All Saints SecondaryStandard Grade Chemistry
Topic 10 – Making Electricity
General Level
1.Leia was investigating electrical conductivity. She set up four experiments.
A / BC / D
Identify the experiment(s) in which the bulb will light.
1 mark (PS)
2.(a) A pupil set up the following cell and measured the cell voltage.
(i)Name the type of charged particle that flows through the connecting wires.
1 mark (KU)
(ii) The pupil repeated the experiment using cans made from different metals.
The results are shown in the table.
Metal can / Cell voltage/Valuminium / 1.86
zinc / 0.92
tin
Complete the table to show a voltage you might expect for the cell using the tin can.
You may wish to use page 7 of the data booklet to help you. 1 mark (PS)
(b)A battery is a number of cells joined together.
Give one advantage of using a battery rather than mains electricity.
1 mark (KU)
3. Pairs of metals can be used to produce a cell.
(a)What is the purpose of the filter paper soaked in sodium chloride solution?
1 mark (KU)
(b)On the wires, indicate the direction of electron flow.
1 mark (PS)
(c)Give the name of a metal which could replace the nickel and cause the electrons to flow in the opposite direction.
1 mark PS)
(d)Cells are used in calculators and watches.
Give a disadvantage of a cell compared with mains electricity.
1 mark (KU)
4.Batteries can be used to power everyday items. A battery is a number of cells joined together.
(a)(i)What happens inside a battery to produce electricity?
1 mark (KU)
(ii) Suggest an advantage in using a battery rather than mains electricity.
1 mark (KU)
(b)A simple cell can be made from everyday objects.
(i) Draw an arrow on the wire to show the direction of electron flow.
1 mark (PS)
(ii) What would happen to the voltage if the iron nail was replaced with aluminium foil?
You may wish to use page 7 of the data booklet.
1 mark (PS)
5.This is a diagram of a dry cell commonly used in torches.
(a) (i) Why is the ammonium chloride used as a paste and not as a
drypowder?
1 mark (PS)
Eventually the cell stops producing electricity and has to be replaced.
(ii) Explain why the cell stops producing electricity.
1 mark (KU)
(b)Car batteries are made from much heavier wet cells containing lead plates and sulphuric acid.
Suggest the main advantage of this lead-acid battery.
1 mark (PS)
6.There are many different types of battery.
(a)The diagram shows an alkaline-manganese battery.
(i)After some time, this battery stops producing electricity.
Why does this happen?
1 mark (KU)
(ii)Suggest -why this type of battery is known as an alkaline battery.
1 mark (PS)
(iii)Why is the potassium hydroxide used in the form of a paste and not as a dry powder?
1 mark (PS)
7.A simple dry cell can be made from everyday materials.
The paste is made from salt (sodium chloride), water and porridge, Porridge is mainly composed of starch.
(a)On the diagram, clearly mark, with an arrow, the direction in which electrons flow through the wire.
1 mark (PS)
(b)Name the electrolyte in the paste.
1 mark KU)
(c)Why could sugar not be used as an electrolyte?
1 mark (PS)
(d)Would the voltage reading be higher or lower if an aluminium can were used?
1 mark (PS)
8. Car batteries can be recharged.
(a)What type of electrolyte is used in a car battery?
1 mark (KU)
(b)Give one advantage of using batteries rather than mains electricity.
1 mark (KU)
9.The diagram shows a copper/zinc cell.
(a)In the cell, the electricity flows through the wires from the zinc to the copper.
Name the type of charged particle that flows through the wires.
1 mark (KU)
(b)What is the purpose of the ion bridge?
1 mark (PS)
(c)Eventually the cell would stop producing electricity. Give a reason for this.
1 mark (KU)
(d)Name a metal which could replace zinc to produce a larger voltage.
You may wish to use page 7 of the data booklet.
1 mark (PS)
Credit Level
1.A bromide ion is formed when a bromine atom gains one electron.
Identify the true statement(s) about this change.
A / The / change represents reduction.B / The / atomic number increases by one.
C / The / particle becomes negatively charged.
D / The / number of electron energy- levels increases by one.
E / The bromide ion has the same electron
arrangement as an argon atom.
1 mark (PS)
2.There are many different types of chemical reaction.
A / B / Creduction / precipitation / displacement
D / E / F
hydrolysis / neutralisation / oxidation
(a)Identify the following type of reaction.
S032-(aq)+H2O(l)SO42-(aq)+2H+(aq)+2e-
1 mark (KU)
(b)Identify the type(s) of reaction represented by the following equation.
Fe(s) + Cu2+S042-(aq) Cu(s) + Fe 2+SO42-(aq)
1 mark (KU)
3.Electrolysis is a common industrial process. Some uses of electrolysis are shown in the diagram.
(a)State what is meant by electrolysis.
1 mark (KU)
(b)Aluminium is extracted by electrolysis of its molten oxide since aluminium oxide does not react when heated with carbon.
Why does aluminium oxide not react with hot carbon?
1 mark (KU)
(c)Chlorine is produced by the electrolysis of sodium chloride solution. Write the ion-electron equation for the formation of chlorine.
