Berry List of Chemistry Experiments (PEKA) Form 5 (Part 3)

by BerryBerryTeacher

in Berry Experiment (Experiments & PEKA)

This post is the list of PEKA experiments for SPM Chemistry Form 5 from Berry Berry Easy. Please familiarise with all these experiments from SPM Form 5 Chemistry Chapter 3: Oxidation and Reduction before conducting them so as to be better prepared. The list of experiments are as below:

Berry List of Chemistry Experiments (PEKA) Form 5 (Part 3)

Chapter 3 – Oxidation and Reduction

List of PEKA experiments:

  1. Redox reaction as loss or gain of oxygen
  2. Change of iron(II) to iron(III) ions and vice versa
  3. Displacement of metals
  4. Displacement of halogens
  5. Transfer of electrons at a distance
  6. Effect of other metals on rusting
  7. Reactivity of metals with oxygen
  8. (A) The position of carbon in the reactivity series of metals with oxygen (B) Heating carbon dioxide with metals
  9. The position of hydrogen in the reactivity series of metals (Demonstration by teacher)
  10. Oxidation and reduction in electrolytic cells
  11. Oxidation and reduction in chemical cells
  12. Oxidation and reduction in voltaic cell with a salt bridge
Number Laboratory Work 3.1
Pg. 67
Title Redox reaction as loss or gain of oxygen
Aim To investigate oxidation and reduction

  • A. Combustion of metal in oxygen
  • To investigate redox reaction in the combustion of metal in oxygen gas, O2
  • B. Heating of metal oxide with carbon
  • To investigate redox reaction in the heating of metal oxide with carbon
Problem Statement A. Combustion of metal in oxygen

  • In the reaction between metals in oxygen, which reagent undergoes oxidation and which reagent undergoes reduction?

B. Heating of metal oxide with carbon

  • In the reaction between metal oxide and carbon, which reagent undergoes oxidation and which reagent undergoes reduction?
Hypothesis A. Combustion of metal in oxygen

  • (I) Magnesium undergoes oxidation to form magnesium ion, Mg2+
  • (II) Oxygen gas undergoes reduction to form oxide ion, O2-

B. Heating of metal oxide with carbon

  • (I) Carbon undergoes oxidation to form carbon dioxide gas
  • (II) Copper(II) oxide, iron(III) oxide and lead(II) oxide undergo reduction to form copper, iron and lead respectively
Apparatus A. Combustion of metal in oxygen

  • A pair of tongs
  • Bunsen burner

B. Heating of metal oxide with carbon

  • Crucible
  • Pipe-clay triangle
  • Tripod stand
  • Bunsen burner
  • Spatula
Material A. Combustion of metal in oxygen

  • 5cm magnesium ribbon
  • Sandpaper
  • Gas jar containing oxygen

B. Heating of metal oxide with carbon

  • Carbon powder
  • Copper(II) oxide powder / Iron(III) oxide powder / Lead(II) oxide powder
Variables A. Combustion of metal in oxygen

  • Manipulated variable: Type of metal
  • Responding variable: Reaction product
  • Controlled / Fixed variable: Oxygen gas and the conditions of reaction

B. Heating of metal oxide with carbon

  • Manipulated variable: Type of metal oxide
  • Responding variable: Reaction product
  • Controlled / Fixed variable: Carbon and the conditions of reaction

.

Number Laboratory Work 3.2
Pg. 71
Title Change of iron(II) to iron(III) ions and vice versa
Aim To investigate oxidation and reduction in the change of iron(II) ions, Fe2+ to iron(III) ions, Fe3+ and vice versa (change of iron(III) ions, Fe3+ to iron(II) ions, Fe2+)
Apparatus
  • Dropper
  • Spatula
  • Test tube
  • Test tube holder
  • Test tube rack
  • Bunsen burner
  • Filter funnel
  • Measuring cylinder
Material
  • 0.5 mol dm-3 freshly prepared iron(II) sulphate, FeSO4 solution
  • 0.5 mol dm-3 iron(III) sulphate, Fe2(SO4)3 solution
  • Bromine water
  • Zinc powder
  • Filter paper (1 piece)
  • 2.0 mol dm-3 sodium hydroxide, NaOH solution
  • 0.5 mol dm-3 potassium hexacynoferrate(III), K3Fe(CN)6 solution

.

Number Laboratory Work 3.3
Pg. 73
Title Displacement of metals
Aim To investigate oxidation and reduction in the displacement of metals from their salt solutions
Problem Statement How does redox reaction occur in a displacement reaction in which a metal is displaced from its salt solution?
Hypothesis
  • (I) The metal that acts as a reducing agent will form metal ion
  • (II) The metal ion that acts as an oxidising agent will be precipated as metal
Apparatus
  • Test tubes
  • Test tube rack
Material
  • Zinc strip
  • Copper strip
  • Magnesium ribbon
  • 0.5 mol dm-3 silver nitrate
  • 0.5 mol dm-3 copper(II) sulphate
  • 0.5 mol dm-3 magnesium sulphate
Variables
  • Manipulated variable: A pair of metals and salt solutions
  • Responding variable: Precipitation of metal and colour changes in the solutions
  • Controlled / Fixed variable: Volumes and concentrations of solutions containing the metal ions

.

