Free Printable Chapter 18 Review

1.

Label the voltaic cell correctly.

a)

Flow of positive ions

b)

Flow of negative ions

c)

Flow of electrons

d)

anode

e)

cathode

f)

M²⁺_^(aq) converting into M_(s)

g)

M_(s) converting into M²⁺_(aq)

1

2

3

4

5

6

7

1)

2)

3)

4)

5)

6)

7)

2.

Figure shows a chemical cell. What is the energy conversion that occurs in the cell?

a)

Chemical energy to electrical energy

b)

Kinetic energy to potential energy

c)

Mechanical energy to heat energy

d)

Electrical energy to chemical energy

3.

Reactions in voltaic (galvanic) cells are.... (2 answers)

a)

spontaneous reactions

b)

non-spontaneous reactions

c)

redox reactions

d)

non-redox reactions

4.

Oxidation happens at the

a)

anode

b)

cathode

c)

salt bridge

d)

voltmeter

5.

Reduction happens at the

a)

anode

b)

cathode

c)

salt bridge

d)

voltmeter

6.

What is the function of Y in cell below?

a)

To complete the circuit

b)

To allow flow of electrons between both cells

c)

To allow flow of ions for charge neutrality

d)

To connect both half cells

7.

The diagram shows the set-up of the apparatus of a chemical cell. Magnesium is converted from Mg_(s) to Mg²⁺_(aq). Which of the following observations will you make?

a)

The magnesium rod becomes thicker

b)

The iron rod becomes thinner

c)

Electrons flow from iron to magnesium

d)

the green colour of iron(II) sulphate becomes paler (lighter)

8.

In which direction does electricity flow in a voltaic cell (battery)?

a)

Electrons flow from the cathode to the anode

b)

Electrons flow from left to right

c)

Electrons flow from anode to cathode

d)

Electrons flow from right to left

9.

What reaction occurs at the anode?

a)

Ag⁺ + e^- →Ag

b)

Ag → Ag⁺ + e^-

c)

Ni²⁺ + 2e^- → Ni

d)

Ni → Ni²⁺ + 2e^-

10.

What reaction occurs at the anode?

a)

Ag⁺ + e^- →Ag

b)

Ag → Ag⁺ + e^-

c)

Ni²⁺ + 2e^- → Ni

d)

Ni → Ni²⁺ + 2e^-

11.

In a Galvanic Cell, the salt bridge...

a)

completes the circuit so that electrons can flow through the wire

b)

maintains charge balance

c)

is soaked in an unreactive electrolyte such as KNO₃

d)

all of the above

12.

What unit of measurement do we use to measure electrical potential?

a)

Watts

b)

Amps

c)

Volts

d)

Ohms

13.

Which way do electrons flow in a galvanic cell? (2 answers)

a)

Cathode to anode

b)

Positive to negative terminal

c)

Anode to cathode

d)

Negative to positive terminal

14.

Match the following keywords and definitions:

a)

A species that accepts electrons from another species, undergoing reduction itself.

1.

Oxidizing Agent

b)

The potential difference between a standard hydrogen electrode (SHE) and another half-reaction

2.

Standard Electrode Potential (E°)

c)

The voltage measured under standard conditions for a galvanic cell. E°cell is the difference between the standard electrode potentials of the two half-reactions (cathode - anode). A positive value indicates a spontaneous reaction.

3.

Standard Cell Potential (E°_cell)

d)

Allows for ionic flow to maintain charge neutrality within the cell while minimizing mixing of solutions.

4.

Salt Bridge

e)

Where oxidation occurs (electrons are lost).

5.

Anode

15.

Under specific conditions, the cell potential E can be considered a standard cell potential E°.
What are these conditions?

a)

Pressure of 1atm for gases

b)

1 mol of all species

c)

1M aqueous for all solutions

d)

298K

e)

KNO₃ must be used for the salt bridge

16.

In a Galvanic Cell, the anode is...

a)

positive

b)

negative

17.

In a Galvanic Cell, the cathode is...

a)

positive

b)

negative

18.

Which of the following diagrams depicts the equilibrium that exists between a piece of zinc metal in contact with an aqueous solution of zinc ions?

a)

b)

c)

d)

19.

