to monitor the rate of the following reaction:
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
Identify two different properties that could be used to monitor the rate of the reaction. Describe
and explain the changes that would occur.
Property 1
Change and explanation
Property 2
Change and explanation
10.
An experiment is done to determine the rate of the following reaction:
2Al(s) + 6HCl(aq) → 3H2(g) + 2AlCl3(aq)
The following data are collected
Time (s)
Mass of Flask + Contents (g)
0.0
30.0
60.0
270.230
270.200
270.170
Calculate the rate of consumption of Al in mol/min.
270.170
Practice Test#1
Chem 12
Chapter 1 - Kinetics
Practice Test 1
Answers
1. Consider the following reaction mechanism:
step 1:
M
+
X
→
step 2:
MX +
A
→
The chemical species MX is a(n)
A.
catalyst
B.
inhibitor
C.
final product
D.
reaction intermediate
MX
D
+
X
2. Consider the following reaction: 2N2O5(g)
→
4NO2(g)
+
O2(g)
At a certain temperature the rate of decomposition of 2N2O5(g) is 2.5 x 10-6 mol/s. The rate of
formation of NO2 is
A.
B.
C.
D.
1.0
1.3
2.5
5.0
x
x
x
x
10-5 mol/s
10-6 mol/s
10-6 mol/s
10-6 mol/s
3. Which of the following factors affect the rates of both homogeneous and heterogeneous reactions.
I
II
III
IV
A.
B.
C.
D.
nature of the reactants
presence of a catalyst
temperature of system
concentration of reactants
I and IV only
II and III only
II, III, and IV only
I, II, III, and IV
4. Which of the following equations represents an endothermic reaction?
A.
B.
C.
D.
N2O4(g)
2H2(g)
2BrCl(g)
2H2(g)
+ 59 kJ → 2NO2(g)
+ O2(g) → 2H2O(l) + 572 kJ
-29.3 kJ →Br2(g) + Cl2(g)
+ O2(g) → 2H2O(l)
ΔH
= -572 kJ
Practice Test#1
Chapter 1 - Kinetics
5. Consider the potential energy diagram. The activation energy for the reverse reaction is
A.
B.
30 kJ
140 kJ
PE
(kJ)
30kJ
170kJ
C.
170 kJ
D.
200 kJ
Progress of the reaction
6. Consider the following mechanism:
Step 1:
Step 2:
Cl + O3 → ClO
O + ClO → Cl
+ O2
+ O2
The reaction intermediate is
A.
B.
C.
D.
Cl
O2
O3
ClO
7. In a reaction mechanism, the rate determining step is the
A.
B.
C.
D.
fastest and has the lowest activation energy.
fastest and has the highest activation energy.
slowest and has the lowest activation energy.
slowest and has the highest activation energy.
8. A catalyst increases the rate of a reaction by
A.
B.
C.
D.
increasing the concentration of reactant(s).
decreasing the concentration of the reactant(s).
increasing the activation energy of the overall reaction.
decreasing the activation energy of the overall reaction.
9. Which of the following properties could be used to measure the rate of the following reaction in a
open container. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
A.
B.
C.
mass of Zn
solubility of HCl
concentration of Cl-
Practice Test#1
D.
colour of the solution
Chapter 1 - Kinetics
Practice Test#1
Chapter 1 - Kinetics
10. Consider the following potential energy diagram:
PE
(kJ)
Progress of the reaction
The above diagram represents an
A.
B.
C.
D.
exothermic reaction involving one step.
exothermic reaction involving two steps.
endothermic reaction involving one step.
endothermic reaction involving two steps.
11. Which of the following are necessary for successful collisions to occur?
I.
II.
III.
A.
B.
C.
D.
Favourable geometry
Sufficient energy
Large ΔH
I only
I and II only
II and III only
I, II, and III
12. Consider the following reaction: 2H2O2(aq) →
2H2O(l) + O2(g)
When 1.0 g of KI is added to the H2O2, bubbles of O2 are produced at an increased rate, The KI is a
A.
B.
C.
D.
product
catalyst
reactant
intermediate
PE
(kJ)
Practice Test#1
Chapter 1 - Kinetics
13. Consider the following
I.
Frequency of successful collision
II.
Volume of the reaction vessel
III.
Pressure of the system
IV
Mass of the system
To increase the rate of a chemical reaction there must be an increase in
A.
B.
C.
D.
I only
I and III only
I, III and IV only
I, II, III, and IV
14. Consider the following reaction mechanism: Step1: ICl + H2 → HI + HCl slow
Step 2: ICl + HI → HCl + I2 fast
The species HCl is a
A.
B.
C.
D.
product
catalyst
reactant
reaction intermediate
15.Consider the following potential energy diagram:
125
100
75
50
25
Progress of the reaction
The activation energy in the forward direction is
A.
B.
C.
D.
25 kJ
50 kJ
100 kJ
125 kJ
Practice Test#1
Chapter 1 - Kinetics
16. Consider the following reactions:
I.
N2 + O2(g) → 2NO(g)
II.
