Quiz 1
Q1 Choose the correct answer:
1) When the system A + B ⇄ C + D is at equilibrium:
a) The sum of the concentrations of A and B must equal the sum of the concentrations of C and
D.
b) The forward reaction has stopped.
c) Both the forward and the reverse reactions have stopped.
d) The
concentrations of the reactants
and
products are not changed
2) Henri
in industry
century,
Châtelier’s
would an
have on
N2(g) +
a) There
ammonia.
b) More
formed.
c) It would
ammonia.
d) The
less.
3)
Le Châtelier studied
equilibrium reactions
in the late 19th
According to Le
principle, what effect
increase in pressure
the yield of ammonia at
equilibrium?
3H2(g) = 2NH3(g)
would be a greater yield of
hydrogen and nitrogen are
have no effect on the yield of
yield of ammonia would be
Consider the following
equilibrium reaction
which one of the following will cause a yellow color to predominate?
a) Addition of sodium hydroxide (NaOH)
b) Addition of hydrochloric acid (HCl)
c) Removal of water
d) Addition of sodium chromate (Na2CrO4)
4) Ammonia is formed in the Haber process according to the following balanced equation
N2 + 3H2 ⇋ 2NH3+ Heat
The table shows the percentages of ammonia present at equilibrium under different
conditions of temperature T and pressure P when hydrogen and nitrogen gases were
mixed in a 3:1 molar ratio.
From the table, what conditions of temperature and
pressure will give the highest yield of ammonia.
a) 100 atm. and 573 K
b) 1000 atm. and 573 K
c) 1000 atm. and 773 K
d) 10 atm. and 573 K
5) The reaction between hydrogen (H2) and nitrogen (N2) is described by the
equation N2 + 3H2 ⇋ 2NH3 + Heat
what will be the effect of increasing the concentration of ammonia
(NH3)? a) The temperature increases
b) More ammonia (NH3) is formed
c) Less nitrogen (N2) is formed
d) More hydrogen (H2) is formed
6) When a
chemical
reaction
has
reached
chemical
equilibrium:
a) The products are forming faster than they are being converted back into reactants. b) The
reactants are forming products while the products are forming reactants by the same rate c)
There are no longer any reactants left.
d) The reactants are no longer reacting.
7) When cobalt (II) chloride is added to water, the following equilibrium is set up , with
the red color predominant.
On adding dilute HCl, the color changes to blue.
Why does this happen?
a) Addition of
chloride ions shifts the equilibrium to the left.
b) More Cl ions were formed.
c) Because water changes the color of the system to blue.
d) The equilibrium shifted to the right.
8) Put these steps in the correct order to describe the creation of a
dynamic equilibrium:
a) T, P, R, S, Q
b) T, P, S, R, Q
c) P, T, S, R, Q
d) P, T, R, S, Q
e) T, P, S, Q, R
9) What does “dynamic” mean
in the term dynamic
equilibrium?
a. The reaction is very
exothermic
b. The forward reaction and the backward reaction are still happening at equal rates.
c. The yield of product per second is very high.
d. The rate of reaction in both directions is very high.
Reaction with dil.H2SO4
10)
(A)(aq) Fe
700oc
(B)(s) (C)(s) Reduction at 4000cCompounds A, B and C respectively represents:
a) FeSO4 , Fe3O4 , FeO
b) FeSO4 , Fe2O3 , FeO
c) Fe2(SO4)3 , Fe2O3 , Fe3O4
d) Fe2(SO4)3 , Fe3O4 , Fe2O3
11) Which of the following statements regarding chemical equilibrium is
false? a) At equilibrium, there is no change in the system apparently.
b) At equilibrium, the concentrations of reactants and products stay the
same c) At equilibrium, the forward and backward reactions cease to occur
d) At equilibrium, the rates of forward and backward reactions are identical
12) In the following reaction:
2SO2(g) + O2(g)⇄2SO3(g) (In closed container)
Which of the following graphs represents the
relation between concentration and time?
