Free Printable Honors Chem Ch 13

1.

What does it mean to describe a reaction as "reversible"?

a)

The reaction can proceed in both the forward and reverse directions

b)

The reaction can only proceed in the forward direction

c)

The reaction can only proceed in the reverse direction

d)

The reaction is stuck, it won't proceed in either direction

2.

When writing a reaction, how is a reversible reaction distinguished from a nonreversible reaction?

By the (a) used in the reaction.

(b) is for reversible equilibria reactions

(c) is for one way, completion reactions

Choose from the below words

arrow

→

molecules

+ or - signs

+

-

Molarity

Molar Mass

coefficients

⇌

3.

If a reaction is reversible, when can it be said to have reached equilibrium?

a)

The system reaches equilibrium when the rate of the forward reaction equals the rate of the reverse reaction.

b)

The system reaches equilibrium when the concentrations of all species are equal to each other.

c)

The system reactions equilibrium when the masses of all species equal the initial molarity of each species.

d)

The system reaches equilibrium when the rate of the forward reaction is twice as fast as the rate of the reverse reaction

4.

If the concentration of products and reactants are equal, is the system at equilibrium?

a)

Not necessarily, in fact, most likely not.

b)

Yes, by definition this is what equilibrium means.

c)

Most of the time yes, but there are a few exceptions.

5.

Write the equilibrium expression, Kc, for the following reaction:

NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH^-(aq)

Kc = (a) / (b)

Choose from the below words

[NH4+][OH-]

[NH3]

[NH4+]

[NH3][H2O]

[OH-]

[H2O]

[NH4+][NH3]

[H2O][OH-]

1

6.

Write the equilibrium expression, Kc, for the following reaction:

Cl₂(g) + 2 I^-(aq) ⇌ 2 Cl^-(aq) + I₂(s)

Kc = (a) / (b)

Choose from the below words

[Cl-]^2

[Cl2][ I-]^2

[Cl-]

[Cl2][ I-]

[Cl-][I2]

[Cl-]^2[I2]

[I2]

[Cl2]

1

7.

Write the equilibrium expression, Kc, for the following reaction:

2 Cs(s) + 2 H₂O(l) ⇌ 2 Cs⁺(aq) + 2 OH^-(aq) + H₂(g)

Kc = (a) / (b)

Choose from the below words

[Cs+]^2 [OH-]^2 [H2]

[Cs+][OH-][H2]

1

[Cs][H2O]

[Cs]^2[H2O]^2

[Cs+]^2[OH-]^2

[Cs+][OH-]

8.

Write the equilibrium expression, Kc, for the following reaction:

CaO(s) + CO₂(g) ⇌ CaCO₃(s)

Kc = (a) / (b)

Choose from the below words

1

[CO2]

[CO2][CaO]

[CaCO3]

9.

The equilibrium concentrations for the reaction below were found to be:
[AgNO₃] = 0.070M, and [Cu(NO₃)₂] = 0.48M at a certain temperature.
2 AgNO₃(aq) + Cu(s) ⇌ Cu(NO₃)₂(aq) + 2 Ag(s)
Find the equilibrium constant, Kc, for the reaction.

a)

97.96

b)

6.857

c)

0.1458

d)

0.3038

10.

The equilibrium pressures for the reaction below are:
P(CO) = 0.0598 atm
P(CO2) = 0.159 atm
CO₂(g) + C(graphite) ⇌ 2 CO(g)
Find the equilibrium constant, Kp, for the reaction.
(Carbon's state of matter is usually written as either graphite or diamond, both of which are solid.)

a)

0.0225

b)

0.376

c)

2.37

d)

2.66

e)

44.5

11.

At 100^oC, K_c = 0.078 for the reaction below.

SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g)

In an equilibrium mixture of the three Gases, the concentrations of SO₂Cl₂ and SO₂ are 0.108 M and 0.052 M respectively. What is the concentration of Cl₂ in the equilibrium mixture?

a)

0.162 M

b)

0.0376 M

c)

0.172 M

d)

6.17 M

e)

13.9 M

12.

At 900 K, the following reaction has a Kc = 0.345.

2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

What is the equilibrium expression?

(a) = (b) / (c)

In an equilibrium mixture, the concentration of SO2 is 0.135 M and O2 is 0.455 M. What is the equilibrium concentration of SO₃ in the mixture?

