NITROGEN & ITS COMPOUNDS.

Haber process.

By the end of the lesson, the learner should be able to:
Identify raw materials for Haber process and how they are obtained in large scale.
Discuss the Haber process.
Represent Haber process in a schematic diagram.

Discussion and explanations.

Chart- schematic diagram.

K.L.B. BK III
PP. 159-160
225-226

NITROGEN & ITS COMPOUNDS.

Uses of ammonia.
Nitric acid. Lab preparation.
Nitric acid Industrial manufacture.

By the end of the lesson, the learner should be able to:
To list down uses of ammonia.
To list down nitrogenous fertilizers.
To describe lab preparation of nitric acid.
To describe industrial manufacture of nitric acid.

Teacher elucidates uses of ammonia and nitrogenous fertilizers.
Teacher demonstration.
Write equations of reaction.
Discussion.
Discussion and writing equations.

charts
Retort stand
Conc. H2SO4
KNO3
Chart
Schematic diagram.

K.L.B. BK III
P. 161

Longhorn
Book III
PP 126 -226

NITROGEN & ITS COMPOUNDS.

Reaction of dilute Nitric acid with metals.

By the end of the lesson, the learner should be able to:
To describe reaction of dilute nitric acid with metals.
To write equations of reactions of dilute nitric acid with metals.

Class experiment:- making observations and recording them in a table.
Discuss the observations.
Write down equations for the reactions.

Magnesium
Zinc
Copper

K.L.B. BK III
PP. 165-166

Longhorn
Book III
PP 166-8

NITROGEN & ITS COMPOUNDS.

Nitric acid and carbonates.
Reaction of dil. nitric acid with hydrogen carbonates.
Dilute nitric acid and metal hydroxides and oxides.
Reaction of nitric acid as an oxidizing agent.
Uses of nitric acid & nitrates.

By the end of the lesson, the learner should be able to:
To describe action of nitric acid on carbonates and hydrogen carbonates.
Write equations for reaction of dil. nitric acid with hydrogen carbonates.
Predict results of reacting dilute nitric acid with metal hydroxides and oxides.
Describe reactions of nitric acid as an oxidizing agent.
To state uses of nitrates.
To describe preparation of nitrates.

Group experiments: - Action of Nitric acid on hydrogen carbonates.
Discussion and corresponding equations.
Group experiments & writing equations for the reactions.
Class experiments: -
Explain observations made.
Discussion
Equations for the reactions for preparation of nitrates.

Solutions of
Na2CO3
NaHCO3
ZnCO3
CuCO3
Metal hydroxides.
Nitric acid acidified iron sulphate, sulphur, and copper metal.
charts

K.L.B. BK III
P. 167

Longhorn
Book III
229-30
K.L.B. BK III
PP. 169-170

Longhorn Book III
PP 239 -240

NITROGEN & ITS COMPOUNDS.

Action of heat on nitrates.

By the end of the lesson, the learner should be able to:
To write equations of decomposition of nitrates on heating.

Discuss above observations.
Write relevant equations.

charts

K.L.B. BK III
P 172

NITROGEN & ITS COMPOUNDS.
SULPHUR AND ITS COMPOUNDS

Test for nitrates.
Nitrogen compounds and the environment.
Extraction of sulphur.

By the end of the lesson, the learner should be able to:
To carry out tests on nitrates.
To explain the pollution of nitrogen compounds in the environment.
To state ways of reducing environmental pollution by nitrogen compounds.
To describe extraction of sulphur by Frasch process.

Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.
Brief guided discussion.
Illustrate and discuss extraction of sulphur.

charts
Chart-the Frasch process.

K.L.B. BK III
PP 173-174

Longhorn
Book III
PP 243

SULPHUR AND ITS COMPOUNDS

Allotropes of sulphur.
Physical properties of sulphur. Heating of sulphur.

By the end of the lesson, the learner should be able to:
To identify allotropes of sulphur.
To describe preparation of allotropes of sulphur.
To list physical properties of sulphur.
To describe effects of heat on sulphur.