Number Laboratory Work 3.4
Pg. 74
Title Displacement of halogens
Aim To investigate oxidation and reduction in the displacement of halogen from its halide solution
Problem Statement How do redox reactions occur in displacement reactions between halogens and aqueous solutions of halide ions?
Hypothesis A more reactive halogen displace a less reactive halogen from an aqueous solutions of its halide ions
Apparatus
  • Test tubes
  • Test tube rack
Material
  • Chlorine water
  • Bromine water
  • Iodine water
  • 0.5 mol dm-3 potassium chlorine, KCl solution
  • 0.5 mol dm-3 potassium bromine, KBr solution
  • 0.5 mol dm-3 potassium iodine, KI solution
  • 1,1,1-tricholoethane, CH3CCl3
Variables
  • Manipulated variable: A pair of halogens and their halide ions
  • Responding variable: Changes in colour in 1,1,1-trichloroethane, CH3CCl3
  • Controlled / Fixed variable: Volume of reaction mixture

.

Number Laboratory Work 3.5
Pg. 77
Title Transfer of electrons at a distance
Aim To investigate oxidation and reduction in the transfer of electrons at a distance
Problem statement How do redox reactions occur in displacement reactions between halogens and aqueous solutions of halide ions?
Hypothesis A more reactive halogen displace a less reactive halogen from an aqueous solution of its halide ions
Apparatus
  • U-tube
  • Galvanometer
  • Connecting wire with crocodile clips
  • Graphite electrode
  • Retort stand and clamp
  • Test tube
  • Dropper / glass tube
  • Stopper with 1 hole
Material
  • 2.0 mol dm-3 sulphuric acid, H2SO4
  • 0.5 mol dm-3 freshly prepared iron(II) sulphate, FeSO4 solution
  • 0.2 mol dm-3 acidified potassium manganate(VII), KMnO4 solution
  • 0.5 mol dm-3 potassium iodide, KI solution
  • 0.2 mol dm-3 acidified potassium dichromate(VI), K2Cr2O7 solution
  • Bromine water
  • 0.2 mol dm-3 potassium thiocyanate, KSCN solution
  • 1% starch solution
Variables
  • Manipulated variable: A pair of halogen and their halide ions
  • Responding variable: Changes in colour in 1,1,1-trichloroethana, CH3CCl3
  • Controlled / Fixed variable: Volume of reaction mixture

.

Number Experiment 3.1
Pg. 81
Title Effect of other metals on rusting
Aim To investigate the effect of other metals on rusting
Problem Statement How do different types of metals in contact with iron affect rusting?
Hypothesis When a more electropositive metal is in contact with iron, the metal inhibits rusting. When a less electropositive metal is in contact with iron, the metal speeds up rusting
Apparatus
  • Test tube
  • Test tube rack
Material
  • Iron nail
  • Magnesium ribbon
  • Copper strip
  • Zinc strip
  • Tin strip
  • Hot jelly solution with a little potassium hexacyanoferrate(III), K3Fe(CN)6 solution and phenolphthalein
  • Sandpaper
Variables
  • Manipulated variable: Types of metals that are in contact with iron / Different types of metals
  • Responding variable: Presence of colouration / Intensity of dark blue colouration / Rusting of iron
  • Controlled / Fixed variable: Clean iron nails, medium in which the iron nails are kept / hot jelly solution, temperature
Operational Definition Blue colouration indicates rusting of iron

.

Number Laboratory Work 3.6
Pg. 85
Title Reactivity of metals with oxygen
Aim
  • (I) To investigate the reactivity of metals with oxygen
  • (II) To arrange metals in terms of their reactivity with oxygen
Problem Statement How do different types of metals react with oxygen?
Hypothesis The more reactive metal react more vigorously with oxygen
Apparatus
  • Boiling tube
  • Retort stand and clamp
  • Bunsen burner
  • Spatula
  • Forceps
Material
  • Magnesium powder
  • Copper powder
  • Iron filings
  • Lead powder
  • Zinc powder
  • Solid potassium manganate(VII), KMnO4
  • Asbestos paper
  • Glass wool
Variables
  • Manipulated variable: Different types of metals
  • Responding variable: the brightness of the flame
  • Controlled / Fixed variable: The amount of the metal and potassium manganate(VII) powder

.