E_cell =

a)

E_red - E_ox

b)

E_red + E_ox

c)

E_ox - E_red

d)

E_ox + E_red

20.

E° for a half reaction will change when you multiply the half-reaction by an integer.

a)

True

b)

False

c)

Sometimes

21.

Calculate E°cell for a Cadmium (Cd) - Zinc (Zn) cell.

a)

1.16 V

b)

-1.16 V

c)

0.36 V

d)

-0.36 V

22.

Calculate E°cell for the following for a Cadmium (Cd) - Copper (Cu) cell.

a)

0.74 V

b)

-0.74 V

c)

-0.06 V

d)

0.06

23.

In a redox reaction, the reducing agent... (choose two options)

a)

is oxidised

b)

is reduced

c)

increases its oxidation number

d)

decreases its oxidation number

24.

In a Galvanic cell, the cations in the salt bridge...

a)

flow the same way as the electrons flow in the wire

b)

flow the opposite way to the electron flow in the wire

c)

stay in the salt bridge

25.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the anode?

a)

HgO + 2 e- → Hg + O^2-

b)

Zn²⁺ + 2 e- → Zn

c)

Zn → Zn²⁺ + 2 e-

d)

ZnO + 2 e- → Zn

26.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the cathode?

a)

HgO + 2 e- → Hg + O^2-

b)

Hg → Hg²⁺ + 2 e-

c)

Zn → Zn²⁺ + 2 e-

d)

ZnO + 2 e- → Zn

27.

What is oxidation number of Cr in Cr₂O_7^2-?

a)

-2

b)

+2

c)

+6

d)

+12

28.

If you want to make a galvanic cell with bromine and zinc, which process will occur at the cathode?

a)

Zn²⁺ forms Zn

b)

Zn forms Zn²⁺

c)

Br₂ forms Br^-

d)

Br^- forms Br₂

29.

Voltaic cells are the same as which other cells?

a)

Galvanic

b)

Electrolyte

c)

Electron

d)

Electrolytic

30.

Choose the correct symbols for each of the uses in 'line notation' describing voltaic cells.

a)

when separating phases (phase boundary)

1.

use a line ' | '

b)

when none of the species in a half cell are solid

2.

use Platinum as an electrode

c)

to represent the salt bridge

3.

use a double line ' | | '

d)

to start and end the line notation

4.

us the electrodes

e)

always

5.

show the state symbols for every species

31.

Which is the conventional way to depict a cell made from a zinc half-cell connected to a copper half-cell?

a)

Zn²⁺_(aq) | Zn_(s) | | Cu_(s) | Cu²⁺_(aq)

b)

Zn²⁺_(aq) | Zn_(s) | | Cu²_(aq) | Cu_(s)

c)

Zn_(s) | Zn²⁺_(aq) | | Cu²⁺_(aq) | Cu_(s)

d)

Zn_(s) | Zn²⁺_(aq) | | Cu_(s) | Cu²⁺_(aq)

32.

Below shows a cell diagram for voltaic cell. Which of the following is FALSE?

a)

Electrons flow from anode to cathode

b)

Oxidation happens in anode

c)

Copper undergo reduction to form copper ions

d)

Zinc undergo oxidation to form Zinc ions

33.

This electrode in a voltaic cell gains mass

a)

anode

b)

cathode

34.

What happens to the cell voltage when the salt bridge is removed?

a)

The cell voltage drops to zero.

b)

The cell voltage increases.

c)

The cell voltage becomes negative.

d)

The cell voltage is unchanged.

35.

In a voltaic cell, the half cell that receives anions from the salt bridge is

a)

cathode

b)

anode

36.

The diagram shows a zinc-copper voltaic cell. Which statement is not correct when the cell is operating?

a)

The overall reaction taking place is:

Cu2+(aq) + Zn(s) → Zn2+(aq) + Cu(s)

b)

The concentration of zinc ions in the zinc half-cell remains constant.

c)

Electrons flow from the zinc to the copper in the external circuit

d)

The salt-bridge allows the flow of ions between the two half-cells

37.

What is the correct derivation for the Nernst Equation at 298K, starting from the equation below?