Discussion and exposition of new concepts.
Class experiment:
Solubility of sulphur in water, benzene, e.t.c,.
Class experiments:
Heating sulphur gently then strongly.
Discuss the observations.

video
charts

K.L.B. BK III
PP. 182-183
Longhorn Book
PP 126-129

SULPHUR AND ITS COMPOUNDS

Chemical properties of sulphur.
Uses of sulphur. Sulphur dioxide.
Physical properties of sulphur dioxide.
Acidic properties of SO2.

By the end of the lesson, the learner should be able to:
To investigate and describe chemical properties of sulphur.
State uses of sulphur.
Describe lab. preparation of sulphur dioxide.
To list down physical properties of sulphur dioxide.
To carry out experiments to determine acidic properties of SO2.

Group experiments.
Discuss observations.
Write corresponding equations.
Teacher elucidates uses of sulphur.
Teacher demonstration:-
Preparation of sulphur dioxide in a fume chamber/in the open.
Carrying out tests on the gas.
Discuss the above tests.
Teacher demonstration to verify acidic properties of sulphur dioxide.
Write equations.

charts
text book
textbook

K.L.B.BK III
PP.188-190
Longhorn
Book III
PP 256-8

K.L.B.BK III
PP 193
Longhorn
Book III
PP 262-3

SULPHUR AND ITS COMPOUNDS

Reducing action of SO2.
Bleaching properties of SO2.
Oxidizing action of SO2.

By the end of the lesson, the learner should be able to:
To verify reducing action of SO2.
To carry out experiments to determine bleaching properties of SO2.
To explain Oxidizing action of SO2.

Class experiments: make observations and draw conclusions.
Write balanced corresponding equations.
Discuss the observations made above.
Write corresponding equations.
Q/A: review redox reactions.
Teacher demonstration: - Lowering magnesium into a jar of SO2; effect of SO2 on hydrogen sulphide.
Discuss observations.
Write equations for the reactions.

Experimental worksheets.
Burning magnesium.
Hydrogen sulphide.

K.L.B.BK III
P. 195

SULPHUR AND ITS COMPOUNDS

Sulphate and sulphite ions. Uses of SO2.
Sulphuric acid. Contact process of manufacture.
Properties of conc. H2SO4.
Physical properties of sulphuric acid.

By the end of the lesson, the learner should be able to:
To carry out tests for Sulphate and sulphite ions.

State uses of SO2.
To identify raw materials for manufacture of sulphuric acid.
To describe the contact process.
Describe properties of conc. H2SO4.
To dilute conc. sulphuric acid.
State physical properties of sulphuric acid.

Class experiments.
Make deductions from the observations made.
Write (ionic) equations for the reactions.
Teacher elucidates uses of SO2.

Discussion using schematic
flow charts.
Writing equations.
Discuss above observations.
Write relevant equations.
Teacher demonstration ? diluting conc. sulphuric acid.
Discuss use of conc. sulphuric acid as a drying and dehydrating agent.

Sodium sulphate
Barium chloride
Barium nitrate.
Chart-schematic
Flow charts.
charts
Conc. sulphuric acid.

K.L.B.
BK III P. 200
Longhorn
Book III
PP 268-9


K.L.B. BK III
PP.201-203
Longhorn
Book III
PP 275-6

SULPHUR AND ITS COMPOUNDS

Chemical properties of Sulphuric acid.
Dilute H2SO4, carbonates and hydrogen carbonates.

By the end of the lesson, the learner should be able to:
To write equations to show that conc. sulphuric acid is a drying and dehydrating agent.
To describe reactions of dilute H2SO4 with metals.
To describe reaction of dilute H2SO4 with carbonates and hydrogen carbonates.

Discussion and explanations.
Group expts. ? reaction of metals with dilute H2SO4, make observations and relevant deductions; writing corresponding equations.
Discussion, writing relevant equations.

Magnesium, zinc, copper metals.
charts

K.L.B.
BK III P. 206
Longhorn
Book III
PP 276-8

SULPHUR AND ITS COMPOUNDS

Dilute H2SO4, and metal oxides and hydroxides.
Dilute H2SO4 and metal oxides & hydroxides.