[SO₃] = (d)

Choose from the below words

Kc

[SO3]^2

[SO2]^2[O2)]

[SO3]

[SO2][O2]

0.00286 M

0.0212 M

0.146 M

0.0535 M

1

13.

Write the equilibrium expression for the following reaction:

Cu2+(aq) + Zn(s) ⇌ Cu(s) + Zn2+(aq)

(a) = (b) / (c)

Choose from the below words

Kc

[Zn2+]

[Cu2+]

[Zn]

[Cu]

[Cu][Zn2+]

[Cu2+][Zn]

1

14.

Equilibrium expressions never include molecules in the (a) phases.

Equilibrium expressions only include molecules in the (b) phases.

Choose from the below words

solid and liquid

gas and aqueous

solid and gas

solid and aqueous

liquid and gas

liquid and aqueous

15.

Write the equilibrium expression for the following reaction:

MgCl2(s) + H2O(l) ⇌ MgO(s) + 2 HCl(g)

(a) = (b) / (c)

Choose from the below words

Kc

[HCl]^2

1

[HCl]

[HCl]^2[MgO]

[MgO]

[MgCl2]

[MgCl2][H2O]

[H2O]

16.

If K > 1, there are more (a) at equilibrium.

If K < 1, there are more (b) at equilibrium

Choose from the below words

products

reactants

gases

liquids

solids

moles

grams

17.

If K > 1, the reaction is a (a) reaction because products are in the (b) of the equilibrium expression.

If K < 1, the reaction is a (c) reaction because the reactants are in the (d) of the equilibrium expression.

Choose from the below words

product favored

reactant favored

fast moving

slow moving

single replacement

double replacement

numerator

denominator

left side

right side

18.

K_sp is the solubility product constant for ionic compounds dissociating in water.

Write the dissociation reaction for Pb(NO₃)₂(s)

(a) ⇌ (b) + (c)

Write the equilibrium expression for Pb(NO₃)₂(s)

Ksp = (d)

Choose from the below words

Pb(NO3)2(s)

Pb2+

2 NO3-

NO3-

Pb

[Pb2+][NO3-]^2

[Pb2+][NO3-]

[Pb2+]

[NO3-]

[Pb2+][NO3-]^2 / [Pb(NO3)2]

19.

K_sp is the solubility product constant for ionic compounds dissociating in water.

Write the dissociation reaction for AgCl(s)

(a) ⇌ (b) + (c)

Write the equilibrium expression for AgCl(s)

Ksp = (d)

Choose from the below words

AgCl(s)

Ag+

Cl-

[Ag+][Cl-]

[Ag][Cl-]^2

[Ag+][Cl-] / [AgCl]

[Ag][Cl]

20.

NiS(s) dissolves according to this reaction:

NiS(s) ⇌ Ni²⁺ + S^2- Ksp = 3.0 x 10^-21

What is the [Ni2+] in a saturated solution of NiS(s)?

a)

5.48 x 10^-11M

b)

3.0 x 10^-11M

c)

3.0 x 10^-21M

d)

1.5 x 10^-21M

21.

CaS(s) dissolves according to this reaction:

CaS(s) ⇌ Ca²⁺ + S^2- Ksp = ?
The [Ca²⁺] is 2.83 x 10^-3 M in a saturated solution of CaS(s). What is the Ksp of CaS?

a)

8.01 x 10^-6

b)

0.00283

c)

8.01

d)

5.66 x 10^-3

22.

What happens to the equilibrium if we add methane (CH₄)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

23.

What happens to the equilibrium if we remove heat?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

24.

What happens to the equilibrium if we add hydrogen (H₂)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

25.

What happens when the pressure is decreased?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

26.

What happens when sodium ions (Na⁺) are added?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

27.

What happens when fluoride ions (F^-) are removed?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

28.

What happens when the system is cooled (heat is removed)?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

29.

What happens when sodium fluoride (NaF) is added?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

30.

What happens when sulfur dioxide (SO₂) is added?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

The reaction does not shift

31.

What happens when oxygen (O₂) is removed?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

The reaction does not shift

32.

What happens when pressure is increased?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

The reaction does not shift

33.

The Kp for the equilibrium reaction given below is 4.38 x 10^-5 at 450°C.

