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All Equilibrium Review (13&16) Unit 7

Total questions: 75

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

Equilibrium for 2CrO42- + 2H+→Cr2O72- + H2O. What happens when OH- ions are added to the system?

a)

Position of equilibrium will shift to right

b)

Color of system will turn from orange to yellow

c)

Kc will decrease

d)

OH- ions will not react, and thus no change is seen.

2.

Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?

a)

Divide Kc by 1

b)

Divide 1 by Kc

c)

Square Kc

d)

Take the square root of Kc

3.

This endothermic reaction is at equilibrium.

If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

a)

To products (right)

b)

To reactants (left)

4.
Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
5.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
6.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Stoichiometry
d)
Chemical Reaction
7.

For the reaction...

SO2 + O2 <−> SO3

If the concentration of SO2 is increased, the system will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left nor right

8.

For the reaction...

heat + N2 + O2 ↔ 2NO

If heat is added to the chemical system, the system will shift _______.

a)

left

b)

right

c)

left and right

d)

neither left nor right

9.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Decreasing the volume of container will

a)

shift the system right

b)

shift the system left

c)

change K

d)

have no effect

10.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Using a catalyst will...

a)

shift the system right

b)

shift the system left

c)

increase the rate of reaction

d)

have no effect

11.

At what time (in seconds) is equilibrium established?

a)

0 seconds

b)

1 second

c)

5 seconds

d)

10 seconds

12.
Why is equilibrium called a dynamic state?
a)
Chemists try to convert as much reactants as possible into products.
b)
The reactions at equilibrium continue to take place once equilibrium is established.
c)
The products of a forward reaction are favored, so equilibrium lies to the right.
d)
All chemical reactions are considered to be reversible under suitable conditions.
13.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
14.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
15.

Consider the following reaction:

2SO2(g) + O2(g) <=> 2SO3(g) ΔΗ = - 197 kJ

Which of the following will NOT shift the equilibrium position to the right?

a)

Adding more O2

b)

Adding a catalyst

c)

Decreasing the volume

d)

Lowering the temperature

16.
An equilibrium constant with a large value, e.g. Kc = 1000, indicates…
a)
A very fast reaction
b)
Mostly products at equilibrium
c)
Mostly reactants at equilibrium
d)
Nothing useful at all
17.

When the following reaction reached equilibrium,

SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)

it was found to contain:

0.40 M SO3 , and 0.30 M NO,

0.15 M NO2 , and 0.20 M SO2.

Calculate the equilibrium constant for this reaction.

a)

4.0

b)

0.42

c)

0.25

d)

1.0

18.

Which is true for a system at equilibrium?

a)

Forward reaction rate is faster than the reverse and concentrations are equal

b)

Forward and reverse reaction rates are equal and concentrations are constant

c)

Forward and reverse reaction rates are equal and concentrations are equal

d)

Forward reaction rate is faster than the reverse and concentrations are constant

19.
What is [H2O] if K = 1.2,
[CO2] = 0.846M, & [CH4]= 0.0713M?
4CuO(s)+CH4(g)↔CO2(g)+4Cu(s) +2H2O(g)
a)
0.101 M
b)
0.318 M
c)
0.0102 M
d)
3.77 M
20.

What is the correct equilibrium expression for the following reaction:

2H2O2 (aq) ↔ 2H2O (l) + O2 (g)

a)

[H2O]2[O2] / [H2O2]2

b)

[H2O2]2 / [H2O]2[O2]

c)

[O2] / [H2O2]2

d)

[H2O]2 / [H2O2]2

21.

0.40 M SO2 and 0.60 M O2 are in a flask when the following reaction occurs:

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

At equilibrium, the flask is found to contain 0.30 M SO3. Based on these results, the equilibrium constant, Kc, for the reaction is...

a)

20

b)

10

c)

6.7

d)

2.0

22.

Which of the following systems would NOT be shifted by a change in the volume of the system at constant temperature?

a)

CO (g) + NO (g) ↔ CO2 (g) + ½N2 (g)

b)

N2 (g) + 3H2 (g) ↔ 2NH3 (g)

c)

N2 (g) + 2O2 (g) ↔ 2 NO2 (g)

d)

NO(g) + O3 (g) ↔ NO2 (g) + O2 (g)

23.

H2 (g) +I2 (g) ↔ 2HI (g)

All gases begin with an initial concentration of 2.0 M. When equilibrium is established, the concentration of HI is 4.8 M. What is the value of the equilibrium constant?

a)

1.2

b)

2.4

c)

32

d)

64

24.