By the end of the lesson, the learner should be able to:
To investigate reaction of dilute H2SO4 with metal oxides and hydroxides.
To explain reactions of dilute H2SO4 with metal oxides and hydroxides.

Class expts.
Observing colour changes.
Discussion, writing relevant chemical equations.

Oxides of magnesium, zinc, copper.
NaOH Solution.
charts

K.L.B.
BK III P. 210
Longhorn
Book III
PP 287-8

SULPHUR AND ITS COMPOUNDS

Hydrogen sulphide. Preparation of the gas. Reaction of the gas with oxygen.

By the end of the lesson, the learner should be able to:
To describe preparation of hydrogen sulphide.
To state properties of the gas.

Theoretical / descriptive approach.
Writing corresponding equations.
Discuss physical properties of the gas and reaction of the gas with oxygen.

charts

K.L.B.
BK III P. 210
Longhorn
Book III
PP 289-90

SULPHUR AND ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS

Reaction of the gas with water. Reducing properties of the gas.
Sulphur and its effects on the environment.
Lab. preparation of chlorine gas.
Physical properties of chlorine.
Chemical properties of chlorine ? reaction with water.

By the end of the lesson, the learner should be able to:
To write equations for reaction of the gas with water.
To demonstrate reducing properties of the gas.
To explain environmental pollution caused by sulphur and its compounds.
Describe laboratory preparation of chlorine gas.
State physical properties of chlorine.
To investigate and explain reaction of chlorine with water.

Writing chemical equations for the reactions.
Discussion and explanation.
Teacher demonstration ? gas prep. tests on the gas.
Q/A: Relate the properties to the method of collection of the gas.
Write equations for the reaction leading to formation of chlorine.
Teacher demonstration:
Writing chemical equations.

charts
Conc. HCl, Manganese (IV) oxide.
charts
Moist blue litmus papers.

K.L.B.
BK III P. 212.
Longhorn
Book III
PP 291-2


K.L.B.BK III
P. 219
Longhorn
Book III
PP 298-9

CHLORINE & ITS COMPOUNDS

Chemical properties of chlorine - Reaction with metals - Reaction with non-metals.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with metals / non-metals.

Teacher demonstration:
Discussion.
Writing chemical equations.

textbook

K.L.B.BK III
PP.
224 -225
Longhorn
Book III
PP 303-5

CHLORINE & ITS COMPOUNDS

- Oxidizing properties of chlorine.
Chlorine and alkalis.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with reducing a gents.
To investigate and explain reaction of chlorine with alkalis.

Group experiments.
Discuss and explain observations made.
Write corresponding chemical equations.
Teacher demonstration: Bubbling chlorine with dilute cold / hot NaOH solution.
Make observations and account for them.

Expt. Worksheets.
Cold / hot NaOH solutions.

K.L.B. BK III
PP. 226 -227
Longhorn Book
PP 307-8

CHLORINE & ITS COMPOUNDS

Test for chlorides.
Uses of chlorine gas.

By the end of the lesson, the learner should be able to:
To carry out tests for chlorides.
To state uses of chlorine.

Class expts.
Discuss observations, results.
Write chemical equations for the reactions.
Teacher elucidates uses of chlorine.

Expt. Worksheets.
Zinc chloride, litmus paper, conc. Sulphuric acid.

K.L.B.BK III
P. 230
Longhorn Book III
PP 318-319

CHLORINE & ITS COMPOUNDS

Hydrogen chloride gas. Lab. prep. Physical properties.
Aqueous hydrogen chloride.
Further chemical properties of hydrogen chloride gas.

By the end of the lesson, the learner should be able to:
To describe Lab. prep of hydrogen chloride gas.
To investigate and state physical properties of hydrogen chloride gas.

To prepare aqueous hydrogen chloride.
To determine chemical properties of hydrogen chloride gas.
To carry out confirmatory test for hydrogen chloride gas.

Teacher demonstration.
Carry out tests on the gas and deduce the properties of the gas.