Products
Reactants
Reactants
Products
13) What is the representation of a reversible
reaction?
a) single arrow
b) double arrows
c) bar
d) none of above
14) Which of the statements regarding
the effect of reactant or product
concentration changes on equilibrium is false?
a) Adding a reactant always shifts a reversible reaction in the direction of reactants. b)
Removing a reactant always shifts a reversible reaction in the direction of reactants. c)
Adding a product causes a reversible reaction to shift in the direction of the formation of
the reactants.
d) Removing a product shifts a reversible reaction in the direction of formation of products
15) Mixture is heated with Dil. HCl and the lead acetate paper turns black by the evolved
gases, the mixture contains:
a) sulphite
b) sulphide
c) sulphate
d) thiosulphate
16) In the following reaction:
2Na3PO4(aq) + 3BaCl2(aq) Ba3(PO4)2(S)
+6NaCl(aq)
Which of the following graphs represents the
relation between concentration and time?
Products
Reactants
Reactants
Products
17) The reaction of carbon monoxide and iodine pentoxide as represented by the equation
Heat + 5 CO (g) + I2O5 (g) ⇄ I2 (g) + 5 CO2 (g).
Carbon dioxide concentration could be increased by
a) Increasing the pressure.
b) Decreasing the pressure.
c) Increasing the temperature.
d) Decreasing the temperature.
18) The opposite chemical reaction is …………..
2Cu (NO3)2 = 2CUO (s) + 4NO2(g) + O2(g)
a. Complete
b. Incomplete
c. Irreversible
d. Both (a) and (c) are correct
19) The opposite graphical figure represents the
reaction of ammonia preparation from hydrogen and
nitrogen elements:
Number (1) represents:
a) H2
b) NH3
c) N2
20) The opposite graphical figure represents the reaction of ammonia preparation from
hydrogen and nitrogen
elements:
Number (2) represents:
a) H2
b) NH3
c) N2
21) The opposite graphical figure represents the
reaction of ammonia preparation from hydrogen and nitrogen elements:
Does line
(x)
represents
the
equilibrium point:
a) True
b) False
22) In the following reaction:
N2 (g) + O2 (g) ⇄ 2NO (g)
On adding N2, the concentration of O2:
a) Increases
b) Decreases
c) Remains unchanged
23) The reaction of iron with dil. hydrochloric acid is complete because
……………. a) It occurs at high temperature
b) It occurs at high pressure
c) Chlorine gas evolves
d) Hydrogen gas evolves
Mention wither the following statement is true or false:
24) At equilibrium, the concentrations of reactants and products will be
equal a. True
b. False
25) Using phenolphthalein to prove that the reaction between acetic acid and ethyl alcohol
is reversible reaction is Useless
a. True
b. False
Quiz 2
Q1 Choose the correct answer:
1) Element (24X) has electronic configuration:
a. [Ar] 4s2 3d4
b. [Ar] 4s1 3d5
c. [Ar] 4s2 3d6
d. [Ar] 4s1 3d10
2) For the
equation
reaction
2HCl(aq) +
H2O(l) +
a. CaCO3
b. CaCO3
c. CaCO3
d.CaCO3
reaction shown in the
below the fastest
will occur between ...
CaCO3(s) CaCl2(aq) +
CO2(g)
chips and 1M HCl
powder and 1 M HCl
powder and 2 M HCl
chips and 2 M HCl
3)
Increasing
the
concentration increases the speed of reaction by …………. a. Lowering
activation energy
b. Increasing collisions
c. Speeding up the reactants
d. Exposing more products
4) A lump of ignited charcoal which is glowing in air burns more vigorously when lowered
into a bottle of pure oxygen. This is due to an increase in
a. Surface area
b. Temperature
c. Concentration
d. Volume
5) The mass of washing soda crystals before heating is 5 g and after strong heating at A
constant temperature, the mass is 1.853g . What is the% of crystallization of water of
washing soda?
a.15%
b. 62.9%
c. 37%
d. 50%
6) Products will form faster if ………………….
a. the particle size of the reactants are larger
b. Temperature is decreased.
c. Concentration of the reactants are increased.
d. Concentrations of products increases.
