Kinetics
1.
High kinetic energy
High activation energy
Catalytic effect on the reaction
Large surface area for the reaction
Consider the following reaction: 2H2O2(aq) → 2 H2O(t) + O2(g)
When 1.0 g of KI is added to the H2O2, bubbles of O2 are produced at an
increased rate. When the reaction is complete, the mass of KI is 1.0 g. The KI is a
A.
B.
C.
D.
4.
Zn(s) + S(s) → ZnS(s)
Ba2+(aq) + SO42-(aq) → BaSO4(s)
NH3(g) + HCl(g) → NH4Cl(g)
2 Ag+(aq) + CO32-(aq) → Ag2CO3(s)
Dust particles suspended in the air inside unheated grain elevators can sometimes
react explosively because the dust particles have a:
A.
B.
C.
D.
3.
Factors that Change the Reaction Rate
Which of the following reactions is the slowest at room temperature?
A.
B.
C.
D.
2.
Quiz #2
Product
Catalyst
Reactant
Reaction Intermediate
Consider the following factors:
I.
II.
III.
Concentration of reactants.
Temperature of reactants.
Surface area of reactants.
The factors that affect the rate of a chemical reaction between two gases are
A.
B.
C.
D.
I and II only
I and III only
II and III only.
I, II, and III
5.
Consider the following reactions:
I.
N2(g) + O2(g) → 2NO(g)
II.
2Mg(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.
6.
An untreated sugar cube does not burn when held over a lighted match. A sugar
cube coated with cigarette ash readily ignites and burns. All of the cigarette ash
remains after the reaction. The factor that caused this change in rate is the
A.
B.
C.
D.
7.
9.
Nature of reactants
Presence of a catalyst
Increase in surface area
Increase in concentration
Which combination of factors will affect the rate of the following reaction?
Zn(s) + 2HCl (aq) → ZnCl2(aq) + H2(g)
A.
B.
C.
D.
8.
II only
I and III only
II and III only
I, II and III
Temperature and surfaces only
Temperature and concentration only
Concentration and surface area only
Temperature, concentration, and surface area
To increase the rate of a reaction there must be an increase in
I
II
III
IV
frequency of successful collisions
volume of reaction vessel
pressure of the system
mass of the system
A.
B.
C.
D.
I only
I and III only
I, III and IV only
I, II, III and IV
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.
Adding NaOH
Removing CO2
C.
D.
10.
Which of the following factors affect the rates of both homogeneous and
heterogeneous reactions
I.
Nature of reactants
II.
Presence of a catalyst
III.
Temperature of system
IV
Concentration of reactants
A.
B.
C.
D.
11.
Nature of reactants
Temperature of system
Surface area of reactants
Concentration of reactants
Consider the following reaction: 2S(s) + 302(g) → 2SO3(g) + heat
The rate of this reaction could be increased by
A.
B.
C.
D.
13.
I and IV only
II and III only.
II, III and IV only
I, II, III and IV
Which of the following factors affects the rate of heterogeneous reactions only.
A.
B.
C.
D.
12.
Adding a catalyst
Decreasing the pressure.
Decreasing temperature
Adding a catalyst
Increasing the concentration of S(s)
Increasing the concentration of SO3(g)
6.0 g of Mg reacts with some HCl in two different experiments. The reaction for
both was:
Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
In the first experiment, it took 6.2 minutes for all the Mg to react. In the second
experiment, it took 10.8 minutes for all the Mg to react. Which of the following
could explain the change in rate in the second experiment?
A.
B.
C.
D.
A catalyst was added
The Mg was powdered
The H2 was decreased
The temperature was decreased
14.
15.
Which of the following reactions is most likely to proceed at the greatest rate?
A.
Zn(s)
+
S(s)

ZnS(s)
B.
H2(g)
+
I2(s)

2HI(g)
C.
Cu(s)
+
Cl2(g) 
D.
2KOH +
H2SO4(aq) 
CuCl2(s)
2H2O(l) + K2SO4(aq)
Consider the following reaction:
Mg(s) + 2HCl(aq) 
MgCl2(aq)
+ H2(g)
Which of the following would increase the reaction rate?
A.
B.
C.
D.
16.
an increase in pressure
an increase in temperature
an increase in the concentration of H2
an increase in the concentration of CaCl2
When a candle C20H42 burns, the following reaction occurs:
2C20H42(s) + 61O2(g)  40CO2 + 42H2O(g)
If the rate of production of CO2 is 0.49 g/min, what is the rate of oxygen
consumption?
A.
B.
C.
D.
17.
Which of the following properties could best be monitored in order to determine
the reaction rate of the above burning candle?
A.
B.
C.
D.
18.
0.24 g/min
0.27 g/min
0.36 g/min
0.54 g/min
mass of C20H42
pressure of H2O
surface area of C20H42
concentration of C20H42
Which of the following factors only affects the rate of heterogeneous reactions?
A.
nature of reactants
B.
C.
D.
19.
presence of a catalyst
temperature of reactants
surface area of reactants
Consider the following experimental results:
Experiment 1
Experiment 2
Reactants
Ca(s) + HCl(aq)
Zn(s)
Temperature
20 0C
40 0C
Concentration
1.0 M
2.0 M
Rates
Fast
Slow
+ HCl(aq)
Which factor would account for the faster reaction rate in Experiment 1?
A.
B.
C.
D.
20.
temperature
surface area
nature of reactants
solution concentration
Consider the following reaction:
2NO(g) + O2(g)
 2NO2(g)
How could the rate of this reaction be increased?
A.
B.
C.
D.
21.
Which factor explains why coal dust is explosive?
A.
B.
C.
D.
22.
Reduce the pressure
Increase the volume
Remove some NO2(g)
Increase the temperature
temperature
surface area
concentration
addition of catalyst
Which factor explains why potassium generally reacts faster than magnesium?
A.
surface area
B.
C.
D.
23.
temperature
concentration
nature of reactants
Which factor explains why gasoline vapour is explosive?
A.
B.
C.
D.
temperature
surface area
concentration
nature of the reactant