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Energy and Equilibria
Lesson outline
Lesson Content
EE1
EE3
4.10, 4.11 &
4.12
P8687
How do you calculate the heat energy (molar
enthalpy) of a combustion reaction?
Know that copper calorimeters are used to measure the
temperature change of water as a fuel is used to heat it
Know how to set up an experiment for investigating the
combustion of alcohols
Calculate heat energy for combustion reactions, i.e. heating
water with alcohol spirit burners
Calculate molar enthalpy for combustion reactions
4.11 & 4.12
P8687
How do you represent enthalpy changes that occur
during a chemical reaction?
Know that ΔH (molar enthalpy) is negative for exothermic and
positive for endothermic reactions
Draw simple energy level diagrams to represent the change in
enthalpy of exothermic and endothermic reactions
Recall that the breaking of bonds is endothermic and that the
making of bonds is exothermic
Calculate the molar enthalpy of simple chemical reactions
using average bond energies
EE4
Page
refs.
How does temperature change during exothermic
and endothermic reactions?
Recall that exothermic reactions give out heat and that
endothermic reactions take in heat
Recall the equation used to calculate heat energy- q=mcT
Know that foam calorimeters are used to measure temperature
changes for displacement, dissolving and neutralisation
reactions
Calculate heat energy for these types of reactions
Know that molar enthalpy is used to represent the change
in energy of a reaction, per mole of limiting reagent
Recall the equation used to calculate H=q / n
Calculate molar enthalpy for the above reactions
EE2
Key
Assess
-ment
Syllabus
statements
4.13, 4.14,
4.15 & 4.16
P8687
What are reversible reactions?
Recall that some reactions are irreversible and can only go in
the forward direction
Recall that some reactions are reversible and are indicated by
the symbol  in equations
Know that heating hydration copper(II) sulfate will remove the
water and that adding water will reverse the reaction
Know that heating ammonium chloride will cause it to reform
in a cooler area of the test tube
TTS iGCSE CHEMISTRY
4.22 & 4.23
P110
-111
Folder
E/G/A/N
Energy and Equilibria
EE5
What is dynamic equilibrium?
Define dynamic equilibrium as both the forward and backward
reactions taking place at the same time, but the concentrations
of reactant and products remaining constant.
Know that an increase in pressure will favour the side with less
gas particles for a reaction at equilibrium
Know that an increase in temperature will favour the direction
which takes in heat (endothermic) for a reaction at equilibrium
Know that an increase in concentration of reactants will favour
the forward reaction (towards the products) for a reaction at
equilibrium
EE6
P112
-113
5.21, 5.22,
5.23 & 5.24
P198
-199
How can you make ammonia on an industrial
scale?
Recall that nitrogen from air, and hydrogen from natural gas or
the cracking of hydrocarbons, are used in the manufacture of
ammonia
Know that for the manufacture of ammonia by the Haber
process, the essential conditions are: i) a temperature of about
450°C ii) a pressure of about 200 atmospheres iii) an iron
catalyst
Discuss the economic reasons for choosing such conditions
Know that the cooling of the reaction mixture liquefies the
ammonia produced and allows the unused hydrogen and
nitrogen to be recirculated
Recall the use of ammonia in the manufacture of nitric acid and
fertilisers
EE7
EE8
4.24 & 4.25
Revision
Test
Folder checklist
All lessons present / titled with lesson code / dated / in correct order
Tables drawn with pencil / ruler / column headings correct
Diagrams drawn with pencil / ruler
Graphs have axis labels / correct scales / title
All homeworks completed
Topic keywords spelt correctly
Strengths
Targets
TTS iGCSE CHEMISTRY
E/G/A/N