7) …………….. can be used in food safety technology which designed to eliminate disease
causing germs from foods.
a. Cobalt
b. Scandium
c. Cobalt 60
d. Zinc
8) The equilibrium constant for the reaction, 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g), is:
a. { 2 [SO2]
+ [O2] } / 2
[SO3]
b. { [SO2]2
x [O2] } /
[SO3]2
c. 2 [SO3] /
{ 2 [SO2] +
[O2] }
d. [SO3]2/ {
[SO2]2 x
[O2] }
9) The
conventional equilibrium constant expression (Kc) for the system below is: 2ICl(s) ⇄ I2(s)
+ Cl2(g)
a. [I2][Cl2]/[ICl]2
b. [I2][Cl2]/2[ICl]
c. [Cl2]
d. [I2][Cl2]
10) Consider the following reversible reaction. In a 3.00 liter container, the following
amounts are found in equilibrium at 400 oC: 0.0420 mole N2, 0.516 mole H2 and 0.0357
mole NH3. Evaluate Kc:0
N2 (g) + 3H2(g) ⇄ 2NH3(g)
a. 0.202
b. 1.99
c. 16.0
d. 4.94
11) The following numbers represents HCl with different concentrations which acid would
react faster with Magnesium?
a. 0.1m
b. 0.4m
c. 1m
d. 2m
12) In the reaction:
2KClO3(s) ⇄ 2KCl(s) + 3O2(g) Kc =27
The concentration of oxygen in this reaction equals …………….
(The reaction takes place in a closed vessel)
b. 20 M
c. 0.002 M
d. 3 M
a. 27 M
13) 2HBr (g) ⇄ H2 (g) + Br2 (v) Kc = 7.7x10-11 at 500k
The predominant direction is …………….. direction.
a. Forward
b.
Backward
14) In the
following
reaction:
SnO2(s) +
2CO (g) ⇄
Sn(s)
+2CO2(g)
Using the
concentrations given in the table below, the value (Kc) for the reaction equals
SnO2
CO
Sn
CO2
0.5 mol/L
0.3 mol/L
Mol/l
0.5 Mol/L
a. 5.5x10-3
b. 2.77x10-3
c. 2.78
d. 5.7
15) You have 4 glass beakers, at each of them 2 cm of magnesium strip reacted with 200
ml of hydrochloric acid under the conditions in each beaker, which beaker has the highest
reaction rate?
a.
Beaker
a
b. Beaker
b
c. Beaker
c
d.Beaker
d
16) The relation that express the equilibrium constant for the reaction between sodium
chloride solution and silver nitratre solution is ……………………… a.
[��������3][��������]
[��������][����������]
b.
[����������]
[��������][����������]
c. [����������][��������]
d. [��������]
[��������]
[��������][����������]
17) In the balanced chemical reaction:PCl5 (g) ⇄ PCl3 (g) + Cl2 (g) ∆ H= (+) The
dissociation of phosphorous pentachloride can increases by …………. a.
Decreasing temperature
b. Decreasing pressure
c. The addition of excess chlorine
d.
Withdrawal of phosphorous
pentachloride
18) 1 mole
in an
and
of N2O4 (g) was placed
empty 1L container
allowed to reach
equilibrium,
to the following
equation:N2O4 (g) ⇄
equilibrium, X mole
had dissociated,
value of the
equilibrium
Kc at the
temperature of the
experiment?
according
2NO2 (g) At
of N2O4 (g)
what is the
constant
a.2��
(1−��) b.
2��
(1−��)2
c. 4��2
(1−��)2 d.
19) The
constant Kc depends on:
a. Temperature
b. Concentrations of product
c. Concentrations of product
d. Pressure
4��2
(1−��)
value of the equilibrium
20) The element which has the electronic configuration [Xe] 4f145d106s1is considered
………………….
a. Paramagnetic in its atomic state
b. Paramagnetic in oxidation state +2
c. Diamagnetic in its atomic state
d. Both (b) and (c) are correct
21) On dissolving each of ………………….. In water, a colored solutions are
formed. a. TiO2, FeCl3
b. FeCl2, CoCl2
c.ZnCl2, NiCl2
d.ScCl3 , ZnSO4
22) the reaction between Silver nitrate and sodium chloride takes time T1 while the
reaction between plant oil and caustic soda takes time T2 then, ………………………
a. T1 = T2
b. T1>T2
c. T2>T1
Q2) Mention wither the following statement is true or false:
1) The value of equilibrium constant decreases to half by increasing the concentration at
the same temperature.
a. True
b. False
2) On
adding
iron, III
chloride
solutions
to
ammonium thiocyanate solution the color of the reaction becomes blood red and on
adding excess of ammonium chloride the intensity of the blood red color decreases
a. True
b. False
3) It is preferable to use nickel block instead of divided nickel in oil
hydrogenation. a. True
b. False
Q1 Choose the correct answer:
Quiz 3
1) Which of the following graphical figures represents the relation between Kc of
exothermic reaction and temperature?
a b c d 2) In the
following reaction the rate of decomposition ……………………………. if we bring a
flask filled with sulphur trioxide and placing it in cooling mixture. SO3 (g) ⇄ SO2 (g)
+ ����O2 (g) ΔH = (-ve)
a) Increases
b) Decreases
c) Does not change
3) The following reaction has two equilibrium constants at two different temperatures.