H2 (g) + I2 (g) ↔ 2HI (g) and Kc = 54.3

If 0.500 mol H2 and 0.500 mol I2 were placed in a 1.00L flask, what would be the concentration of HI at equilibrium?

a)

0.5M

b)

1.0M

c)

3.68M

d)

0.393M

25.

H2C2O4 + 2 H2O ↔ 2 H3O+ + C2O4 2–


Oxalic acid, H2C2O4, is a diprotic acid with

K1 = 5 x 10–2 and K2 = 5 x 10–5.

What is the equilibrium constant for the reaction represented above?

a)

5 x 10–2

b)

5 x 10–5

c)

2.5 x 10–6

d)

5 x 10–7

26.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
27.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
28.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
29.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
a)
([Fe]3[H2O]4 ) / ([Fe3O4][H2]4)
b)
([Fe3O4][H2]4)/ ([Fe]3[H2O]4)
c)
[H2O]4 / [H2]4
d)
([Fe][H2O]) / ([Fe3O4][H2])
30.

Consider the following equation: CO(g) + 2H2(g) ⇌ CH3OH(g) + Heat

Which of the factors below would decrease the concentration of CH3OH at equilibrium?

a)

adding CO

b)

incresing H2

c)

decrease in the temperature

d)

increasing the temperature

31.
Predict the effect of decreasing the volume of the container on the following reaction: 
2NH3(g) ⇋ N2(g) + 3H2(g) 
a)
shift left
b)
shift right
c)
no change 
d)
all the above
32.
What is the proper Keq for the following reaction? 
   2 NO(g)  +  O2(g) ⇌2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq =  [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
33.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
34.

For reaction a<-- --> b. Use the graph to determine what the Keq will be.

a)

K > 1

b)

K < 1

c)

K = 1

d)

Not enough information

35.

(Calculator Allowed) What is [H2O] if K = 1.2,

[CO2] = 0.846M, & [CH4]= 0.0713M?

4CuO(s)+CH4(g)↔CO2(g)+4Cu(s) +2H2O(g)

a)

0.101 M

b)

0.318 M

c)

0.0102 M

d)

3.77 M

36.

(Calculator Allowed) The solubility of CuI is 2 x 10-6 molar. What the the solubility product constant, Ksp, for CuI?

a)

8 x 10-18

b)

2 x 10-6

c)

4 x 10-12

d)

2 x 10-12

37.
When Keq > 1, 
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
38.
The reaction quotient for a system is 7.2 × 102. If the equilibrium constant for the system is 36, what will happen as equilibrium is approached?
a)
There will be a net gain in product
b)
There will be a net gain in reactant.
c)
There will be a net gain in both product and reactant
d)
There will be no net gain in either product or reactant.
39.

Which one of the following will change the value of an equilibrium constant?

a)

changing temperature

b)

adding other substances that do not react with any of the species involved in the equilibrium

c)

varying the initial concentrations of reactants

d)

varying the initial concentrations of products

e)

changing the volume of the reaction vessel

40.

(Calculator allowed) The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is ksp = 8.3 x 10-17.

a)

3.8 × 10-11

b)

3.0 × 10-10

c)

9.1 × 10-9

d)

3.5 × 10-9

e)

1.4 × 10-8

41.

2 BaO2(s) ⇄ 2 BaO(s) + O2(g)

ΔH°= 162 kJ/molrxn

APMCQ: A sealed rigid vessel contains BaO2(s) in equilibrium with BaO(s) and O2(g) as represented by the equation above. Which of the following changes will increase the amount of BaO2(s) in the vessel?

a)

Removing a small amount of O2(g)

b)

Removing a small amount of BaO(s)

c)

Adding He gas to the vessel

d)

Lowering the temperature

42.

APMCQ: A 0.10 mol sample of each of the four species in the reaction represented above is injected into a rigid, previously evacuated 1.0 L container. Which of the following species will have the highest concentration when the system reaches equilibrium?

a)

H2S(g)

b)

CH4(g)

c)

CS2(g)

d)

H2(g)

43.

2 S(s) + 2 O2(g) ⇄ 2 SO2(g) K1 = 2 x 10105

2 SO2(g) + O2(g) ⇄ 2 SO3(g) K2 = 7 x 1024

APMCQ: Given the value of the equilibrium constants K1 and K2 for the reactions represented above, what is the value of the equilibrium constant, K3, for the following reaction?

