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EQUILIBRIUM CONSTANT, Kp and Ksp

Total questions: 25

Worksheet time: 6hrs 15mins

Name
Class
Date
1.

Calculate the equilibrium constant (Kc) for the given reaction and tell whether equilibrium lies to the left or the right.

PCl5 (g) ↔ PCl3 (g) + Cl2 (g)

Equilibrium concentrations are: [PCl5] = 0.25 M, [PCl3] = 9.7 × 10-4 M, and [Cl2] = 3.2 × 10-3 M.

a)

1.02 lies to the left

b)

0.000012 lies to the left

c)

1.02 lies to the right

d)

0.000012416 lies to the left

2.
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]
3.

When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc, for the reaction is

a)

20

b)

10

c)

6.7

d)

2.0

4.

H2(g)+Cl2(g)⇌2HCl(g)

The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

5.

What is the equilibrium expression for: Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g) Kc =

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]
6.

For the reaction... N2 (g) +  3 H2 (g) ⇌ 2 NH3 (g) If the pressure in the system is increased,  which substance(s) will increase in concentration?

a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
7.

For the reaction...

N2 (g) + 3 H2(g) ⇌ 2 NH3 (g)


If the pressure in the system is increased, which substance(s) will increase in concentration?

a)

N2

b)

H2

c)

N2 and H2

d)

NH3

8.
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.
9.

For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.

a)

6.2 x 10-10 M

b)

2.5 x 10-5 M

c)

1.1 M

d)

1.2 M

10.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
11.
Which equation represents Dalton's Law?
a)
e=mc2
b)
PV=nRT
c)
P1/T1=P2/T2
d)
Ptotal=P1, P2, P3...
12.
Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
13.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
14.

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

a)

200 mmHg

b)

80 mmHg

c)

40 mmHg

d)

120 mmHg

15.

Mole fractions always have a value between:

a)

0 and 1

b)

0 and 100

16.

When pressure is measure in Pascals, Pa, what would be the units of the equilibrium constant, Kp, for the reaction shown?

a)

Pa2

b)

Pa-1

c)

No units

d)

Pa-2

17.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
18.

What is the equilibrium expression for the following reaction?

N2O4(g)⟺ 2NO2(g)N_2O_{4\left(g\right)}\Longleftrightarrow\ 2NO_{2\left(g\right)}  

a)

Kp=PN2O4PNO2      2K_p=\frac{P_{N_2O_4}}{P_{NO_2}^{\ \ \ \ \ \ 2}}^{ }  

b)

Kp=PN2O42PNO2K_p=\frac{P_{N_2O_4}}{2P_{NO_2}}  

c)

Kp=2PNO2PN2O4K_p=\frac{2P_{NO_2}}{P_{N_2O_4}}  

d)

Kp=PNO2      2PN2O4K_p=\frac{P_{NO_2}^{\ \ \ \ \ \ 2}}{P_{N_2O_4}}  

19.

In the following ICE box, what number should go where the star is?

a)

+0.20

b)

+0.10

c)

-0.20

d)

-0.10

20.

In the following ICE box, what numbers should go where the stars are?

a)

-0.4 and -0.4

b)

+0.4 and +0.4

c)

-0.8 and -1.2

d)

+0.8 and +1.2

21.

a)

A

b)

B

c)

C

d)

D

22.

a)

A

b)

B

c)

C

d)

D

23.
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
24.
a)

A

b)

B

c)

C

d)

D

25.
a)

a

b)

b

c)

c

d)

d

e)

e

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