Mg(s) + O2(g) → 2MgO(s)
III.
CaCO3(s) + 2H+(aq) → Ca2+ (aq) + H2O(l) + CO2(g)
Increasing the surface area will increase the reaction rate in
A.
B.
C.
D.
II only
I and III only
II and III only
I, II, and III
17. Consider the following reaction mechanism: Step 1: V3+ + Cu2+ → V4+ + Cu+ slow
Step 2: Cu+ + Fe3+→ Cu2+ + Fe2+ slow
The reaction intermediate is
A.
B.
C.
D.
Cu+
Cu2+
V3+
Fe3+
18. The rate of a chemical reaction can be expressed in
A.
B.
C.
D.
grams per mole
energy consumed per mole
volume of gas per unit time
mole formed per litre of solution
19. Consider the following reaction:
2MnO4-(aq) + 5C2O42-(aq) 16H+(aq) → 2Mn2+(aq) + 10CO2(g) + 8H2O(l)
The rate of decomposition of the oxalate ion is increased by
A.
B.
C.
D.
adding NaOH.
removing CO2
adding a catalyst
decreasing the pressure
20. The minimum amount of energy needed to start a reaction is called the
A.
B.
C.
D.
activation energy.
energy of reaction.
entropy of reaction
reaction mechanism energy
Practice Test#1
Chapter 1 - Kinetics
21. An 8.00g piece of magnesium was placed into 6.0 M HCl. After 25 s, 3.50 g of unreacted
magnesium remained. The average rate at which magnesium was consumed is
A.
B.
C.
D.
0.14 g/s
0.18 g/s
0.32 g/s
4.50 g/s
22. In general rates double when the temperature is increased by 10 oC. The temperature of a reaction
is increased by 40 oC. The rate will increase by a factor of
A.
B.
C.
D.
2
4
8
16
23. Consider the following factors
I.
reactant particles collide
II.
sufficient kinetic energy is present
III.
a favourable geometry exists
IV.
catalysts are present
Which combination of the above factors is required for all successful collisions?
A.
B.
C.
D.
I only
II and III only
I, II and III only
I, II, III, and IV
24. Consider the following reaction at constant temperature in an open system:
MgCO3(s) + 2HCl(aq) → CO2(g) + H2O(l) + MgCl2(aq)
Which of the following properties could be used to determine the reaction rate.
A.
B.
C.
D.
mass of the system
pressure of the gas
concentration of H2O
concentration of MgCO3
25. Which combination of factors will affect the rate of the following reaction?
MgCO3(s) + 2HCl(aq) → CO2(g) + H2O(l) + MgCl2(aq)
A.
temperature and surface area only
B.
temperature and concentration only
C.
concentration and surface area only
D.
temperature, concentration, and surface area only
Practice Test#1
Chapter 1 - Kinetics
26. As reactant molecules approach each other
A.
B.
C.
D.
heat is released
a reaction intermediate forms
kinetic energy changes into potential energy
potential energy changes into kinetic energy
Consider the following potential energy diagram for the next three five questions.
2
PE
4
1
3
Progress of reaction
27. The interval representing ΔH for the reverse reaction is
A.
B.
C.
D.
1
2
3
4
28. The interval representing ΔH for the forward reaction is
A.
B.
C.
D.
1
2
3
4
29. The interval representing Ea for the reverse reaction is
A.
B.
C.
D.
1
2
3
4
Practice Test#1
Chapter 1 - Kinetics
30. The interval representing Ea for the forward reaction is
A.
B.
C.
D.
1
2
3
4
31. The interval representing the energy of the activated complex is
A.
B.
C.
D.
1
2
3
4
32. When a catalyst is added to a reaction, ΔH will
A.
B.
C.
D.
increase slowly
remain constant
decrease slowly
increase rapidly due to the alternate pathway
33. Consider the following reaction: Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
Data for the reaction is shown below:
Time
Mass of Zn (g)
Volume of H2 (mL)
Temperature (oC)
0
2
4
4.65
4.50
4.35
0
50
100
20
21
22
The rate of the reaction can be measured in units of
A.
B.
C.
D.
g/min
g/mL
min/mL
g/(mL)(oC)
34. When a lit match is touched to the wick of a candle, the candle begins to burn. When the match is
removed, the candle continues to burn, the match,
A.
B.
C.
D.
behaves as a catalyst
supplies the activation energy
is part of the rate determining step
lowers the activation energy barrier
35. Consider the following reaction: 2NO(g) + O2(g) → 2NO2(g) + 112 kJ
ΔH for the above reaction is:
Practice Test#1
A.
B.
C.
D.
Chapter 1 - Kinetics
positive and the reaction is exothermic
negative and the reaction is exothermic
positive and the reaction is endothermic
negative and the reaction is endothermic
36. Consider the following reaction: 2S(s) + 3O2(g) → 2SO2(g) + heat
The rate of this reaction could be increased by
A.
B.
C.