You may wish to use the data booklet to help you.
1 mark (PS)
(d)Tin plated iron rusts very rapidly if the plating is scratched. Explain why the iron rusts so rapidly.
2 marks (KU)
4.Helen set up the cell shown below.
The reaction taking place at electrode A is
Fe3+(aq) + e- Fe2+(aq)
(a)(i) On the diagram, clearly mark the path and the direction of
electron flow.
1 mark (PS)
(ii) What term is used to describe the type of chemical reaction taking place at electrode A?
1 mark (KU)
(b)Iodine forms at electrode B.
(i)What would you see happening around electrode B?
1 mark (PS)
(ii)Write an ion-electron equation for the chemical reaction taking place at electrode B.
You may wish to use the data booklet to help you.
1 mark (PS)
5.The diagram shows a cell which can produce electricity.
(a)What is the purpose of the ion bridge?
1 mark (KU)
(b)Name a tin compound which could be used to make the solution containing tin ions.
You may wish to use page 5 of your data booklet to help you.
1 mark (PS)
(c)The following cell produces a higher voltage than the cell above.
Suggest a name for metal X.
1 mark (PS)
6.Copper displaces silver from silver(I) nitrate solution.
Cu(s) + 2Ag+(aq) + 2N03- (aq) Cu2+(aq) + 2N03- (aq) + 2Ag(s)
(a)Rewrite the equation omitting the spectator ions.
1 mark (KU)
(b)Write the ion-electron equation for the oxidation step in the displacement reaction.
You may wish to use the data booklet to help you.
1 mark (PS)
(c)The reaction can also be carried out in a cell.
(i)Complete the three labels on the diagram.
1 mark (PS)
(ii)The purpose of the ion bridge is to complete the circuit.
Suggest why sodium carbonate solution should not be used in the ion bridge.
You may wish to use the data booklet to help you.
1 mark (PS)
7.Zinc reacts with copper sulphate solution.
Zn(s) + Cu2+(aq) + SO32- (aq) Zn2+(aq) + S042-(aq) + Cu(s)
(a)Rewrite the equation omitting the spectator ions.
1 mark (KU)
(b) Draw a labelled diagram in the space below to show how all of the pieces of apparatus shown can be used to make a cell.
2 marks (PS)
8.Silver oxide cells are used in calculators and watches.
(a)(i) How iselectricity produced in a cell?
1 mark (KU)
(ii) Give a disadvantage of a cell.
1 mark (KU)
(b)The equation shows the reaction which takes place at the zinc electrode.
Zn(s) + 2(OH)-(aq) Zn0(s) + H2O(l) + 2e-
State why the equation represents oxidation.
1 mark (KU)
(c)Why has the separator been soaked in potassium hydroxide solution?
1 mark (PS)
9.Acids can be shown to contain H+(aq) using a Hoffman voltameter.
(a)Why must a d.c. supply be used?
1 mark (KU)
(b) The volume of hydrogen gas produced over a period of time was measured
during the electrolysis of dilute sulphuric acid.
The results are shown in the table.
Time (min) / 0 / 5 / 8 / 12 / 20Volume of gas (cm3) / 0 / 8.5 / 13.5 / 20.0 / 33.0
Draw a line graph of the results.
2 marks (PS)
(c) Predict the volume of hydrogen gas which would be produced during the first
10 minutes.
1 mark (PS)
(d) Write the ion-electron equation for the formation of hydrogen gas.
You may wish to use your data booklet to help you.
1 mark (KU)
10.Roy wanted to show that chemicals can be used to produce an electric current.
When the crocodile clips (labelled A and B) were attached to certain parts of the apparatus, the ammeter gave a reading.
(a)i) Show clearly on the diagram, using labels A and B, where the
crocodile clips could have been attached.
1 mark (PS)
(ii)Why was no current produced when the porous cardboard container was replaced by a glass beaker?
1 mark (PS)
(iii)What would happen to the reading on the ammeter if the zinc rod was replaced with a tin rod in a tin chloride solution?
1 mark (PS)
(b)Roy was instructed to make 50 cm3of a 1 mol/litre solution of copper chloride, CuC12.
Calculate the mass, in grams, of copper chloride needed.
Show your working clearly.
2 marks (KU)
19.The cell below can be used in a carbon monoxide detector.
Carbon monoxide enters the cell along with oxygen from the air at electrode A.
The reactions occurring at each electrode are:
Electrode A
CO(g) + H20(g)CO2(g) + 2H+(aq) + 2e-
Electrode B
2H+(aq) + 202 (g) + 2e H20 (l)
(a)On the diagram, clearly mark the path and direction of electron flow.
1 mark (PS)
(b)What is the purpose of the electrolyte in the above cell?
1 mark (KU)
(c)Sugar solution cannot be used as an electrolyte.
1 mark (PS)
(d)Platinum is used for the electrodes in this cell
(i)To which family of metals does platinum belong
1 mark (PS)
(ii)Platinum is also used as a catalyst in a catalytic converter in car exhausts.
What does a catalytic converter do?
1 mark (KU)
Topic 10 Homework – Making Electricity