6 electrochemistry

WAJA F4 Chemistry 2009 Chapter 6: Electrochemistry

CHAPTER 6: ELECTROCHEMISTRY

A ELECTROLYTES AND NON-ELECTROLYTES

Activity 11. State the meaning of electrolyte:

An electrolyte is a substance that can conduct (a) ……………………in (b)………………

state or (c) ……………………. (d)……………………. and undergo (e)……………………

(f)…......................….

2. A non-electrolyte is a substance that cannot conduct (g)……………………. either in

(h)……………………. state or (i)……………………….. solution.

3. Ionic compounds in molten state or in aqueous solution are electrolytes

because these substances contain freely (j) …………………. …………………….

4. Covalent compounds are non-electrolytes and these substances contain neutral

(k) ................... and no freely (l) ……………………… …………… However,

certain covalent compounds such as hydrogen chloride, ammonia and ethanoic

acid when dissolved in water are electrolytes. This is because these compounds react

with water to produce freely (m) ………………… …………..

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Learning Outcomes:

You should be able to: state the meaning of electrolyte, classify substances into electrolytes and non-electrolytes. relate the presence of freely moving ions to electrical conductivity.


5. Ionic compounds in molten state or in aqueous solution are electrolytes while covalent compounds and ionic compounds in solid state are non-electrolytes. Metals are non-electrolytes but are good conductors of electricity.

Classify the substances in the text box below into electrolyte and non-electrolyte

Electrolyte Non-electrolyte

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Solid lead(II) chloride, molten aluminium oxide, lead(II) nitrate solution, solid sodium chloride, sodium chloride solution, magnesium, molten lead(II) chloride, glucose solution, glacial ethanoic acid, dilute ethanoic acid, molten naphthalene, ethanol, silver, tetrachloromethane, sodium hydroxide solution, aqueous ammonia


B ELECTROLYSIS OF MOLTEN COMPOUNDS

Activity 21. What do you understand by the term electrolysis?

Electrolysis is a process whereby compounds in (a) .................... or (b) ..……………

states are broken down (or decomposed) into their constituent (c) …………………… by

passing (d) ……………………. through them.

2. Anode is the electrode which is connected to the (e) …………………. terminal of a battery.

3. Cathode is the electrode which is connected to the (f) ……………………… terminal of a battery.

4. Carbon or platinum is chosen as electrodes as they are chemically inert or unreactive. 5. The diagram below shows the set-up of apparatus of electrolysis of molten lead(II)

bromide. Name the main apparatus and materials in the diagram.

Activity 31. Diagram 3.1 shows the relationship between the presence of freely moving ions and

electrical conductivity.The box below shows a list of statements that explain the why ionic compound in solid state do not conduct electricity but will conduct electricity in aqueous solution. The statements are arranged in random order.Choose the correct statement from the box below and write it into the correct text box in Diagram 3.1.

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Learning Outcomes:You should be able to: describe electrolysis, describe electrolytic cell, identify cations and anions in a molten compound, describe evidence for the existence of ions held in a lattice in solid state but move freely in

molten state, describe electrolysis of a molten compound, write half-equations for the discharge of ions at anode and cathode, predict products of the electrolysis of molten compounds.


Diagram 3.1

2. Colour all the cations red and the anions blue in solid sodium chloride and in the electrolyte in Diagram 3.1 above.

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During electrolysis cations are attracted to the cathode and anions are attracted to the anode. Solid sodium chloride contains sodium ions and chloride ions which are in fixed position and

not freely moving. In solid state, sodium ions and chloride ions are strongly attracted by electrostatic forces in a

lattice. Electric circuit is complete due to the flow of electrons along the connecting wires and

movement of ions in the solution. If the electrodes are placed further apart, the ammeter reading will decrease because there

will be an increase in internal resistance. Aqueous sodium chloride contains freely moving ions to conduct electricity.


Activity 4

1. Given below is a list of ionic compounds in molten state. Identify the cation and anion in each electrolyte.

Electrolyte(Molten)

Cation AnionName Formula Name Formula

Sodium chloride

Lead(II) oxide

Potassium bromide

2. Given below is a list of electrolytes and products discharged at both electrodes. Based on the given substance discharged at the electrode, write a half equation to represent the reaction occurring at the electrode.

Electrolyte(molten)

Substance discharged at the electrodesand the half equation

Anode Cathode

(i) Aluminium oxide

Oxygen gas Half equation:

……………………………………..

Aluminium Half equation:

……………………………………..

(ii) Potassium iodide Iodine Half equation:

……………………………………

Potassium Half equation:

……………………………..………

(iii) Sodium chloride Chlorine gas Half equation:

…………………………………..…

Sodium Half equation:

………….…………………………

(iv) Zinc bromide Bromine gas Half equation:

………………………………..……

Zinc Half equation:

…………….………………………

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Activity 5 1 The flow chart below is used to predict the products formed at the electrodes during the

electrolysis of molten lead(II) bromide.

