Free Printable Redox + Electrochemistry Mr.Alaa 0589151029

Worksheets

Redox + Electrochemistry Mr.Alaa 0589151029

Total questions: 68

Worksheet time: 57mins

Name

Class

Date

Which direction do the electrons flow in wire X and which metal is oxidized?

Which species is oxidized in the following reaction?

Ag⁺

Cu²⁺

Metal A is more reactive than metal B. Which statement is correct?

Electrons flow in the external circuit from A to B

Positive ions flow through salt bridge from A to B

Positive ions flow in external circuit from B to A.

Electrons flow through salt bridge from B to A

What is the function of Y in cell below?

To complete the circuit

To allow flow of electrons between both cells

To allow flow of ions

To connect both half cells

Reduction happens at the

anode

cathode

salt bridge

voltmeter

Oxidation happens at the

anode

cathode

salt bridge

voltmeter

Reactions in voltaic cells are

spontaneous, redox reactions

non-spontaneous, redox reactions

spontaneous, non-redox reactions

non-spontaneous, non-redox reactions

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

Electrons flow from the cathode to the anode

Electrons flow from left to right

Electrons flow from anode to cathode

Electrons flow from right to left

What reaction occurs at the anode?

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni²⁺ + 2e^- → Ni

Ni → Ni²⁺ + 2e^-

10.

In a voltaic cell, electrodes used are copper (electrolyte: copper (II) sulphate solution) and zinc (electrolyte: zinc nitrate solution). What is the half-equation that occur at the copper electrode?

Cu --> Cu2+ + 2e

2H+ + 2e --> H2

Cu2+ + 2e --> Cu

11.

A voltaic cell is producing the redox reaction below.

Mg(s) + Fe²⁺(aq) → Mg²⁺(aq) + Fe(s)

Which statement is correct when the cell produces electricity?

Magnesium atoms lose electrons.

Mass of the iron electrode decreases.

Electrons flow from the iron half-cell to the magnesium half-cell.

Negative ion flow from magnesium half-cell to iron half-cell.

12.

Which species is oxidized in the following reaction?

Ag⁺

Cu²⁺

13.

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

cathode

anode

14.

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

cathode

anode

15.

The anode is where oxidation occurs in...

A Galvanic Cell/ voltaic

A Electrolytic Cell

Both Galvanic and Electrolytic cells

16.

In an electrolytic cell, the positive electrode is the

anode, where oxidation occurs

anode where reduction occurs

cathode where oxidation occurs

cathode where reduction occurs

17.

What is an electrolytic cell?

a cell that converts chemical energy into electrical energy

a cell that converts electrical energy into electrical energy

a cell that converts electrical energy into chemical energy

A cell that converts kinetic energy into potential energy.

18.

What occurs during electrolysis of a molten salt?

Electricity is produced by a spontaneous redox reaction

Electricity cause a non-spontaneous redox reaction to occur

Electrons flow through the molten salt

Electrons are removed from both ions of the molten salt

19.

The reaction is non-spontaneous in ...

A Galvanic/ Voltaic Cell

A Electrolytic Cell

Both Galvanic and Electrolytic cells

20.

Calculate the cell potential of voltaic cell

–1.51

- 0.03

+0.03

+1.51

21.

Voltaic cell is made by connecting two half-cells below. Which statement is correct?

Mn is oxidized and voltage is 1.06 V

Pb is oxidized and voltage is 1.06 V

Mn is oxidized and voltage is 1.32 V

Pb is oxidized and voltage is 1.32 V

22.

Calculate the cell potential of voltaic cell

–1.60 V

+1.60 V

–3.12 V

+3.12 V

23.

Which represents reduction process occurring in standard hydrogen electrode?

H_2(g) → 2H⁺_(aq) + 2e^–

H⁺_(aq) + OH^–_(aq) → H₂O_(l)

2H⁺_(aq) + 2e^– → H_2(g)

O_2(g) + 4H⁺_(aq) + 4e– → 2H₂O_(l)

24.