$E_{cell}=E_{cell}^o-\frac{RT}{nF}\ln Q$

a)

$E_{cell}=E_{cell}^o-\frac{1.00}{nF}\log Q$

b)

$E_{cell}=E_{cell}^o-\frac{0.0591}{n}\log Q$

c)

$E_{cell}=E_{cell}^o+\frac{0.0591}{n}\ln Q$

d)

$E_{cell}=E_{cell}^o-\frac{0.0591}{n}\ln Q$

38.

What is the correct Nernst equation for the following cell:

Mg_(s) | Mg²⁺_{(aq, 0.001M)} | | Al³⁺_{(aq, 0.001 M)} | Al _(s)

a)

$E_{cell}=E_{cell}^{o_{ }}−\ \frac{0.0592}{6}\log\frac{\left[Mg^{2+}\right]^3}{\left[Al^{3+}\right]^2}$

b)

$E_{cell}=E_{cell}^{o_{ }}−\ \frac{0.0592}{6}\log\ \frac{\left[Al^{3+}\right]^2}{\left[Mg^{2+}\right]^3}$

c)

$E_{cell}=E_{cell}^{o_{ }}+\ \frac{0.0592}{3}\log\frac{\left[Mg^{2+}\right]^3}{\left[Al^{3+}\right]^2}$

d)

$E_{cell}=E_{cell}^{o_{ }}-\ \frac{0.0592}{3}\log\frac{\left[Mg^{2+}\right]^3}{\left[Al^{3+}\right]^2}$

39.

At different concentrations of ions in the two half cells, the measured current differs. Sort the statements into the correct categories.

Zn_(s) + Cu²⁺_(aq)→ Zn²⁺_(aq) + Cu_(s)

E° = 1.10 V ΔG° = -212 kJ/mol K = 1.5 × 10³⁷

$Q\ =\ \frac{\left[Zn^{2+}\right]}{\left[Cu^{2+}\right]}$

$Remember\ that\ \ \ \ E_{cell}=E_{cell}^o-\frac{RT}{nF}\ln Q$

Categorize the following

Q < 1

Q = 1

Q > 1

Q = K = 1.5 x 10³⁷

The concentration of copper ions is greater than zinc ions

The concentrations of copper and zinc ions are equal

Standard conditions

The concentration of zinc ions is greater than copper ions

The cell is at equilibrium

The cell is "dead".

lnQ < 0 i.e. negative

lnQ = 0

lnQ > 0 i.e. positive

E cell > E° cell

E cell = E° cell

E cell < E° cell

E = zero

40.

Calculate the E_cell for the following galvanic cell.

Zn(s) | Zn²⁺ (aq, 1.0M) || Ag⁺ (aq, 1.5M) | Ag(s)

E_Ag⁺| _Ag = +1.08V and E_Zn²⁺|_Zn = -0.76V

a)

0.32 V

b)

0.33 V

c)

1.84 V

d)

1.85 V

41.

Calculate the cell potential, E_cell of the electrochemical cell in which reaction

Pb²⁺ (aq) + Cd (s) → Pb (s) + Cd²⁺ (aq)

Given that E^o_cell = +0.277 V,

[Cd²⁺] = 0.02M, and [Pb²⁺] = 0.2M.

a)

0.207 V

b)

0.255 V

c)

0.307 V

d)

0.355 V

42.

The cathode is ___________.

Zn(s)|Zn(aq)²⁺‖Cd(aq)²⁺|Cd(s).

a)

Zn

b)

Zn²⁺

c)

Cd

d)

Cd²⁺

43.

The cathode is ___________.

Sn(s)|Sn(aq)²⁺‖Ag(aq)²⁺|Ag(s).

a)

Sn

b)

Sn²⁺

c)

Ag

d)

Ag²⁺

44.

Which is correct to write cell notation

Anode: Zn

Cathode: Ni

a)

Zn²⁺(aq, 1M) | Zn (s) || Ni (s) | Ni²⁺(aq, 1M)

b)

Zn (s) | Zn²⁺(aq, 1M) || Ni²⁺(aq, 1M) | Ni (s)

c)

Zn²⁺(s, 1M) | Zn (aq) || Ni (aq) | Ni²⁺(s, 1M)

d)

Zn (aq) | Zn²⁺(s, 1M) || Ni²⁺(s, 1M) | Ni (aq)

45.