2. In the spaces below, draw a similar flow chart (as in question 1) to predict the products formed at the electrodes from the electrolysis of molten zinc chloride, ZnCl2.

C ELECTROLYSIS OF AQUEOUS SOLUTION

Learning Outcomes:You should be able to: identify cations and anions in an aqueous solution, describe the electrolysis of an aqueous solution, explain using examples factors affecting electrolysis of an aqueous solution, write half equations for the discharge of ions at the anode and the cathode, predict the products of electrolysis of aqueous solutions.

Activity 6

1. State three factors that may influence the selective discharge of ions during the electrolysis of an aqueous solution.

(a) …………………………………………………………………………………………………

(b) ………………………………………………………………………………………………….

(c) ………………………………………………………………………………………………….

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d

Molten lead(II) bromide

a

gf

e

cb

Consists of

(Ions that are present)

( Movement of ions)To anode

To cathode

(Half equation)At Anode

At Cathode

(Products formed)At Anode

At Cathode


2. In an aqueous solution of sodium chloride, apart from sodium ions, Na+ and chloride

ions, Cl-- , ………………………ions, ……… and ……………………………….ions, ……

from the slight dissociation of water are also present.

3. List the electrochemistry series (cations and anions) in order of increasing ease of discharge.

Ease of discharge increases

Cation: …………………………………………………………………………………………….

Anion: ……………………………………………………………………………………………..

4. The following statements refer to the factors that affect the electrolysis of an aqueous solution. Fill in the blanks.

(a) The ions that are placed …………………… in the electrochemical series will be ……………….. discharged.

(b) If the concentration of a particular ion is …………………, the ion is ……………..

………………………

(c) In the electrolysis of copper(II) sulphate, CuSO4 ……………..using copper

electrodes, no ions are discharged at the anode. Instead, the copper anode …………………… and ………………………… in the electrolyte.

Activity 7The diagram below shows the set-up of apparatus of an electrolytic cell containing concentrated copper(II) sulphate solution. Two test tubes filled with copper(II) sulphate solution were placed over the electrodes J and K to collect any gas evolved. The switch is then turned on so that electrolysis of copper(II) sulphate solution can occur.

(a) Identify the cations and the anions present in the aqueous solution.

Cations: …………………………………….. Anions: …………………..………………………

(b) Identify which electrode ( J or K ) is the anode and the cathode:

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Anode ……………………………….. Cathode ……………………………………….

(c) (i) Which ion is selectively discharge at the anode? ………………………………………

(ii) Give a reason for your answer in (c) (i). …………………………………………………..

…..…………………………………………………………………………………………….

(iii) What do you observe at the anode? ………………………………………………………

(iv) Give one test to confirm the gas released at K. …………………………………………

………………………………………………………………………………………………. (v) Write a half equation to represent the discharge of ions at anode.

…….……………………………………………………………………………………………

(d) (i) Which ion is selectively discharge at the cathode? …………………………………………

(ii) Give a reason for your answer in (d) (i) ………………………………………………….

…………………………………………………………………………………………………

(iii) Which do you observe at the cathode? …………………………………………………

(iv) Write a half equation to represent the discharge of ions at the cathode.

…………………………………. ………………………………………………………….

(e) What do you observe about the copper(II) sulphate solution? …………………………………………………………………………………………………..

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Activity 8The table below shows three electrolytic cells with different electrolytes and different electrodes. You are required to answer each section by writing your answer in the spaces provided.

1. In the diagrams, label the cathode with the symbol “” and the anode with the symbol “+”.

2. Show the direction of the flow of the electrons with arrowheads, “ > “

3. Write the formula of all ions in the electrolyte.

4. Write the formula of ions which are attracted to the cathode.Underline the formula of ion which is selectively discharged.

5. Write the half equation to represent the reaction at the cathode.

6. What will you observe at the cathode?

7. Write the formula of ions which are attracted to the anode.Underline the formula of ion which is selectively discharged.

8. Write the half equation to represent the reaction at the anode.

9. What will you observe at the anode?

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D ELECTROLYSIS IN INDUSTRIES

Learning Outcomes:You should be able to: state uses of electrolysis in industries, explain the extraction, purification and electroplating of metals involving electrolysis in industries, write chemical equations to represent the electrolysis process in industries, justify uses of electrolysis in industries, describe the problem of pollution from electrolysis in industry.

Activity 9

1. Fill in the blanks.

The application of electrolysis in industries are (a) ……………………………………….