N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Calculate Q for the following mixture. If it is not at equilibrium, indicate the direction in which the mixture must shift to achieve equilibrium.

98 atm NH₃, 45 atm N₂, 55 atm H₂

Is the reaction at equilibrium? (a)

If not at equilibrium, in which direction will the reaction shift to reach equilibrium? (b) because (c)

Choose from the below words

no, not at equilibrium

reaction will shift left

K < Q

K > Q

K = Q

reaction will shift right

yes, the reaction is at equilibrium

reaction won't shift

34.

The Kp for the equilibrium reaction given below is 4.38 x 10^-5 at 450°C.

N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Calculate Q for the following mixture. If it is not at equilibrium, indicate the direction in which the mixture must shift to achieve equilibrium.

57 atm NH₃, 143 atm N₂, 197 atm H₂

Is the reaction at equilibrium? (a)

If not at equilibrium, in which direction will the reaction shift to reach equilibrium? (b) because (c)

Choose from the below words

no, not at equilibrium

reaction will shift left

K > Q

K < Q

K = Q

reaction will shift right

yes, the reaction is at equilibrium

reaction won't shift

35.

The Kp for the equilibrium reaction given below is 4.38 x 10^-5 at 450°C.

N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Calculate Q for the following mixture. If it is not at equilibrium, indicate the direction in which the mixture must shift to achieve equilibrium.

13 atm NH₃, 17 atm N₂, 61 atm H₂

Is the reaction at equilibrium? (a)

If not at equilibrium, in which direction will the reaction shift to reach equilibrium? (b) because (c)

Choose from the below words

reaction will shift left

K > Q

K < Q

K = Q

reaction will shift right

reaction won't shift

yes, the reaction is at equilibrium

36.

What is the value of the equilibrium constant at 500⁰C for the formation of NH₃ according to the following equation if at equilibrium, the following concentrations were found?
1.35M H₂
1.15M N₂
0.413 M NH₃
N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

a)

K_c = 0.0603

b)

K_c = 0.365

c)

K_c = 0.0797

d)

K_c = 0.193

e)

K_c = 0.146

37.

A 0.72 mol sample of PCl5 is initially put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl₃(g) and 0.40 mol of Cl₂(g).

PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

Calculate the value of the equilibrium constant, Kc.

a)

0.2

b)

0.3

c)

0.4

d)

0.5

e)

0.6

38.

Calculate the value of the equilibrium constant K_p for the reaction below from these equilibrium pressures: NO=0.050 atm; Cl₂=0.30 atm; NOCl=1.2 atm
2 NO(g) + Cl₂(g) ⇌ 2 NOCl(g)

a)

1920

b)

172.8

c)

0.12

d)

1600

e)

80

39.

Analysis of the gases in a sealed vessel containing NH₃, N₂, and H₂ at equilibrium at 400⁰C established the concentrations of N₂ to be 1.2 M and H₂ 0.24 M. Calculate the equilibrium molar concentration of NH₃. N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) K_c = 0.50 at 400₀C

a)

0.144

b)

0.00829

c)

0.0911

d)

0.612

e)

0.0132

40.

Barium sulfate dissociates in water according to the following reaction:

BaSO₄(s) ⇌ Ba²⁺(aq) + SO₄^2-(aq) Ksp = 1.1 x 10^-11

Which expression would solve for the molar solubility of BaSO₄?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{1.1x10^{-11}}=x$

b)

1.1 x 10^-11= x

c)

$\sqrt[3]{1.1x10^{-11}}=x$

d)

$\sqrt[3]{\frac{1.1x10^{-11}}{4}}=x$

e)

$\sqrt[]{5.5x10^{-12}}=x$

41.

Barium carbonate dissociates in water according to the following reaction:

BaCO₃(s) ⇌ Ba²⁺(aq) + CO₃^2-(aq) Ksp = 5.0 x 10^-9

Which expression would solve for the molar solubility of BaCO₃?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{5.0x10^{-9}}=x$

b)

5.0 x 10^-9= x

c)

$\sqrt[3]{5.0x10^{-9}}=x$

d)

$\sqrt[3]{\frac{5.0x10^{-9}}{4}}=x$

e)

$\sqrt[]{2.5x10^{-9}}=x$

42.