Class experiment leading to deduction of chemical properties of hydrogen chloride gas.
Class experiment leading to deduction of further chemical properties of hydrogen chloride gas / confirmatory test for hydrogen chloride gas.

Sodium chloride crystals, conc H2SO4
Distilled water.
Ammonia solution.

K.L.B.BK III
P. 232
Longhorn
Book III
PP 323-4


K.L.B.BK III
P. 234

CHLORINE & ITS COMPOUNDS

Large-scale production of hydrochloric acid.
Uses of hydrochloric acid.
Effects of hydrochloric acid on the environment.

By the end of the lesson, the learner should be able to:
Identify raw materials for manufacture of hydrochloric acid in large scale.
Describe the manufacturing process.
To state uses of hydrochloric acid.
To explain effects of hydrochloric acid on the environment.

Discussion and giving relevant equations.
Brief discussion.
Discussion and explanation.
Assignment.

charts

K.L.B.BK III
P. 237
Longhorn Book III
P 330

ACIDS, BASES AND SALTS.

Strength of acids. Acids in aqueous form.

By the end of the lesson, the learner should be able to:


Define an acid in terms of hydrogen ions.

Explain strength of acids in aqueous form in terms of number of hydrogen ions present.

Class experiments: investigate reactions of magnesium and zinc carbonate with different acids.
Make and record observations in tabular form.
Make deductions from the observations.
Write relevant chemical equations and ionic equations.
Detailed discussion leading to the definition of an acid and explanation of strength of an acid.

Magnesium strip, zinc carbonate,
2M HCl,
2M H2SO4,
2M ethanoic acid.

K.L.B. BK IV
Pages 1-4

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.
Definition of a base in terms of hydroxide ions.

By the end of the lesson, the learner should be able to:
Determine strength of acids using pH values.
Determine strengths of acids by comparing their electrical conductivities.
Classify acids as either strong or weak in terms of partial dissociations in aqueous solutions.
Define a base in terms of hydroxide ions.

Q/A: review determination of strength of acids using a litmus paper and pH scale.
Class / group experiments: record colour of universal indicator in
2M HCl and 2M ethanoic acid.
Set up voltameters of 2M HCl and 2M ethanoic acid in turns.
Record amounts of current .
Discuss the observations.
Write corresponding ionic equations.
Teacher demonstration:
Dissolve calcium hydroxide in water.
Carry out litmus test on the resulting solution.
Discuss the results; hence define a base in terms of hydroxide ions.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.
Red litmus paper, calcium hydroxide solid.

K.L.B. BK IV
Pages 4-6

ACIDS, BASES AND SALTS.

Neutralization reaction.
Strength of bases.
Dissolving hydrogen chloride gas in water / methylbenzene.
Dissolving ammonia gas in water/ methylbenzene.

By the end of the lesson, the learner should be able to:
Determine the results of reaction of an acid and a base.
Compare strengths of bases using pH values and electrical conductivity.
Classify bases/ alkali as either strong or weak in terms of complete / partial ionization.
Define a polar and a non-polar solvent.
Investigate effect of a polar / non-polar solvent on ammonia gas.

Add 1M HCl to an aqueous solution of Calcium hydroxide drop wise until colour, change of the universal indicator is noted.
Write ionic equation for the reaction.
Carry out pH tests of 2M NaOH and 2M ammonia solution using universal indicator solutions; and observe colour changes.
Carry out electrical conductivity tests of voltameters of the above solutions.
Discussion: relate number of hydroxide ions to pH values and electrical conductivity of bases.
Teacher demonstration:
Dissolving HCl gas in different solvents.
Discuss the observations.
Write down related balanced chemical equations.
Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.

1M HCl,
Calcium hydroxide,
universal indicator.
2M NaOH,
2M ammonia solution, universal indicator solutions, dry cells,
carbon electrodes,
milliammeters,
wires, switches etc
Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.

K.L.B. BK IV
Page 7
K.L.B. BK IV
Pages 9-11

ACIDS, BASES AND SALTS.

Amphoteric oxides.

By the end of the lesson, the learner should be able to:
Define an amphoteric oxide.
Identify some amphoteric oxides.