Zn (s) | Zn²⁺(aq, 1M) || H⁺(aq, 1M) | H₂(g, 1 atm) | graphite (s)

Based on cell notation above, give the one electrolyte that can be used in the cathode.

a)

ZnSO₄(aq)

b)

H₂(aq)

c)

ZnCl₂(aq)

d)

HCl (aq)

46.

Based on the cell notation below, give a suitable formula for X in the cell notation below?

X | H₂(g, 1 atm) | H⁺(aq,1M) || Ag⁺(aq, 1M) || Ag (s)

a)

Ag (s)

b)

H (s)

c)

Pt (s)

d)

Zn (s)

47.

Based on cell notation, write overall equation:

Al(s) | Al³⁺(aq, 1M) || Pb²⁺(aq, 1M) | Pb(s)

a)

Pb(s) + Al³⁺(aq) ----------> Pb²⁺(aq) + Al(s)

b)

Pb²⁺(aq) + Al(s) ---------->Pb(s) + Al³⁺(aq)

c)

3Pb(s) + 2Al³⁺(aq) ----------> 3Pb²⁺(aq) + 2Al(s)

d)

3Pb²⁺(aq) + 2Al(s) ---------->3Pb(s) + 2Al³⁺(aq)

48.

Which of the cell notation is CORRECT for this redox equation:

2Ag⁺(aq) + Cu(s) --> Cu²⁺(aq) + 2Ag(s)

a)

Cu(s) │ Cu²⁺(aq, 1M) ║ 2Ag⁺(aq, 1M) │ 2Ag(s)

b)

Cu(s) │ Cu²⁺(aq, 1M) ║ Ag⁺(aq, 1M) │ Ag(s)

c)

Ag(s) │ Ag⁺(aq, 1M) ║ Cu²⁺(aq, 1M) │ Cu(s)

d)

2Ag(s) │ 2Ag⁺(aq, 1M) ║ Cu²⁺(aq, 1M) │ Cu(s)

49.

How can the cell potential, E_cell be increased based on the Nernst equation:
$E_{cell}=E_{cell}^o−\ \frac{0.0592}{n}\log\ \frac{\left[Zn^{2+}\right]}{\left[Ni^{2+}\right]}$

a)

Increase temperature

b)

Decrease concentration Ni²⁺

c)

Increase concentration Ni²⁺

d)

Choose E^ocell anode and cathode the positive value

50.

Calculate the cell potential, E_cell of the electrochemical cell in with reaction

Pb²⁺ + Cd → Pb + Cd²⁺

Given that E^o_cell = 0.277 V

[Cd²⁺] = 0.02M, and [Pb²⁺] = 0.2M

$E_{cell}^{ }=\ E_{cell}^o-\frac{0.0592}{n}\log Q$

a)

0.207 V

b)

0.255 V

c)

0.307 V

d)

0.355 V

51.

Calculate the concentration of silver ions Ag⁺ :
E^o_(Ag⁺/Ag) = 0.8V
E^o_(Cu²⁺/Cu) = 0.34V
Cell potential, E_cell(at 25^oC) = 0.422V,
Given [Cu²⁺] = 0.1M

(give your answer to 2decimal places)

$E_{cell\ }=\ E_{cell}^{o_{ }}-\frac{0.591}{n}\log\ Q$

(a)

52.

Standard electrode potential of a half-cell is measured with reference to

a)

standard hydrogen electrode with 1.00M H₂SO₄ solution

b)

standard oxygen electrode with 1.00M H₂SO₄ solution

c)

standard chlorine electrode with 1.00M H₂SO₄ solution

d)

d) standard hydrogen electrode with 1.00 M HCl solution

53.

What is the correct derivation for the Nernst Equation, starting from the equation below?

$E_{cell}=E_{cell}^o-\frac{RT}{nF}\ln Q$

a)

$E_{cell}=E_{cell}^o-\frac{1.00}{nF}\log Q$

b)

$E_{cell}=E_{cell}^o-\frac{0.0591}{n}\log Q$

c)

$E_{cell}=E_{cell}^o+\frac{0.0591}{n}\ln Q$

d)

$E_{cell}=E_{cell}^o-\frac{0.0591}{n}\ln Q$

54.

What phase must a compound be in order for electrolysis to work? (choose 2 of 4)

a)

molten

b)

solid

c)

aqueous

d)

gaseous

55.