2 S(s) + 3 O2(g) ⇄ 2 SO3(g) K3 = ?

a)

1 x 10130

b)

3 x 1080

c)

1 x 1065

d)

2 x 1040

e)

7 x 1024

44.

2 XY(g) ⇄ X2(g) + Y2(g) Kp = 230

A certain gas, XY(g), decomposes as represented by the equation above. A sample of each of the three gases is put in a previously evacuated container. The initial partial pressures of the gases are shown in the table above.


APMCQ: The temperature of the reaction mixture is held constant. In which direction will the reaction proceed?

a)

The reaction will form more products.

b)

The reaction will form more reactant.

c)

The mixture is at equilibrium, so there will be no change.

d)

It cannot be determined unless the volume of the container is known.

45.

2X(g) + Y(g) ⇄ 3Z(g)

APMCQ: The reaction mixture represented above is at equilibrium at 298 K, and the molar concentrations are [X] = 2.0 M, [Y] = 0.5 M, and [Z] = 4.0 M. What is the value of the equilibrium constant for the reaction at 298 K ?

a)

0.5

b)

2

c)

4

d)

16

e)

32

46.

CaCO3(s) ⇄ CaO(s) + CO2(g) ΔH° = 178 kJ/molrxn

APMCQ: The reaction system represented above is at equilibrium. Which of the following will decrease the amount of CaO(s) in the system?

a)

Increasing the volume of the reaction vessel at constant temperature

b)

Lowering the temperature of the system

c)

Removing some CO2(g) at constant temperature

d)

Removing some CaCO3(s) at constant temperature

47.

COCl2(g) ⇄ CO(g) + Cl2(g)

APMCQ: COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previously evacuated flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690 K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K?

a)

0.2

b)

0.05

c)

0.8

d)

1.0

48.

CdF2(s)⇄Cd2+(aq)+2F−(aq)

APMCQ: A saturated aqueous solution of CdF2 is prepared. The equilibrium in the solution is represented above. In the solution, [Cd2+]eq=0.0585 M and [F−]eq=0.117 M. Some 0.90M NaF is added to the saturated solution. Which of the following identifies the molar solubility of CdF2 in pure water and explains the effect that the addition of NaF has on this solubility?

a)

The molar solubility of CdF2 in pure water is 0.0585 M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF2.

b)

The molar solubility of CdF2 in pure water is 0.0585 M, and adding NaF has no effect on the solubility because only changes in temperature can increase or decrease the molar solubility of an ionic solid.

c)

The molar solubility of CdF2 in pure water is 0.117M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF2.

d)

The molar solubility of CdF2 in pure water is 0.176 M, and adding NaF increases this solubility because the Na+ ions displace the Cd2+ ions, causing the equilibrium to shift to favor the products.

49.

APMCQ: For which of the equilibrium systems represented below will the amount of product(s) at equilibrium increase if the volume of the reaction vessel is increased at a constant temperature?

a)

PCl5(g) ⇄ PCl3(g) + Cl2(g)

b)

2 NO(g) + O2(g) ⇄ 2 NO2(g)

c)

N2(g) + O2(g) ⇄ 2 NO(g)

d)

2 CO(g) ⇄ C(s) + CO2(g)

50.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
51.
2SO2(g)+O2(g)⇌2SO3(g)
Using a catalyst
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase rate of reaction
d)
have no change
52.

2SO2(g)+O2(g)⇌2SO3(g)

Decreasing the volume of container will

a)

shift equilibrium right

b)

shift equilibrium left

c)

change K

d)

have no change

53.
Equilibrium for 2CrO42- + 2H+→Cr2O72- + H2O. What happen when OH- ions are added to the system?
a)
Position of equilibrium will shift to right
b)
Color of system will turn from orange to yellow
c)
Kc will decrease
d)
OH- ions will not react, and thus no change is seen.
54.
Which of the following shows the correct dissolution reaction for BaCl2?
a)
Ba 2+(aq) + Cl2-(aq) -> BaCl2(s)
b)
BaCl2(aq) -> Ba 2+(aq) + 2Cl-(aq)
c)
 BaCl2(s) -> Ba 2+(aq) + 2Cl-(aq)
d)
Ba 2+(aq) + 2Cl-(aq) -> BaCl2(s)
55.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
56.
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
a)
3.51 x 10-9
b)
1.40 x 10-8
c)
4.62 x 10-6
d)
1.52 x 10-3
57.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
58.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
59.
The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:
a)
2s2 = Ksp
b)
2s3 = Ksp
c)
4s3 = Ksp
d)
8s3 = Ksp
60.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
61.