Number Laboratory Work 3.7
Pg. 87
Title
  • A. The position of carbon in the reactivity series of metals with oxygen
  • B. Heating carbon dioxide with metals
Aim
  • A. To determine the position of carbon in the reactivity series of metals
  • B. To determine the ability of a metal to remove oxygen from carbon dioxide.
Problem Statement How is the position of carbon in the reactivity series of metals determined?
Hypothesis
  • (I) A reaction occur if carbon is more reactive than the metal
  • (II) A reaction not occur if carbon is less reactive than the metal
  • (III) Carbon is placed between aluminium and zinc in the reactivity series of metals
Apparatus A. The position of carbon in the reactivity series of metals with oxygen

  • Crucible / Porcelain dish / Asbestos paper
  • Spatula
  • Bunsen burner
  • Pipe-clay triangle
  • Tripod stand

B. Heating carbon dioxide with metals

  • Gas jar
  • Gas jar cover
  • A pair of tongs
Material A. The position of carbon in the reactivity series of metals with oxygen

  • Carbon powder
  • Solid copper(II) oxide, CuO
  • Solid magnesium oxide, MgO
  • Solid aluminium oxide, Al2O3
  • Solid zinc oxide, ZnO

B. Heating carbon dioxide with metals

  • Magnesium ribbon
  • Gas jar filled with carbon dioxide gas, CO2
  • Sandpaper
Variables A.

  • Manipulated variable: Type of metal oxide
  • Responding variable: Intensity of flame
  • Controlled / Fixed variable: Carbon powder

B.

  • Manipulated variable: Type of metal
  • Responding variable: Intensity of flame
  • Controlled / Fixed variable: Carbon dioxide gas and the conditions of reaction

.

Number Laboratory Work 3,8
Pg. 89
Title The position of hydrogen in the reactivity series of metals (Demonstration by teacher)
Aim To determine the position of hydrogen in the reactivity series of metals
Problem Statement How is the position of hydrogen in the reactivity series of metals determined?
Hypothesis Hydrogen is placed between zinc and iron in the reactivity series of metals
Apparatus
  • Combustion tube
  • Porcelain dish
  • Flat-bottomed flask
  • U-tube
  • Thistle funnel
  • Delivery tube
  • Bunsen burner
  • Retort stand and clamps
  • Stopper with 1 hole
  • Stopper with 2 holes
Material
  • 2.0 mol dm-3 sulphuric acid, H2SO4
  • 1.0 mol dm-3 copper(II) sulphate, CuSO4 solution
  • Zinc granules
  • Solid copper(II) oxide
  • Solid zinc oxide
  • Solid lead(II) oxide
  • Solid iron(III) oxide
  • Anhydrous calcium chloride
Variables
  • Manipulated variable: Different types of metal oxides
  • Responding variable: Intensity of flameControlled / Fixed variable: Hydrogen gas and the conditions of reaction

.

Number Laboratory Work 3.9
Pg. 95
Title Oxidation and reduction in electrolytic cells
Aim To investigate oxidation and reduction in electrolytic cellsA. Electrolytic cell involving molten electrolyteB. Electrolytic cell involving aqueous electrolyte
Apparatus A. Electrolytic cell involving molten electrolyte

  • Crucible
  • Cardboard
  • Battery
  • Connecting wire with crocodile clips
  • Tripod stand
  • Bunsen burner
  • Pipe-clay triangle
  • Carbon electrode
  • Switch
  • Ammeter
  • Light bulb
  • A pair of tongs
  • Spatula

B. Electrolytic cell involving aqueous electrolyte

  • Battery
  • Connecting wire with crocodile clips
  • Electrolytic cell
  • Carbon electrode
  • Switch
  • Ammeter
  • Light bulb
  • Small test tube
  • Beaker
  • A pair of tongs
Material A. Electrolytic cell involving molten electrolyte

  • Solid lead(II) bromide, PbBr2

B. Electrolytic cell involving aqueous electrolyte

  • 0.5 mol dm-3 potassium iodide, KI solution
  • Starch solution
  • Sandpaper
  • Wooden splinter

.

Number Laboratory Work 3.10
Pg. 97
Title Oxidation and reduction in chemical cells
Aim To investigate the oxidation and reduction in chemical cells
Apparatus
  • Porous pot
  • Voltmeter
  • Connecting wires with crocodile clips
  • Beaker
  • Measuring cylinder
Material
  • 1.0 mol dm-3 copper(II) sulphate, CuSO4 solution
  • 1.0 mol dm-3 zinc sulphate ZnSO4 solution
  • Copper strip
  • Zinc strip
  • Sandpaper

.

Number Laboratory Work 3.10 (Similar experiment)
Pg. 97
Title Oxidation and reduction in voltaic cell with a salt bridge
Aim To investigate the oxidation and reduction in chemical cells
Apparatus
  • Voltmeter
  • Connecting wires with crocodile clips
  • 100 cm3 beakers
  • Measuring cylinder
Material
  • 1.0 mol dm-3 copper(II) sulphate, CuSO4 solution
  • 1.0 mol dm-3 zinc sulphate ZnSO4 solution
  • 1.0 mol dm-3 lead(II) nitrate Pb(NO3)2 solution
  • 1.0 mol dm-3 iron(II) sulphate FeSO4 solution
  • Copper plate
  • Zinc plate
  • Lead plate
  • Iron nail
  • Sandpaper
  • Saturated potassium chloride, KCl solution
  • Filter paper strip

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