67149845 biology form 5 experiment list

Chapter 1 – Rate of Reactions

List of PEKA experiments:

1. Average rate of reaction and instantaneous rate of reaction

2. Effect of surface area on the rate of reaction

3. Effect of concentration on the rate of reaction

4. Effect of temperature on the rate of reaction

5. Effect of catalyst on the rate of reaction

6. Effect of the amount of catalyst on the rate of reactionNumber Laboratory Work 1.2

Pg. 3

Title Average rate of reaction and instantaneous rate of reaction

Aim To determine the average rate of reaction and the instantaneous rate of reaction

Apparatus 50 cm3 beaker Test tube Spatula

Material Marble chip 2.0 mol dm-3 hydrochloric acid (HCl) 0.1 mol dm-3 sodium thiosulphate, Na2S2O3solution 1.0 mol dm-3 lead(II) nitrate solution

.

Number Experiment 1.1

Pg. 6

Title Effect of surface area on the rate of reaction

Aim To investigate the effect of total surface area of the reactant on the rate of reaction

Problem Statement

How does the total exposed surface area of a solid reactant affect the rate of reaction?

Hypothesis When the total surface area of marble chips increases, the rate of reaction increases. / The smaller the size of the reactant particles, that is, the larger the total surface area of the reactant particles, the higher the rate of reaction.

Apparatus 50 cm3 measuring cylinder 150 cm3 conical flask Stopper with delivery tube Basin Burette Spatula Electronic balance

Stopwatch

Material 0.5 mol dm-3 hydrochloric acid (HCl) 2 g large marble chips 2 g small marble chips Water

Variables Manipulated variable: Total surface area of marble chips Responding variable: Rate of reaction Controlled / Fixed variable: Mass of marble chips, volume and

concentration of hydrochloric acid (HCl), temperature

Operational Definition

1. Smaller marble chips have a larger total surface area than larger marble chips of the same mass.

2. For the graph of the volume of gas released against time, the curve with higher initial gradient indicates a higher initial rate of reaction.

.


Pg. 10

Title Effect of concentration on the rate of reaction

Aim To investigate the effect of concentration on the rate of reaction

Problem Statement

How does the concentration of a reactant affect the rate of reaction? / Does high concentration of sodium thiosulphate Na2S2O3 solution decrease the time taken for the mark ‘X’ to disappear from sight?

Hypothesis When the concentration of sodium thiosulphate, Na2S2O3 solution increases, the rate of reaction increases. / The higher the concentration of sodium thiosulphate Na2S2O3 solution, the shorter the time taken for the mark ‘X’ to disappear from sight.

Apparatus 150 cm3 conical flask 50 cm3 measuring cylinder 10 cm3 measuring cylinder Stopwatch

Material 0.2 mol dm-3 sodium thiosulphate solution 1.0 mol dm-3 sulphuric acid Distilled water White paper marked ‘X’ at the centre

Variables Manipulated variable: Concentration of sodium thiosulphate, Na2S2O3 solution

Responding variable: Rate of reaction Controlled / Fixed variable: Concentration, volume and initial

temperature of sulphuric acid, H2SO4. Total volume of reactants


Rate of reaction is inversely proportional to the time taken for the the mark ‘X’ to disappear from sight

.


Pg. 13

Title Effect of temperature on the rate of reaction

Aim To investigate the effect of temperature on the rate of reaction

Problem Statement

How does temperature affect the rate of reaction?

Hypothesis An increase in temperature will increase the rate of reaction.

Apparatus 150 cm3 conical flask 50 cm3 measuring cylinder 10 cm3 measuring cylinder Stopwatch Thermometer Bunsen burner Tripod stand Wire gauze

Material 0.2 mol dm-3 sodium thiosulphate solution 1.0 mol dm-3 sulphuric acid White paper marked ‘X’ at the centre

Variables Manipulated variable: Temperature of sodium thiosulphate, Na2S2O3 solution

Responding variable: The time taken for the cross ‘X’ to disappear Controlled / Fixed variable: volume and concentration of sodium

thiosulphate Na2S2O3solution, volume and concentration of sulphuric acid, size of conical flask


Rate of reaction is inversely proportional to the time taken for the mark ‘X’ to disappear from sight

.