The solubility of CuI is 2 x 10-6 molar. What is the solubility product constant, Ksp, for CuI?

a)

4 x 10-12

b)

2 x 10-12

c)

1.4 x 10-3

d)

2 x 10-6

62.

The Ksp expression for the solubility of silver chromate, Ag2CrO4, is

a)

Ksp = [Ag+]2[CrO42-]

b)

Ksp = [Ag+][CrO42-]

c)

Ksp = [Ag+][CrO42-]2

d)

Ksp = [Ag+]2[CrO42-]4

63.

Three saturated solutions (X, Y, and Z) are prepared at 25oC. Based on the information in the table, which of the following lists the solutions in order of increasing [M+] ?

a)

B < C < A

b)

A < C < B

c)

C < A < B

d)

B < A < C

64.

Calculate the molar solubility of AgCl in a 0.10 M solution of NaCl. Ksp of AgCl is 1.8 x 10-10

a)

1.3 x 10-5 M

b)

5.5 x 10-1 M

c)

4.2 x 10-5 M

d)

1.8 x 10-9 M

65.

Based on the Ksp values in the table above, a saturated solution of which of the following compounds has the lowest [Cl–] ?

a)

PbCl2

b)

CuCl

c)

AgCl

d)

NaCl

66.

Solutions of lead(II) nitrate and potassium iodide react according to the following equation:


Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)


A molecular-level representation illustrating solutions of the reactants lead(II) nitrate and potassium iodide is shown in the image. Which of the following would be the best molecular-level representation after the reaction has taken place?

a)

a

b)

b

c)

c

d)

d

67.

Solutions of lead(II) nitrate and potassium iodide react according to the following equation:


Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)


Which species act as spectator ions in this reaction?

a)

K+, NO3-

b)

Pb2+, I-

c)

K+, Pb2+

d)

I-, NO3-

68.

Pb2+(aq) + 2Cl-(aq) → PbCl2(s)


A chemist mixes a dilute solution of lead(II) perchlorate with an excess of potassium chloride to precipitate lead(II) chloride (Ksp = 1.7 x 10-5). The net ionic equation is given above for the reaction.


Which of the following particulate views represents the experiment after the reactants are mixed thoroughly and the solids are given time to precipitate?

a)

(A)

b)

(B)

c)

(C)

d)

(D)

69.

Consider the following solubility data for various chromates at 25oC.

Ag2CrO4, Ksp = 9.0 x 10-12

BaCrO4, Ksp = 2.0 x 10-10

PbCrO4, Ksp = 1.8 x 10-14

The chromate that is the most soluble in water at 25oC on a molar basis is:

a)

Ag2CrO4

b)

BaCrO4

c)

PbCrO4

d)

impossible to determine

70.

The molar solubility of PbBr2 is 2.17 x 10-3 M at a certain temperature. Calculate Ksp for PbBr2.

a)

6.2 x 10-6

b)

6.4 x 10-7

c)

4.1 x 10-8

d)

3.4 x 10-6

71.

What is the molar solubility, s, of Ba3(PO4)2 in terms of Ksp?

a)

s = Ksp1/2

b)

s = Ksp1/5

c)

s = [Ksp/27]1/5

d)

s = [Ksp/108]1/5

72.

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if Qsp _____ Ksp, and will continue to precipitate until Qsp _____ Ksp.

a)

is greater than; equals

b)

is less than; is greater than

c)

is less than; equals

d)

equals; is less than

73.

A swimming pool was sufficiently alkaline so that CO2 absorbed from the air produced in the pool a solution which was 2 x 10-4 M in CO32- M. If the pool water was originally 4 x 10-3 M in Mg2+, 6 x 10-4 M in Ca2+ and 8 x 10-7 M in Fe2+, then a precipitate should form of:

a)

only MgCO3

b)

only CaCO3

c)

only FeCO3

d)

only CaCO3 and FeCO3

74.

Which solid will precipitate first if an aqueous solution of Na2CrO4 at 25oC is slowly added to an aqueous solution containing 0.001 M Pb(NO3)2 and 0.100 M Ba(NO3)2 at 25oC?

a)

BaCrO4(s)

b)

NaNO3(s)

c)

PbCrO4(s)

d)

Pb(NO3)2(s)

75.

A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly until the solid AgCl just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 x 10-10 and for AuCl = 2.0 x 10-13.

a)

2.0 x 10-10 M

b)

1.1 x 10-6 M

c)

4.5 x 10-7 M

d)

1.8 x 10-7 M

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