An example for weak electrolyte is:

a)

HCl

b)

NaOH

c)

Acetic acid

d)

H₂SO₄

56.

6. Why is sodium chloride not able to conduct electricity in a solid state?

a)

Ion move freely

b)

Solid sodium chloride contains sodium ions

c)

Sodium ions and chloride ions are held together by the strong electrostatics force caused them not to move freely

d)

Sodium ions receive electrons to form a metal and chloride ions lose electrons to form chlorine gas

57.

Why must electrolyte must be in the liquid or aqueous state?

a)

So the ions can move

b)

So that ions does not get hot

c)

So the elements can move

d)

So the ions can be attracted

58.

What are the ions present in molten lead(II) bromide?

a)

PbBr₂

b)

Pb and Br

c)

Pb²⁺and Br^-

d)

Pb²⁺and Br₂^-

59.

V²⁺ + 2e^- --> V . E^o= -1.18V

Pb²⁺ + 2e^- --> Pb . E^o= -0.13V

Which of the following mathematical relationships would be most useful for determining the change in mass of an electrode after 1.0 minute of the cell's operation without having to use a balance?

a)

$E_{cell}^o\ =E_{cell}^o-\frac{RT}{nF}\ln Q$

b)

$I=\frac{q}{t}$

c)

$\Delta G=-nFE_{ }^o$

d)

$\Delta G=\Delta H-T\Delta S$

60.

Which factors affect amount of metal formed during electrolysis? (choose more than one)

a)

Charge on the metal ion

b)

Current

c)

Time

d)

Volume of electrolyte

61.

Which equation allows you to calculate the mass of a metal that will deposit on an electrode?

a)

$m\ =\ \frac{I\cdot t}{MM\cdot n\cdot F}$

b)

$m\ =\ \frac{n\cdot F}{MM\cdot I\cdot t}$

c)

$m\ =\ \frac{MM\cdot I\cdot t}{n\cdot F}$

d)

$m\ =\ \left(MM\cdot I\cdot t\right)\left(nF\right)$

62.

The anode is where oxidation occurs in...

a)

A Galvanic Cell

b)

A Electrolytic Cell

c)

Both Galvanic and Electrolytic cells

63.

In an electrolytic cell, the positive electrode is the

a)

anode, where oxidation occurs

b)

anode where reduction occurs

c)

cathode where oxidation occurs

d)

cathode where reduction occurs

64.

The method of coating metals by immersing the metals in a solution and then passing an electric current through the liquid is called ________

a)

Electrolysis

b)

Electrospading

c)

Electropalting

d)

Electroplation

65.

What is electrolysis?

a)

breaking down of a compound using a current

b)

making a compound using a current

66.

$m=\frac{MM\cdot I\cdot t}{n\cdot F}$

What are the units of the following:

mass = (a) moles = (b) times = (c) Faraday = (d) current = (e)

Choose from the below words

g

kg

mol e-

mol X^2+

seconds

minutes

C/mol e-

C

A

V

67.

What is the name given to the solution that is being electrolyzed?

a)

Salt solution

b)

Electrolyze

c)

Solvent

d)

Electrolyte

68.

Which of the following is TRUE about the particles present in solid and molten sodium chloride?

a)

both solid and molten sodium chloride contain ions

b)

solid sodium chloride contains atoms while molten sodium chloride contains ions

c)

solid sodium chloride contains molecules while molten sodium chloride contains ions

d)

solid sodium chloride contains atoms while molten sodium chloride contains molecules

69.

Why must electrolytes must be in the liquid (molten) or aqueous state?

a)

So the ions can move

b)

So that ions does not get hot

c)

So the elements can move

d)

So the ions can be attracted

70.

Which of the following is NOT an electrolyte?

a)

molten glucose (C₆H₁₂O₆)

b)

aqueous ammonia (NH₃)

c)

molten lead(II) bromide

d)

molten potassium iodide

71.

Glucose (C₆H₁₂O₆) does not conduct electricity because it...

a)

contains freely moving electrons

b)

has very low melting points

c)

does not contain ions

d)

contains ionic compounds which can dissolve in water

72.