H2 (g) + I2 (g)⇄2HI(g) KC = 67 at 8500c
H2 (g) + I2 (g) ⇄2HI(g) KC = 50 at 4480c
The previous reaction is ……………………….. as …………………..
a) Endothermic, The value of Kc decreases as the temperature increases
b) Exothermic, The value of Kc decreases as the temperature increases
c) Endothermic, the value of Kc decreases as the temperature decreases
d) Exothermic, the value of Kc decreases as the temperature decreases
4) …………… when burns in hot air , it produces carbon dioxide gas which reacts with
the excess of coke producing carbon monoxide gas which acts as reducing agent for the
iron oxide in …………….. Furnace.
a) Coke , Midrex
b) Coke , Blast
c) Carbon monoxide , blast
d) Carbon monoxide , midrex
5) Which of the following statements regarding the use of catalysts is false?
a) Catalysts lower the activation energy for a reaction
b) Catalysts decreases the proportion of molecules that possess sufficient energy to clear the
activation energy barrier
c) A Catalyst remains unchanged after the chemical reaction
d) A catalyst increases the rate of both the forward & backward reaction equally
6) To get iron oxide which contain the most stable oxidation state of iron :
a) Heating
oxalate in
of air
b) Reaction
ammonium
of the
iron III
ammonium
the product
Reduction
7) On
the
reaction,
iron II
absence
iron II chloride with
hydroxide then heating
product c) Reacting
chloride with
hydroxide then heating
above 2000c d)
of magnetite
heating
following
the
equilibrium constant value ……… N2 (g) + O2 (g) + heat ⇄2NO (g)
a) Increases
b) Decreases
c) Remains constant
8) Which of the following figures represents the reaction rate on a adding a catalyst to a
reversible reaction at the time t1?
a b c d 9) Which of the following graphs represent the relation between Kp of a gaseous
equilibrium reaction and the external; pressure applied to it at constant temperate?
abcd
10) 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.
When the reaction is complete, the mass of KI is 1.0 g The KI is a
a) Product.
b) Catalyst
c) Reactant.
11) Which
activated
graph shows the
relationship between
molecules and
temperature?
a
bcd
12) Which of the following reactions when heated the value of KC increases?
a) N2O4 + 59kj ⇄ 2NO2(g)
b) 2H2(g) + O2(g) ⇄2H2O(l) + 572kj
c) 2BrCl(g) – 29.3kj ⇄ Br2(g) + Cl2(g)
d) C(s) + O2(g) ⇄2CO(g) H = - 394 kj
13) Which of the following would react most rapidly?
a) Powdered Zn in 1.0 M HCl at 25° C
b) Powdered Zn in 2.0 M HCl at 40°
c) A lump of Zn in 2.0 M HCl at 25° C
d) A lump of Zn in 1.0 M HCl at 40° C
14) In the equilibrium reaction:
H2(g) + CO2(g)⇄CO(g) + H2O(v) H = +41kj
What happen on heating the reaction with keeping the container volume constant?
a) [CO] increase and KP value does not change
b) [CO] increase and KP value increases
c) [CO2] increases and KP value decreases
d) [CO2] increases and KP value does not change
15) In the equilibrium reaction:
[N2] can be increased by ………………..
a) Decreasing the amount of N2H4
b) Increasing the amount oh H2
c) Raising the temperature
d) Reducing the pressure
N2H4(g) ⇄ N2(g) + 2H2(g) + Heat
16) The percentage of Fe3O4 in magnetite, knowing that by treating 0.5 g of the ore in a
certain
is
55.8 , O
a) 30%
b) 70%
c) 44.9%
d) 80%
way, 0.362 g of Fe2O3
precipitated. [Fe =
=16]
17)
According
to the
following
diagram,
and C are
…………
a) Fe2O3 ,
b) Fe2O3 , FeO, Fe3O4
c) FeO , Fe3O4 , Fe2O3
d) Fe3O4 , Fe2O3 , FeO
compounds A , B
….. , ……… and
respectively
FeO , Fe2O3
18) According to the following reaction: 2H2O(l) + energy ⇄ H3O+ OH-(aq) On
decreasing the temperature the value of Kc …………….