(b) ……………………………………………… and (c) ……………………………………

In the extraction of aluminium from its ore, (d) ….……………… electrodes are used

and (e) ……..………………. is added to aluminium oxide to lower its melting point.

In purification of metals, the pure metal is made the (f) ….………………. and the

impure metal is made the (g) ……….……………. The electrolyte used is an aqueous

salt solution of the metal ions.

In electroplating of metals, the (h) ………..…………….is made the anode and the (i)

……………… to be (j) ..…..………………….. is made the cathode. The electrolyte

used is an aqueous salt solution of the electroplating metal.

The purposes of electroplating metals are to make the electroplated object more (k)

………………………………….. and (l) …………………..……………… to corrosion.

2. Below are shown the three uses of electrolysis in industries. Fill in the blanks.

Extraction of aluminium from bauxites

Purification of copper from impure mined copper

Electroplating of iron spoon with silver

1. Substance used as cathode and anode

Cathode:

Anode:

Cathode:

Anode:

Cathode:

Anode

2. Electrolyte used

3. Half equation representing the process.

Cathode:

Anode:

Cathode:

Anode:

Cathode:

Anode:

E VOLTAIC CELLS

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Activity 10 1. A simple voltaic cell can be constructed by immersing two ……………………….

metals in an ………………………. connected by …………………

2. In a voltaic cell, ……………………… energy is converted to ……………………. energy.

3. THE ELECTROCHEMICAL SERIES is an arrangement of metals based on the tendency of each metal atom to donate electrons. Complete the table below.

Electrochemical series of metalsCation formed and number of

electron(s) released during the process

K K+ + e

Al Al3+ + 3e

* Note: Hydrogen is not a metal, but it is included in the Electrochemical Series.

4. The diagram below shows an example of a simple voltaic cell.

Learning outcomes:You should be able to: describe the structure of a simple voltaic cell and Daniell cell, explain the production of electricity from a simple voltaic cell, explain the reactions in a simple voltaic cell and Daniell cell, compare and contrast the advantages and disadvantages of various voltaic cells, describe the differences between electrolytic and voltaic cells.

Tendency of metal atoms to donate electrons to form ions increases

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In the text box below are sentences explaining the production of electricity from a simple voltaic cell. The sentences are listed in random order. You are required to arrange these sentences in the best possible order so as to give a clear description of the reactions occurring in a simple voltaic cell.

[If you have any problem, you can refer to page 104 of the text book for guidance.]

Answer:

(a) ………………………………………………………………………………………………………

………………………………………………………………………………………………………

(b) ………………………………………………………………………………………………………

………………………………………………………………………………………………………

(c) ……………………………………………………………………………………………………..

………………………………………………………………………………………………………

(d) ………………………………………………………………………………………………………

An example of a simple voltaic cell is a magnesium strip and a copper strip immersed in dilute sodium chloride solution.

The electrons then flows from the magnesium ribbon to the copper plate through the wire and this results in the flow of electrical current.

Hence magnesium atom releases electrons more easily than a copper atom and the magnesium act as the negative terminal of the cell.

The overall equation for the reaction is given as follows. Mg(s) + 2H+(aq) Mg2+(aq) + H2(g)

Magnesium is placed higher than copper in the electrochemical series. At the negative terminal, each magnesium atom releases two electrons and the Mg2+

formed moved into the solution. Mg(s) Mg2+ (aq) + 2e At the positive terminal which is the copper plate, the electrons are accepted by the H+

ions in sodium chloride solution. 2H+ + 2e H2 (g)

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………………………………………………………………………………………………………

(e) ………………………………………………………………………………………………………

………………………………………………………………………………………………………

(f) ……………………………………………………………………………………………………… ……………………………………………………………………………………………………………

(g) ……………………………………………………………………………………………………….

……………………………………………………………………………………………………..

Activity 111. (a) Draw and label the set-up of apparatus of a Daniell cell consisting of a salt bridge.

(b) (i) Which metal in the Daniell cell is the negative terminal?

…………………………………………………………………………………………………(ii) Give reason for your answer in (b)(i).

………………………………………………………………………………………………… (iii) Write a half equation to represent the reaction occurring at the negative terminal.

…………………………………………………………………………………………………. (c) Write a half equation to represent reaction at positive terminal.

…………………………………………………………………………………………………… (d) What do you observe at

(i) negative terminal

………………………………………………………………………………………………….. (ii) positive terminal

………………………………………………………………………………………………….. (e) State two functions of the salt bridge.

1. ……………..……………………………………………………………………………… 2. ………………………………………………………………………………………………

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2. The table below listed are five types of voltaic cells commonly used in our daily lives. Each voltaic cell has its advantages and disadvantages. Complete the table by stating the advantages and disadvantages of each voltaic cell.