Class experiment:
Carry out acid / base reactions with metal oxides.
Q/A: make deductions from the results.
Writing and balancing relevant equations.

2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 12-14

ACIDS, BASES AND SALTS.

Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.
Equations for formation of insoluble chlorides, sulphites and sulphates.
Complex ions.

By the end of the lesson, the learner should be able to:
Define a precipitate.
Write ionic equations showing formation of precipitates.
Find out cations that form (in)soluble chlorides, sulphates and sulphites.
Write down equations for formation of insoluble chlorides, sulphites and sulphates.
Explain formation of complex ions.

Q/A: review definition of a salt.
Class experiment;
Add sodium carbonate or a suitable carbonate to various salt solutions containing Mg2+, Al3+, Ca2+, etc.
Make observations and discuss the results.
Class experiments: measure 2cc of 0.1M solution containing Pb2+ into a test tube.
Add drops of 2M NaCl solution.
(Later 2M Sodium Sulphate and 2M Sodium Sulphate).
Warm the mixture and make observations.
Repeat the procedure using other salt solutions containing other ions.
Tabulate the results.
Q/A: review observations made in the above experiments.
Discuss the solubility of the cations.
Write relevant ionic equations.
Add drops of 2M sodium hydroxide / 2M ammonia solution to a solution containing Mg2+, Zn2+, etc.

Make observations and discuss the results.

Soluble carbonates e.g. Na2CO3, K2CO3, (NH4)2CO3
Salt solutions containing Mg2+, Al3+, Ca2+, etc.
0.1M solution containing Pb2+, 2M NaCl solution, 2M sodium sulphate, source of heating.
student book
2M Sodium hydroxide (2M ammonia solution),
solution containing Mg2+, Zn2+, etc.

K.L.B. BK IV
Pages 14-16
K.L.B. BK IV
Pages 18-20

ACIDS, BASES AND SALTS.

Solubility of a salt at a given temperature.
Problems solving on solubility.

By the end of the lesson, the learner should be able to:
Define the term solubility.
Determine solubility of a given salt at room temperature.
Solve problems involving solubility of a solute in a solvent at a given temperature.

Q/A: review the terms saturated, unsaturated solutions & crystallization.
Class experiment: determine mass of a solute that dissolves in 100cc of water at room temperature.
Worked examples.
Supervised practice.
Written assignment.

Suitable solutes.
Evaporating dish, watch glass, heating source, thermometer.

K.L.B. BK IV
Pages 20-21

ACIDS, BASES AND SALTS.

Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.

By the end of the lesson, the learner should be able to:
Investigate the effect of temperature on solubility of a solute in a solvent.
Determine the effects of various salts on soap.

Experiments involving solubility of KClO3 at different temperatures.
Note temperatures at which crystallization occurs.
Oral questions and discussion.
Group experiments: form soap lather in distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
Note volume of soap that forms lather readily.

KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.

K.L.B. BK IV
Pages 22-25

ACIDS, BASES AND SALTS.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Removal of hardness of water.
Endothermic and Exothermic Reactions.
Energy level diagrams.

By the end of the lesson, the learner should be able to:
Identify ions for hardness of water.
Identify methods of removing hardness of water.
State merits & demerits of hard water.
To differentiate between endothermic & exothermic reactions.
Represent endothermic reactions with exothermic reactions with energy level diagrams.

Review results of above experiments.
Probing questions & brief discussion.
Assignment.
Investigate temperature changes in solution formation.
Obtain changes in temperature when ammonium nitrate and sodium hydroxide are dissolved in water, one at a time.
Probing questions on relative energies of reactants and products in endothermic and exothermic and endothermic reactions.

student book
Ammonium nitrate,
Sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 27-29

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.
CAT
Molar heat of solution.

By the end of the lesson, the learner should be able to:
Define the term enthalpy.
Distinguish positive enthalpy change from negative enthalpy change.

Determine the M.P/ B.P of a pure substance.

Determine molar heat of solution of given substances.