D.
decreasing the temperature
adding a catalyst
increasing the concentration of S
decreasing the surface area of the S
37. Consider the following reaction: ½H2 + ½I2 → HI ΔH = +28 kJ
The activation energy for the formation of HI is 167 kJ. The activation energy for the decomposition of
HI is
A.
B.
C.
D.
28 kJ
139 kJ
167 kJ
195 kJ
38. Some reactants are more reactive than others because of their activation energy Ea. What graph
shows the relationship between Ea and rate.
A.
B.
Ea
Ea
Rate
C.
Rate
D.
Ea
Rate
Ea
Rate
39. The activated complex is a chemical species that is
`
A.
stable and has low PE.
B.
stable and has high PE.
C.
unstable and has low PE.
D.
unstable and has high PE.
Practice Test#1
Chapter 1 - Kinetics
40. As an activated complex changes into products,
A.
B.
C.
D.
potential energy changes into kinetic energy.
kinetic energy changes into potential energy.
kinetic energy changes into activation energy.
potential energy changes into activation energy.
Chemistry 12
PE
1999
Subjective
Ea
∆H
energy of activated complex
Progress of the reaction
1. On the potential energy diagram above, clearly label the activation energy, heat of the reaction
(∆H), and the energy of the activated complex.
(3 marks)
2. Is the above reaction endothermic or exothermic in the forward direction? (1 mark)
3. On the graph below, draw the potential energy diagram for an exothermic reaction and label the
activation energy.
(2 marks)
PE
Ea
4. Nitric oxide (NO) is involved in the decomposition of ozone by the following mechanism:
Step 1: O3 + sunlight → O2 + O
Progress
Step 2: O3 + NO →
NO2 of
+ the
O2 reaction
Step 3: NO2 + O → NO + O2
a) Write the net equation for the decomposition reaction
2O3 + sunlight → 3O2
b) Identify a catalyst
Practice Test#1
Chapter 1 - Kinetics
NO
c) Identify a reaction intermediate
NO2 and O
d) What is the function of sunlight in this reaction? (4 marks)
Provides the activation energy
5. Consider the following reaction:
2NO + 2H2 → 2H2O + N2
a) Explain why the reaction is likely to involve more than one step.
Reactions that have more than three reactant particles likely have mechanisms.
b) A proposed mechanism for the above reaction is: Step 1: NO + H2 → N + H2O
Step 2:
?
Step 3: N2O + H2 → N2 + H2O
Write the equation for step 2.
NO + N → N2O
6. Define the term activation energy.
The minimum energy required for a successful collision
7. The combustion of coal, C, produces carbon dioxide and water according to the following equation:
C(s) + O2(g) → CO2(g) + 394 kJ
a) What is ∆H for this reaction? (1 mark)
∆H + -394 kJ
b) Using the collision theory, explain why a lump of coal does not react with oxygen at room
temperature and pressure. (1 mark)
The Ea is too high for the room temperature collisions to be successful.
c) Many coalmine disasters have resulted when a spark ignites coal dust in the air. Explain using the
collision theory. (2 marks)
The spark provides the Ea, the reaction is exothermic and has a high surface area and an
explosion results.
8. State two reasons why some collisions may not result in a chemical reaction.
(2 marks)
Practice Test#1
Chapter 1 - Kinetics
Not sufficient energy
Poor collision geometry
9. A student wishes to monitor the rate of the following reaction:
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
Identify two different properties that could be used to monitor the rate of the reaction. Describe and
explain the changes that would occur. Any two of the following.
Property 1
Mass of CaCO3
Change and explanation
Decreases as reactants are converted into products
Property 2
Concentration of HCl
Change and explanation
Decreases as reactants are converted into products
Property 3
Concentration of CaCl2
Change and explanation
Increases as reactants are converted into products
Property 4
Volume of CO2 gas
Change and explanation
Increases as reactants are converted into products
Property 5
Mass of open system
Change and explanation
Decreases as gas escapes
Property 6
Pressure of a closed system
Change and explanation
Increases as gas is produced
10.
An experiment is done to determine the rate of the following reaction:
2Al(s) + 6HCl(aq) → 3H2(g) + 2AlCl3(aq)
Time (s)
Mass of Flask + Contents (g)
0.0
30.0
60.0
270.230
270.200
270.170
60.0 s
0.060 g H2
270.170
Practice Test#1
Chapter 1 - Kinetics
Calculate the rate of consumption of Al in mol/min.
0.060 g H2
60.0 s
x
60 s
1 min
x
1mole H2
(3 marks)
x
2.0 g
2 mol Al
3 mol H2
= 0.020 mol Al/min
1.00 g of Al is placed in a beaker
and allowed to react for 12.00 minutes
with 2.00 M HCl. If the rate of consumption
of HCl is 0.250 g/min, calculate the amount
of Al remaining.
12.00 min x 0.250 g HCl x
1 min
1.00 g
- 0.740 g
= 0.26 g
1 mol x 2 mol Al
36.5 g
6 mol HCl
x
27.0 g
1 mole
Note the loss of one sig fig.
=
0.740 g