Which one of the following statements is true for both galvanic cells and electrolytic cells?

a)

Reduction occurs at the negative electrode in both cells.

b)

Reduction occurs at the cathode in both cells.

c)

Anions migrate to the cathode in both cells.

d)

The anode is positive in both cells.

73.

What does the Cathode (-) do to ions in electrolytic cells?

a)

Give electrons to the positive ions to turn them into atoms

b)

Take electrons from the positive ions

c)

Turn ions back into atoms by removing electrons

d)

Turn atoms into ions by adding electrons

74.

Anion loses electrons at the

a)

cathode

b)

anode

75.

What substances are produced at positive/negative electrodes during the electrolysis of molten NaCI?

a)

Anode: Na⁺
Cathode: Cl₂

b)

Anode: Cl^-
Cathode: Na⁺

c)

Anode: Na
Cathode: Cl₂

d)

Anode: Cl₂
Cathode: Na

76.

What do you expect to observe at the positive and negative electrodes during electrolysis of molten NaCI?

a)

Anode: pH increases
Cathode: pH decreases

b)

Anode: metallic substance forms
Cathode: greenish bubbles form

c)

Anode: bubbles form
Cathode: bubbles form

d)

Anode: greenish bubbles form
Cathode: metallic substance forms

77.

Complete the answers for MOLTEN calcium bromide:

Cation: (a) Anion: (b) Product at the cathode: (c) Product at the anode: (d)

Choose from the below words

Ca²⁺

Br ⁻⁻

Ca

Br₂

Br₂⁻⁻

78.

A spoon is electroplated with chromium using chromium(III) nitrate. Which statement is correct?

a)

Positive electrode increases in mass

b)

Concentration of Cr³⁺ ions in solution decreases

c)

Reduction occurs at the anode

d)

Reaction at the cathode is Cr³⁺ + 3e^– → Cr

79.

What happens at the anode? (two answers)

a)

Cations are attracted, and are oxidised

b)

Anions are attracted, and are oxidised

c)

If there are competing species;

the most negative E^o gets oxidised

d)

If there are competing species;

the most positive E^o gets oxidised

80.

The diagram shows the electrolysis of copper(II) chloride solution using carbon as electrodes.

Which of the following is the correct half-equation representing the reaction at anode?

Cl_2(g) + 2e^- → 2Cl^-_(aq) (E° = 1.36 V)

O_2(g)+ 4H⁺_(aq) + 4e^- → 2H₂O_(l) (E° = 1.23 V)

a)

2H₂O_(l)→ O_2(g)+ 4H⁺_(aq) + 4e^-

b)

2Cl^- → Cl₂ + 2e^-

c)

Cu → Cu²⁺ + 2e^-

d)

Cu²⁺ + 2e^-→ Cu

81.

Molten X is electrolysed using carbon electrodes. After 10 minutes, a brown solid is deposited on the cathode and a brown gas is released at the anode. What is molten X?

a)

Lead(II) chloride

b)

Lead(II) bromide

c)

Copper(II) chloride

d)

Copper(II) bromide

82.

What happens during the electrolysis of water?

Categorize the following

bubbles of hydrogen is produced

bubbles of oxygen is produced

2H₂O_(l) + 2e^-→ H_2(g)+ 2OH^-_(aq)(E° = -0.83 V)

O_2(g)+ 4H⁺_(aq) + 4e^- → 2H₂O_(l) (E° = 1.23 V)

pH around this electrode decreases

pH around this electrode increases

Anode

Cathode

83.

Aqueous zinc chloride is electrolysed using platinum electrodes. What are the products expected at each electrode based purely on E^o values?

Zn²⁺_(aq)+ 2e⁻ → Zn_(s) (E° = -0.76 V)

2H₂O_(l) + 2e^-→ H₂ _(g)+ 2OH^-_(aq) (E° = -0.83 V)

Cl_2(g) + 2e^- → 2Cl^-_(aq) (E° = 1.36 V)

O_2(g)+ 4H⁺_(aq) + 4e^- → 2H₂O_(l) (E° = 1.23 V)

a)

cathode: hydrogen

anode: chlorine

b)

cathode: oxygen

anode: hydrogen

c)

cathode: zinc

anode: oxygen

d)

cathode: zinc

anode: water

Chapter 18 Review

Total questions: 83

Worksheet time: 2hrs 50mins

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