Pg. 15

Title Effect of catalyst on the rate of reaction

Aim To investigate the effect of a catalyst on the rate of reaction

Problem Statement

How does a catalyst affect the rate of reaction? / How do catalysts affect the rate of decomposition of hydrogen peroxide?

Hypothesis The presence of a catalyst increases the rate of reaction. / Manganese(IV) oxide increases the rate of decomposition of hydrogen peroxide.

Apparatus Test tube Test tube rack Spatula Wooden splinter Retort stand and clamp 10 cm3 measuring cylinder Electronic balance Weighing bottle

Material 20-volume hydrogen peroxide, H2O2 solution 1.0 g Manganese(IV) oxide powder

Variables Manipulated variable: Presence or absence of a catalyst Responding variable: The release of oxygen gas / Rate of reaction Controlled / Fixed variable: Volume and concentration of hydrogen

peroxide (H2O2) solution, temperature


The decomposition of hydrogen peroxide is fast if the glowing wooden splinter rekindles brightly and rapidly.

The decomposition of hydrogen peroxide is slow if the glowing wooden splinter glows dimly and slowly.

.


Pg. 17

Title Effect of the amount of catalyst on the rate of reaction

Aim To investigate the effect of the amount of catalyst on the rate of reaction.

Problem Statement

How does the amount of a catalyst affect the rate of reaction? / Does higher amount of catalysts increases the rate of reaction?

Hypothesis When the amount of a catalyst used increases, the rate of reaction increases. / The higher the amount of the catalysts, the higher the rate of reaction.

Apparatus 50 cm3 measuring cylinder 150 cm3 conical flask Stopper with delivery tube Burette Retort stand and clamp Basin Stopwatch Electronic balance Spatula Weighing bottle Beakers

Material 2-volume hydrogen peroxide solution 1.0 g manganese(IV) oxide powder

Variables Manipulated variable: amount / mass of catalyst Responding variable: Rate of reaction Controlled / Fixed variable: Temperature, volume and concentration of

hydrogen peroxide solution


The curves for the graph of volume of gas liberated against time a higher gradient indicated a higher rate of reaction.

Chapter 3 – Oxidation and Reduction


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

13.

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 burnerB. 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 oxygenB. 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 reactionB. 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

.


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)3solution 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

.


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

.


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

.


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

.


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


Blue colouration indicates rusting of iron

.


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

.


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 standB. 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, ZnOB. 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 powderB.

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

.


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 SpatulaB. 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

.


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

Chapter 4 – Thermochemistry


1. Exothermic and endothermic reactions

2. Heat of precipitation

3. Heat of displacement

4. Heat of neutralisation

5. Heat of neutralisation of acids and alkalis of different strength

6. Heat of neutralisation

7. Heats of combustion for alcoholsNumber Laboratory Work 4.1

Pg. 101

Title Exothermic and endothermic reactions

Aim To identify an exothermic or endothermic reaction

Problem Statement

How to identify exothermic or endothermic reactions?

Hypothesis Exothermic reaction occurs when the temperature of the reaction mixture increases.Endothermic reaction occurs when the temperature of the reaction mixture decreases.

Apparatus Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Spatula Glass rod 50 cm3 measuring cylinder

Material Solid sodium hydrogen carbonate, NaHCO3

Solid sodium hydroxide, NaOH Solid ammonium chloride, NH4Cl Solid ammonium nitrate, NH4NO3

Solid ammonium sulphate, (NH4)2SO4

2.0 mol dm-3 hydrochloric acid, HCl Distilled water

Variables Manipulated variable: Pairs of reactants Responding variable: The temperature change in the reaction mixture Controlled / Fixed variable: Types of container, volume of solution or

water

===============================================


Pg. 104

Title Heat of precipitation

Aim To determine the heat of precipitation of silver chloride, AgCl

Apparatus Plastic cup with cover / Polystyrene cup 0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder

Material 0.5 mol dm-3 silver nitrate solution 0.5 mol dm-3 sodium chloride solution