Voltaic cell Advantages Disadvantages

1. Lead-acid accumulator

2. Dry cell

3. Mercury cell

4. Alkaline cell

5. Nickel-cadmium cell

Activity 12What are the differences between an electrolytic cell and a voltaic cell?Table 12.1 are statements showing differences between an electrolytic cell and a voltaic cell. Complete Table 12.2 by choosing the correct matching statements.

It does not require a source of electric current

It requires a source of electric current

The electrical energy causes chemical reactions to occur at the electrodes.Electrical energy chemical energy

The chemical reaction that occur at the electrodes produces electric current. Chemical energy electrical energy

The electrodes must be of two different metals

The electrodes may be of the same material such as carbon

Electrons flow from the positive electrode (anode) to the negative electrode (cathode).

Electrons flow from the more electropositive metal (negative terminal) to the less electropositive metal (positive terminal).

Ions receive electrons at the positive terminal.(Reduction)

Ions donate electrons at the positive terminal. (Oxidation)

Ions receive electrons at the negative terminal.(Reduction)

Ions donate electrons at the negative terminal.(Oxidation)

Table 12.1

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DIFFERENCESElectrolytic cell Aspect Chemical cell

Source of electric current

Conversion of energy

Type of electrodes

Direction of flow of electrons

Type of reaction at positive terminal

Type of reaction at negative terminal

Table 12.2

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F THE ELECTROCHEMICAL SERIES

Learning Outcomes:You should be able to: describe the principles used in constructing the electrochemical series, construct the electrochemical series, explain the importance of electrochemical series, predict the ability of a metal to displace another metal from its salt solution, write the chemical equations for metal displacement reactions.

Activity 13Three experiments were conducted to investigate the potential differences between three pairs of metals in a voltaic cell. An electrochemical series for four metals P, Q, S and T is then constructed based on the potential difference obtained. Three pair of metals used as electrodes in different voltaic cells are: P and Q, Q and S and S and T.All the metals are cleaned with sandpaper before used.50 cm3 of 1.0 mol dm-3 sodium nitrate solution is poured into a beaker as electrolyte.

Experiment IThe electrodes P and Q are immersed into the solution. The two electrodes are connected to a voltmeter using copper wires. Electrode Q is the positive terminal. The voltmeter reading is recorded.

Experiment IIThe electrodes Q and S are immersed into the solution. The two electrodes are connected to a voltmeter using copper wire. Electrode Q is the positive terminal. The voltmeter reading is recorded.

Experiment IIIThe electrodes S and T are immersed into the solution. The two electrodes are connected to a voltmeter using copper wire. Electrode T is the positive terminal. The voltmeter reading is recorded.

Based on Experiment I, II and III, answer the questions below.(a) Record the voltmeter reading of each experiment in the spaces provided. Experiment 1 Experiment II Experiment III

Voltmeter reading: …………. Voltmeter reading: …………… Voltmeter reading: ….……..

(b) Construct a table to record the data from the above experiments.

01 2 3 4

56

V

01 2 3 4

56

V

01 2 3 4

56

V

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(c) List the apparatus and materials that you will need to carry out this experiment.

Apparatus: ……………………………………………………………………………………….

……………………………………………………………………………………………………..

Materials: ………………………………………………………………………………………..

……………………………………………………………………………………………………(d) State all the variables:

1. Manipulated variable: …………………………………………………………………..

2. Responding variable: …………………………………………………………………….

3. Controlled variable: ………………………………………………………………………

(e) State the hypothesis: ……………………………………………………………………….

…………………………………………………………………………………………………..(f) Based on the information obtained in Experiment I, what can you infer about metal P and

Q?

……………………………………………………………………………………………………(g) Write a half equation for the reaction occurring in negative of Experiment I, assuming the

cation has a +2 charge.

……………………………………………………………………………………………………….(h) Arrange the metals P, Q, S and T in descending order of their tendency to donate

electrons....……………………………………………………………………………………………………

(i) Another voltaic cell is set-up using metals T and Q as electrodes. Predict the potential difference produced in the cell.

……………………………………………………………………………………………………..(j) Given that metal X is placed between metal S and metal Q in the electrochemical series,

can metal X displace metal S from its salt solution? Give an explanation for your answer

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….(k) Given that copper is more electropositive than metal T, a displacement reaction will

occur when copper is immersed into a salt solution of metal T, TNO3. Write the chemical equation for this reaction.

……………………………………………………………………………………………………….(l) State three important uses of the electrochemical series

…………………………………………………………………..…………………………………

…………………………………………………………………………………………………….

……………………………………………………………………………………………………...

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6 electrochemistry

Documents

sodium half equation

potassium half equation

aluminium half equation

zinc half equation

half equation anodecathode

molten state

nonelectrolytes activity

list of electrolytes