a) Increases
b) Decreases
c) Remains unchanged
19) The time taken for the reaction to reach equilibrium equals ………
seconds.
a) 1
b) 3
c) 4
d) 6
20) The partial pressure of oxygen gas in this
equilibrium reaction:
N2(g) +
2O2(g) ⇄
2NO2(g)
Kp= 40
Knowing
that the
partial
pressures
of nitrogen
and
nitrogen
dioxide
gases are
0.05 and
0.1 atm.
respectively equals …………
a) 0.4 atm.
b) 0.07 atm.
c) 0.01 atm.
d) 0.104 atm.
21) In the equilibrium reaction: 2H2O (v) ⇄ 2H2 (g) + O2 (g) at 5000c If the partial
pressure of H2, O2 and water vapor are 3.66x10-8, 1.83x10-8 and 25.35 atm. respectively,
the equilibrium constant KP equal
a) 3.815x10-26
b) 0.104
c) 0.056
d) 1.5x10-3
Mention wither the following statement is true or false:
1) Water gas role in the midrex furnace differs from its role in (Fisher-Tropsch) method.
a) True
b) False
2) Collision theory states that all collisions lead to chemical reactions.
a) True
b) False
3) We can distinguish between dil. sulphuric acid and conc. Sulphuric acid using iron and
acidified potassium dichromate solution.
a) True
b) False
4) Milk will go sour in a couple of days when left at room temperature, yet it can reaming
unspoiled for 2 weeks when refrigerated.
a) True
b) False
Quiz 4
1) Q1 Choose the correct answer:
1) The following relationship [OH-]= √����������can be used to
determine the concentration of hydroxide ion for the solution of
……………………. a) NaOH
b) NH3+
c) KOH
d) Mg(OH)2
2) concentration for [H+] ions = concentration of the acid in the case of:
a) H2CO3
b) CH3COOH
c) HNO3
d) HCN
3) Which
of the
following
represents
the
ionization
of HCl:
s
f
100%
n
o
o
r
i
e
d
b
n
u
v
m
a
c
n
u
s
a)
i
o
n
e
l
s
e
t
o
e
f
l
m
r
n
i
a
R
m
a
u
s
n
e
l
e
u
v
c
i
e
t
l
a
l
o
e
m
R
HCl H+ Cl
Before
ionization 100%
l
o
e
d
HCl
e
b
f
n
o
o
r
i
e
d
b
n
m
a
u
s
50%
b) c)
25%
25%
s
n
e
l
e
v
i
u
c
t
e
a
l
l
o
e
R
s
f
o
r
e
b
m
u
n
e
v
i
t
a
l
e
d
R
n
n
o
a
i
m
HCl H+
Cl
s
e
l
100%
100%
u
c
e
l
o
m
HCl H+ Cl
4) Which of the graphical figures does represents the relation between [OH
-
], [H3O+] in aqueous solution at 25oc?
5)
For CH3COOH the
correct graph is:
Ka
Ka
Ka
α
a)
α
Ka
b)
α
c) d)α
6) Electronic configuration of a transition element Z in +3 oxidation state is [Ar] 3d 5,
element Z is used ...............
a) In galvanization of other metals
b) As a catalyst in Haber-Bosch method
c) In dental implants
d) Used in food preserving process
7) A liter of CH3COOH solution, we can increase its electrical conductivity by ………..
a) Dissolving the same mass of the solute in half liter
b) Adding more solute to this liter
c) Dissolving the same mass of the solute in 2 liters
d) Both (b) and (c) are correct
8) On diluting of sulphuric acid solution , the strength of the illumination of the lamb
connected to it ………..
a) Increases
b) Decrease
c) Remains constant
9) Which of the following aqueous solution will be the best conductor of electricity?