===============================================


Pg. 106

Title Heat of displacement

Aim To determine the heat of displacement of copper

Apparatus Plastic cup with cover / Polystyrene cup

0 – 110˚C thermometer Glass rod 50 cm3 measuring cylinder

Material 0.5 mol dm-3 copper(II) sulphate solution Zinc power

===============================================


Pg. 108

Title Heat of neutralisation

Aim To determine the heats of neutralisation between strong acids and strong alkalis


Material 2.0 mol dm-3 hydrochloric acid, HCl 2.0 mol dm-3 sodium hydroxide, NaOH solution 2.0 mol dm-3 nitric acid, HNO3

2.0 mol dm-3 potassium hydroxide, KOH solution

===============================================


Pg. 109

Title Heat of neutralisation of acids and alkalis of different strength

Aim To determine and compare the heats of neutralisation between acids and alkalis of different strength

Problem Statement

How do the heat of neutralisation for reactions between acids and alkalis of different strength?

Hypothesis The values of heat of neutralisation for reactions between strong acids and strong alkalis are higher than that of reactions between strong acids and weak alkalis / weak acids and strong alkalis or weak acids and weak alkalis.


Material 2.0 mol dm-3 ethanoic acid, CH3COOH 2.0 mol dm-3 hydrochloric acid, HCl 2.0 mol dm-3 sodium hydroxide, NaOH solution 2.0 mol dm-3 ammonia, NH3 solution

Variables Manipulated variable: Different strength of acids and alkalis Responding variable: The value of heat of neutralisation Controlled / Fixed variable: Volume and concentration of acids used,

volume and concentration of alkalis used.

===============================================


Pg. 110

Title Heat of neutralisation

Aim To determine and compare the heats of neutralisation between: Hydrochloric acid (strong acid), HCl and sodium hydroxide (strong

base), NaOH solution Ethanoic acid (weak acid), CH3COOH and sodium hydroxide (strong

base), NaOH solution Hydrochloric acid (strong acid), HCl and ammonia (weak base),

NH3 solution Ethanoic acid (weak acid), CH3COOH and ammonia(weak base),

NH3 solution

Problem Statement

How are the heats of neutralisation determined and compared?

Hypothesis The heat of neutralisation between hydrochloric acid and sodium hydroxide is higher than the heat of neutralisation between ethanoic acid and ammonia solution.

Apparatus 50 cm3 burette 25.0 cm3 pipette Pipette filler Retort stand and clamps Plastic cup / Polystyrene cup 250 cm3 beaker Magnetic stirrer Magnetic stir bar Temperature sensor Computer Computer interface Stopwatch

Material 1.0 mol dm-3 hydrochloric acid, HCl 1.0 mol dm-3 sodium hydroxide, NaOH solution 1.0 mol dm-3 ethanoic acid, CH3COOH 1.0 mol dm-3 ammonia, NH3 solution

Variables Manipulated variable: Different types of acids and bases Responding variable: Heat of neutralisation Controlled / Fixed variable: Volume and concentration of acid and alkali

used

===============================================


Pg. 112

Title Heats of combustion for alcohols

Aim To determine the heats of combustion for alcohols

Problem Statement

Does alcohol with a higher number of carbon atoms per molecule have a higher heat of combustion?

Hypothesis The higher the number of carbon atoms in the alcohol molecules, the higher is the heat of combustion.

Apparatus Copper can Thermometer Glass rod / Stirrer Measuring cylinder Tripod stand Spirit lamp Wooden block Weighing balance Wind shield / Asbestos screen

Material Methanol Ethanol Propanol / Prop-1-ol Butanol / But-1-ol Water

Variables Manipulated variable: Different types of alcohols Responding variable: Heat of combustion of alcohol Controlled / Fixed variable: Volume of water and copper can / metal

container (calorimeter)

Chapter 5 – Chemicals for Consumers


1. Soap preparation processNumber Laboratory Work 5.1

Pg. 117

Title Soap preparation process

Aim To prepare soap using the saponification process

Apparatus 250 cm3 beakers 50 cm3 measuring cylinder Spatula Glass rod Filter funnel Wire gauze Tripod stand Bunsen burner Wash bottle Test tube

Material Palm oil 5.0 mol dm-3 sodium hydroxide, NaOH solution Sodium chloride powder Filter paper (3 pieces)

Distilled water

67149845 biology form 5 experiment list

Documents