Iron(II) carbonate dissociates in water according to the following reaction:

FeCO₃(s) ⇌ Fe²⁺(aq) + CO₃^2-(aq) Ksp = 2.1 x 10^-11

Which expression would solve for the molar solubility of FeCO₃?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{2.1x10^{-11}}=x$

b)

2.1 x 10^-11= x

c)

$\sqrt[3]{2.1x10^{-11}}=x$

d)

$\sqrt[3]{\frac{2.1x10^{-11}}{4}}=x$

e)

$\sqrt[]{1.05x10^{-11}}=x$

43.

Nickel(II) sulfide dissociates in water according to the following reaction:

NiS(s) ⇌ Ni²⁺(aq) + S^2-(aq) Ksp = 3 x 10^-20

Which expression would solve for the molar solubility of NiS?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{3x10^{-20}}=x$

b)

3 x 10^-20= x

c)

$\sqrt[3]{3x10^{-20}}=x$

d)

$\sqrt[3]{\frac{3x10^{-20}}{4}}=x$

e)

$\sqrt[]{1.5x10^{-20}}=x$

44.

Barium fluoride dissociates in water according to the following reaction:

BaF₂(s) ⇌ Ba²⁺(aq) + 2 F^-(aq) Ksp = 1.7 x 10^-6

Which expression would solve for the molar solubility of BaF₂?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{1.7x10^{-6}}=x$

b)

1.7 x 10^-6= x

c)

$\sqrt[3]{1.7x10^{-6}}=x$

d)

$\sqrt[3]{\frac{1.7x10^{-6}}{4}}=x$

e)

$\sqrt[]{8.5x10^{-7}}=x$

45.

Magnesium hydroxide dissociates in water according to the following reaction:

Mg(OH)₂(s) ⇌ Mg²⁺(aq) + 2 OH^-(aq) Ksp = 1.8 x 10^-11

Which expression would solve for the molar solubility of Mg(OH)₂?

(Molar solubility is "x" in the Ksp equation)

a)

$\sqrt[]{1.8x10^{-\ 11}}=x$

b)

1.8 x 10^-11= x

c)

$\sqrt[3]{1.8x10^{-11}}=x$

d)

$\sqrt[3]{\frac{1.8x10^{-11}}{4}}=x$

e)

$\sqrt[]{9.0x10^{-12}}=x$

46.

Cadmium(II) carbonate dissociates in water according to the following reaction:

CdCO₃(s) ⇌ Cd²⁺(aq) + CO₃^2-(aq) Ksp = ?

The molar solubility of CdCO3 is 1.34 x 10^-7 M.

How do you solve for the Ksp?

a)

Ksp = x²

x = 1.34 x 10^-7

b)

Ksp = x³

x = 1.34 x 10^-7

c)

Ksp = 4x³

x = 1.34 x 10^-7

d)

$\sqrt[3]{\frac{x}{4}}=Ksp$

x = 1.34 x 10^-7

e)

$\sqrt[]{x}=Ksp$

x = 1.34 x 10^-7

47.

Calcium sulfate dissociates in water according to the following reaction:

CaSO₄(s) ⇌ Ca²⁺(aq) + SO₄^2-(aq) Ksp = ?

The molar solubility of CaSO₄is 0.0049 M.

How do you solve for the Ksp?

a)

Ksp = x²

x = 0.0049

b)

Ksp = x³

x = 0.0049

c)

Ksp = 4x³

x = 0.0049

d)

$\sqrt[3]{\frac{x}{4}}=Ksp$

x = 0.0049

e)

$\sqrt[]{x}=Ksp$

x = 0.0049

48.

Silver(I) carbonate dissociates in water according to the following reaction:

Ag₂CO₃(s) ⇌ 2 Ag⁺(aq) + CO₃^2-(aq) Ksp = ?

The molar solubility of Ag₂CO₃is 1.27 x 10^-4 M.

How do you solve for the Ksp?

a)

Ksp = x²

x = 1.27 x 10^-4

b)

Ksp = x³

x = 1.27 x 10^-4

c)

Ksp = 4x³

x = 1.27 x 10^-4

d)

$\sqrt[3]{\frac{x}{4}}=Ksp$

x = 1.27 x 10^-4

e)

$\sqrt[]{x}=Ksp$

x = 1.27 x 10^-4

Honors Chem Ch 13

Total questions: 48

Worksheet time: 40mins

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