Calculate the cell potential of voltaic cell

+ 0.01

+ 0.89

+ 1.77

+ 2.65

25.

What is the equation and cell potential?

2Al³⁺ + 3Ni → 2Al + 3Ni²⁺ E^O = 1.89 V

2Al + 3Ni²⁺ → 2Al³⁺ + 3Ni E^O = 1.89 V

2Al³⁺ + 3Ni → 2Al + 3Ni²⁺ E^O = 1.43 V

2Al + 3Ni²⁺ → 2Al³⁺ + 3Ni E^O = 1.43 V

26.

What is E^o for the following reaction?

+0.85

+0.51

–1.53

–1.87

27.

What is cell potential?

0.67

0.93

1.47

1.73

28.

Which of the following is a reversible battery type?

Alkaline battery

Lithium battery

Silver battery

Zinc carbon battery

29.

In dry cell ----------- is cathode

Zn plate

Powdered MnO₂and Carbon

Graphite rod

ZnCl₂and NH₄Cl

30.

During recharge secondary cells act like ------------ cells

Galvanic

electrolytic

Concentration

Voltaic

31.

In Lead Acid cells ------ is anode and ------is cathode

Pb is anode and PbSO₄ is cathode

Pb is anode and PbCl is cathode

Pb is anode and PbO₂is cathode

PbO₂is anode and PbCl is cathode

32.

The given reaction is for lead storage batteries done under acid (H₂SO₄ is an acid). What species is being reduced in this reaction?

PbO₂

H₂SO₄

None of the above

33.

What is the name of the process that uses electricity to separate the elements in a compound?

reduction

electrolysis

extraction

mining

34.

The electrodes in electrolysis of aluminium are made of

Steel

Anodes

Graphite

Plastic

35.

When NaCl solution is electrolysed what has forms at the anode?

Hydrogen

Oxygen

Chlorine

Sodium

36.

What is the equation to show what happens to Cl ions at the anode.

Cl^- --> Cl + e-

2Cl^- --> Cl₂ + 2e-

Cl₂ + 2e-2Cl^-

Cl₂ + 2e-_-->2Cl^-

37.

What is the half-equation for the discharge of hydroxide ions?

2O^2---> O₂+ 4e^-

OH^- --> OH + e

4OH^- --> 2H₂O + O₂ + 4e^-

2H₂O + O₂ + 4e^- --> 4OH^-

38.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

Bromine atoms in lead(II) bromide are converted to ions when it is melted

Electrons flow through the lead(II) bromide when it is melted

The ions in lead(II) bromide are mobile charge carriers in the molten state.

There are no ions in solid lead(II) bromide

39.

What ions are present in molten aluminium oxide?

Al³⁺, O^2-, H⁺, OH^-

Al³⁺, O^2-

Al³⁺, OH^-

40.

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

Salt solution

Electric solution

Mineral solution

Electrolyte

41.

Explain why the electrolyte has to be a liquid.

So the ions can move

So the electrons can move

So that it doesn't get too hot

So the fish are ok

42.

___________ electrode is an inert electrode.

Copper

Iron

Carbon

Zinc

43.

What is the equation to show what happens to Cl ions at the anode.

Cl^- --> Cl + e-

2Cl^- --> Cl₂ + 2e-

Cl₂ + 2e-2Cl^-

Cl₂ + 2e-_-->2Cl^-

44.

When NaCl solution is electrolysed what has forms at the anode?

Hydrogen

Oxygen

Chlorine

Sodium

45.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

Bromine atoms in lead(II) bromide are converted to ions when it is melted

Electrons flow through the lead(II) bromide when it is melted

The ions in lead(II) bromide are mobile charge carriers in the molten state.

There are no ions in solid lead(II) bromide

46.