(The concentration of all solutions equal 1 molar dissolved in the same amount of
water)
a) NH3
b)
CH3COOH
c) HCl
d) C6H12O6
10)
Ostwald’s
dilution
law is
applicable
on
……………..
a) HCl
b) CH3COOH
c) KOH
d) H2SO4
11) Which one of the elements with the following outer orbital configurations may exhibit
the largest number of oxidations?
a) 3d5 4s1
b) 3d54s2
c) 3d24s2
d) 3d34s2
12) Which of the following elements does not show variable oxidation
state? a) Copper
b) Iron
c) Zinc
d) Titanium
13) Which one of the following the lowest electric conductivity?
a) 1 molar of HCl solution of HCl dissolved in benzene
b) 1 molar of HCl solution dissolved in water
c) 0.001 molar of acetic acid dissolved in water
d) 0.01 molar of acetic acid dissolved in water
14) Which one of the following solutions have the highest electrical
conductivity? a) 1 molar of HCl solution of HCl dissolved in benzene
b) 1 molar of HCl solution dissolved in water
dissolved in water
d) 0.01 molar of acetic acid dissolved in benzene
c) 0.001 molar of acetic acid
15) The [OH-] ion concentration of 0.1 M ammonium hydroxide solution. Knowing that its
ionization constant = 1.8x10-5
a) 2.87 M
b) 1.34 x10-3 M
c) 2.04 x 10-6 M
d) 3.08 x
10-10 M
16) Which
in water?
a) Ti3+
b) V3+
c) Cu3+
d) Sc3+
of the following is colorless
17)
a) Pressure
b) Volume
c) Dilution
d) None of
Ionization depends upon
18) A
acid, its
0.008 (at
solution,
ionization
the same
a) 0.001
b) 0.0098
c) 0.008
d) 0.2
weak monoprotic
degree of ionization =
25oc) in 0.15 M
the degree of
in 0.1 M solution at
temperature?
these
19) Penicillin is used as an antibiotic, it is a weak acid and its degree of ionization = 2x10 -2
in 1 L volume solution which contains 0.25 mole. Of penicillin, the equilibrium constant of
penicillin equals ……………
a) 2x10-4
b) 1x10-2
c) 1x 10-4
d) 3x10-3
20) The hydroxyl ion concentration in 0.2 M solution of methyl amine CH3NH2 (at 25oc),
knowing that its ionization constant = 3.6 x10-4
a) 1.2 x 10-3 M
b) 3.7 x10-4 M
d) 4.5 x10-1M
c) 8.5x10-3 M
21) In the equilibrium process:
CH3COOH (aq) + H2O(l) ⇄ CH3COO-(aq) + H3O+(aq)
Adding drops of HCl …………… the concentration of acetate ion.
a) Increases
b)
Decreases
c)
Does not change
22) The
acetic
a) 1.2
b) 1.34
c) 1.45
d) 1.9 x
23)
ions
of
hydronium ion
concentration in 0.1 M
acid solution (25oc),
knowing that its ionization
percentage = 1.34%
x10-8 M
x10-3 M
x 10-1 M
10-3 M
When excess hydroxide
where added to 1.0 liter
CaCl2 solution, Ca(OH)2
precipitate was formed .
the calcium ions in the
were precipitated in 7.4
of Ca (OH) 2, then what
initial concentration of
CaCl2 solution? (Ca= 40 ,
O=16 , Cl =35.5)
0.05 molar b) 0.10 molar
If all of
solution
grams
was the
the
H=1 ,
a)
c)0.15 molar d) 0.20 molar
Q2. Choose the proper answer for each of the following (True or False): 1) Ostwald
formulated a rule which predicts the effect of different factors on the system
under equilibrium.
a) True
b) False
2) The electric conductivity of hydrofluoric acid increases by dilution
a) True
b) False
Model Answer Quiz 1
1
D
2
A
3
A
4
B
5
D
6
B
7
A
8
B
9
B
10
B
11
C
12
C
13
B
14
A
15
B
16
B
17
C
18
D
19
A
20
B
21
A
22
B
23
D
24
B
25
A
Model Answer Quiz 2
1
B
2
C
3
B
4
C
5
B
6
C
7
C
8
D
9
C
10
B
11
D
12
D
13
B
14
C
15
D
16
B
17
B
18
D
19
A
20
D
21
B
22
C
1
B
2
A
3
B
Model Answer Quiz 3
1
A
2
A
3
C
4
B
5
B
6
C
7
A
8
D
9
C
10
B
11
C
12
A
13
B
14
B
15
D
16
B
17
D
18
B
19
D
20
B
21
A
1
A
2
B
3
A
4
A
Model Answer Quiz 4
1
B
2
C
3
C
4
B
5
B
6
B
7
C
8
C
9
C
10
B
11
B
12
C
13
A
14
B
15
B
16
D
17
C
18
B
19
C
20
C
21
B
22
B
23
B
1
B
2
A