Q/A and brief discussion.
Class experiments: determine B.P of pure water/ M.P of naphthalene / ice.
Use experimental results to plot temperature-time graphs.
Explain the shape of the graphs.
Q/A: review kinetic theory of matter.
Apply the theory to explain the shape of the graph, and nature of bonding in substances.


Dissolve known masses of ammonia nitrate / sodium hydroxide in known volumes of water.
Determine temperature changes.
Calculate molar heat of solution. Supervised practice.

Ice, naphthalene, thermometers, graph papers.
Ammonia nitrate / sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 35-39

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of H2SO4.

By the end of the lesson, the learner should be able to:
Determine molar heat of solution of H2SO4.

Dissolve some known volume of conc. H2SO4 in a given volume of water.
Note the change in temperature.
Work out the molar heat of solution of H2SO4.

Conc. H2SO4, thermometers.

K.L.B. BK IV
Pages 42-45

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.

By the end of the lesson, the learner should be able to:
Define the term enthalpy of combustion.
Determine the enthalpy of combustion of ethanol.
Explain why actual heats of combustion are usually lower than the theoretical values.

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.

Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.

K.L.B. BK IV
Pages 45-48

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of displacement of ions.
Molar heat of solution of neutralization.

By the end of the lesson, the learner should be able to:
Define the term molar heat of solution of displacement of ions.
Determine the molar heat of solution of displacement of ions.
Define the term neutralization.
Determine the molar heat of neutralization of HCl with NaOH.

Group experiments/ teacher demonstration.
Note steady temperature of solutions formed when zinc/ iron / magnesium reacts with copper sulphate solution.
Work out the molar heat of displacement of a substance from a solution of its ions.
Class experiments:
Neutralize 2M HCl of known volume with a determined volume of 1M / 2M sodium hydroxide.
Note highest temperature of the solution.
Work out the molar heat of neutralization.
Solve other related problems.
Assignment.

Zinc, iron, magnesium, copper sulphate solution.
2M HCl of known volume, 1M / 2M sodium hydroxide.

K.L.B. BK IV
Pages 48-50

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Standard enthalpy changes.
Hess?s Law.
Heat of solution hydration energy and lattice energy.

By the end of the lesson, the learner should be able to:
Define the term standard enthalpy change.
Denote standard enthalpy change with the correct notation.
State Hess?s law.
Solve problems related to Hess?s law.
Define the terms lattice energy and hydration energy.
Explain the relationship between heat of solution, hydration energy.
Solve related problems.

Exposition & brief discussion.
Detailed discussion & guided discovery of the law.
Illustrations of energy cycles and energy levels leading to Hess?s law.
Worked examples.
Supervised practice
Written assignment.
Exposition of new concepts.
Guided discovery of the relationship between heat solution hydration energy and lattice energy.
Worked examples.
Assignment.

student book

K.L.B. BK IV
Pages 54-56
K.L.B. BK IV
Pages 60-64

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
RATES OF REACTION & REVERSIBLE REACTIONS.
RATES OF REACTION & REVERSIBLE REACTIONS.

Heat values of fuels.
Environmental effects of fuels.
Effect of concentration on rate of a reaction
Effect of time of reaction on the rate of reaction.

By the end of the lesson, the learner should be able to:
Define the term fuel.
Describe energy changes when a fuel undergoes combustion.
Outline factors considered when choosing a suitable fuel.
Outline some environmental effects of fuels.
Identify measures taken to reduce environmental
pollution.
Explain the effects of change of concentration of reactants on a reaction.
Explain how the rate or reaction changes as the reaction proceed

Probing questions and brief discussion.
Q/A & open discussion.
Group experiments to investigate effect of concentration on rate of reaction using dil. HCl and magnesium ribbons.
Determine the time taken for reactions to be complete.
Calculation of concentration of HCl in moles per litre.
Discuss the observations and sketch illustrative graphs.
Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl.
Collect evolved gas and sketch and illustrative graphs.
Discuss the results.

student book
Portions of 2M HCl diluted with different volumes of water,
Stopwatches.
Magnesium ribbons, stopwatches, conical flask.
100cm3 0.5M HCl, syringes, stoppers, tubes and connectors.

K.L.B. BK IV
Pages 64-66