What is the product formed at the anode during the electrolysis of concentrated copper(II) chloride?

copper

chlorine

hydrogen

oxygen

47.

Choose the half-equation that shows the discharge of aluminium ion.

Al³⁺ - 3e^- --> Al

Al²⁺ + 3e^- --> Al

Al³⁺ + 3e^- --> Al

Al³⁺ --> Al + 3e^-

48.

What is the half-equation for the discharge of hydroxide ions?

2O^2---> O₂+ 4e^-

OH^- --> OH + e

4OH^- --> 2H₂O + O₂ + 4e^-

2H₂O + O₂ + 4e^- --> 4OH^-

49.

What is the product formed at the cathode during the electrolysis of molten magnesium fluoride?

magnesium

hydrogen

fluorine

oxygen

50.

Electricity is passed separately through concentrated hydrochloric acid, concentrated aqueous

sodium chloride and dilute sulfuric acid.

In which rows are the electrolysis products correctly named?

1, 2 and 3

1 and 2 only

1 and 3 only

2 and 3 only

51.

The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous

sodium chloride using carbon electrodes.

At which electrode(s) is hydrogen produced?

electrode 1 only

electrodes 1 and 3

electrode 2 only

electrodes 2 and 4

52.

___________ electrode is an inert electrode.

Copper

Iron

Carbon

Zinc

53.

Positive ions (cations) will move towards the cathode (-) where they will discharge by....

Breaking apart

Losing electrons

Clumping together.

Gaining electrons

54.

What state must the ionic compound be in to be electrolysed?

aqueous only

solid only

solid or aqueous only

molten or aqueous only

55.

What is Brine?

Water with a high concentration of Sodium Chloride

Water with a high concentration of Lead Bromide

Vinegary water

Pure water

56.

Na is a metal, and Chlorine is non-metal halogen. Which of these will be broken down into positive ions, and which will be negative ions?

Na+ and Cl-

Na- and Cl+

Na+ and Cl+

Na- and Cl-

57.

Water is composed of H₂O (2 Hydrogen and 1 Oxygen). Which of these will be broken down into positive ions, and which will be negative ions?

H+ and OH-

H- and OH+

HH+ and O-

OO+ and H-

58.

Which ions are attracted to the negative electrode (cathode)?

Na+ and H+

Cl- and OH-

Na+ and Cl-

H+ and OH-

59.

Hydrogen gas will form at which electrode?

Negative electrode (cathode)

Positive electrode (anode)

Both

Neither

60.

Chlorine gas will form at which electrode?

Negative electrode (cathode)

Positive electrode (anode)

Both

Neither

61.

Which of the following statements is NOT true about the rusting of an iron nail

Corrosion is the oxidation deterioration of a metal by an electrochemical process

Iron rusts faster if it is in contact with a more electropositive metals

Rusting of iron occurs when oxygen and water are present

When iron rusts, iron is first oxidised to Fe²⁺ ions

62.

What is frequently done to protect aluminium articles from subsequent corrosion?

Aluminium is coated with an inert metal

Cryolite is added to the aluminium ore before it is used

Aluminium is first oxidised by air to form an inert oxide layer

The aluminium is made the anode during electrolysis

63.

Which statement explains why graphite powder is spread onto plastic material first in plastic electroplating process?

Graphite is an electric conductor

Plastic becomes more resistant to heat

Plastic electroplating process is accelerated

Graphite can form chemical bond with plastic

64.

Electroplating is a process whereby a metal surface is coated with a non-metal.

True

False

65.

The electrode that contains the plating metal

Anode

Cathode

66.

The electrode that contains the item to be electroplated

Anode

Cathode

67.

The electrode that contains the plating metal

Anode

Cathode

68.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

Molten calcium chloride

Aqueous silver nitrate

Sodium chloride solution

Copper(II) sulphate solution

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Redox + Electrochemistry Mr.Alaa 0589151029

Total questions: 68

Worksheet time: 57mins

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