iGCSE Scheme of Work
Year 10
Sept 2012
Equilibrium
Lesson
Lesson 1
Reversible
reactions
Learning
Objectives
understand that
some reactions are
reversible and are
indicated by the
symbol ⇌ in
equations
describe reversible
reactions such as
the dehydration of
hydrated copper(II)
sulfate and the
effect of heat on
ammonium chloride
Activities
Assessment Safety
 Starter-Write the one-way reaction and the
reversible reaction equations on the board.
 Ask pupils to comment on differences
between the two.
MAIN
 Students practical on reversible reaction, see
worksheet. Heat ammonium chloride and
copper sulphate in separate test tubes.
 Show students the Animation C3 3.6
‘Reversible energy’ from Additional Science
CD ROM
 Pupils make notes from board including change
in rates of forward and reverse reactions to
equilibrium.
 Homework
 :Eye
Ask students to
find one further
example of an
equilibrium
reaction and
write a word
and symbol
equation to
represent it.
protection
should be
worn at all
times. As
acidic
hydrogen
chloride
gas and
alkaline
ammonia
gas are
produced,
the mineral
plug must
be used
and the
reaction
should be
carried out
in a well ventilated
room.
Ammonium
chloride is
harmful –
CLEAPSS
Hazcard 9
 Plenary
True or false – Pupils use ‘show me boards to
answer questions.’
All chemical reactions are reversible. [False]
A closed system has no mass change. [True]
Equilibrium can only happen in closed systems. [True]
A double-headed arrow in an equation shows that it is
a non-reversible reaction. [False]
In a reversible reaction, reactants make products and
products make reactants. [True]
Show powerpoint.
(5 minutes)
Needs a
more
rigorous
homework
Other
emphasis
iGCSE Scheme of Work
Year 10
Sept 2012
Equilibrium
Lesson
Lesson 2
Endothermic
and
exothermic
Learning
Objectives
understand that
chemical reactions in
which heat energy is
given out are
described as exothermic
and those in which heat
energy is taken in are
endothermic
Activities

Starter- Use a Bunsen burner to discuss the
energy exchanges occurring between the reaction
and the surroundings. Discuss this and the
opposite possibility and the terms exothermic and
endothermic reactions.

Practical
Pupils use coffee cup calorimeter as described on
sheet. Do this for zinc/copper sulphate and
endothermic expt. .

Notes Pupils write notes on endo/exo. They need
to understand the relationship with reversible
reactions.

Plenary- Use e-science ppt presentation
Assessment Safety
Students could
list one
exothermic
reaction and
one
endothermic
reaction that
they could not
live without and
state why
A more
rigorous
homework is
needed here
Other
emphasis
iGCSE Scheme of Work
Year 10
Sept 2012
Equilibrium
Lesson
Learning
Objectives
Activities
Assessment Safety

STARTER
 Video – Show RSC video about the industrial
production of ammonia. Use focus sheets.
Homework –
Fritz Haber
worksheet
Lesson 3
Making
Ammonia

understand that
nitrogen from air,
and hydrogen from
natural gas or the
cracking of
hydrocarbons, are
used in the
manufacture of
ammonia
describe the
manufacture of
ammonia by the
Haber process,
including the
essential conditions:
i a temperature of
about
450°C
ii a pressure of
about 200
atmospheres
iii an iron catalyst

understand how the
cooling of the
reaction mixture
liquefies the
ammonia produced
and allows the
unused hydrogen and
nitrogen to be
recirculated
MAIN
 Introduce the production of ammonia and the
benefits to society of ammonia and its compounds.
 Give pupils notes on the Haber process including
equations and state conditions for all processes.
 Show students the Simulation C2 3.7 ‘Making
Ammonia’ and allow them to explore the resource if
possible.
 Pupils to use their book and the e-science video to
complete the Haber process flow chart.
PLENARY
 Questions and answers – Give each student a slip
of paper (about A5 size). Ask them to write a
question and its answer on the paper about the
Haber process and reversible reactions, cut each
answer free from the question and give them to
you. Now give a question and answer to each
student but they should not match. Read the first
question out, the student with the correct answer
should read it out, then read their question and so
on.
Other
emphasis
iGCSE Scheme of Work
Year 10
Sept 2012
Equilibrium
Lesson
Learning
Objectives
Activities
Assessment Safety

Starter
Needs exam
question
H/W
Lesson 4
More about
the Haber
process,

Conditions for
equilibrium.

understand the
concept of dynamic
equilibrium
predict the effects of
changing the
pressure and
temperature on the
equilibrium position
in reversible
reactions.

True or false questions about the Haber process could use show me boards.
 The t/f questions are on e-science ppt, C2 5.3
Main
 Give the students data for the yield of the Haber
process at different temperatures and different
pressures. Students could then plot two graphs to
show the trend in yield as these variables change.
Higher attaining students could have two x-axis scales
describe the
and plot onto one graph. They could then be
manufacture of
encouraged to use the graphs to make conclusions
ammonia by the
Haber process,
about how temperature and pressure affects this
including the
reaction. Students could then be encouraged to
essential conditions:
explain these trends using information from the
Student Book, related to their earlier work on energy
i a temperature of
changes in reactions.
about
This could be in groups, who then present their work
450°C
or as individual Q + A.
ii a pressure of
about 200
atmospheres
iii an iron catalyst
describe the use of
ammonia in the
manufacture of nitric
acid and fertilisers
Discuss and makes notes on uses of ammonia
Plenary
C2 5.3 activity sheet: The yield in the Haber process.
Other
emphasis
iGCSE Scheme of Work
Year 10
Sept 2012
Equilibrium
Lesson
Lesson 5
Learning
Objectives
Activities
Test Old AQA test is fine here
Assessment Safety
Other
emphasis