2C
Copy the title
Task C1
Equations
P7
Match the word
symbol and
balanced
equations
For each reaction
identify the
reactants and
products
Explain what s l g
mean
Identify the number and types of
atoms in balanced chemical equations
Word equation:
Magnesium +
oxygen 
magnesium oxide
Word equation:
Hydrogen +
nitrogen 
ammonia
Word equation:
Sodium + chlorine
 sodium chloride
Word equation:
Carbon + oxygen
 carbon dioxide
Symbol equation:
Mg(s) + O2(g) 
MgO (s)
Balanced equation:
2Mg(s) + O2(g) 
2MgO (s)
Symbol equation:
H2(g) + N2 (g) 
NH3(s)
Balanced equation:
2H2 (g) + 3N2 (g)
 2NH3 (g)
Symbol equation:
Na (s) + Cl2 (g)
NaCl (s)
Balanced equation:
2Na (s) + Cl2 (g)
2NaCl (s)
Symbol equation: C
(s) + O2 (g) CO2
Word equation:
Magnesium +
oxygen 
magnesium oxide
Word equation:
Hydrogen +
nitrogen 
ammonia
Word equation:
Magnesium +
oxygen 
magnesium oxide
Word equation:
Hydrogen +
nitrogen 
ammonia
Word equation:
Sodium + chlorine
 sodium chloride
Word equation:
Carbon + oxygen
 carbon dioxide
Word equation:
Sodium + chlorine
 sodium chloride
Word equation:
Carbon + oxygen
 carbon dioxide
Symbol equation:
Mg(s) + O2(g) 
MgO (s)
Balanced equation:
2Mg(s) + O2(g) 
2MgO (s)
Symbol equation:
Mg(s) + O2(g) 
MgO (s)
Balanced equation:
2Mg(s) + O2(g) 
2MgO (s)
Symbol equation:
H2(g) + N2 (g) 
NH3(s)
Balanced equation:
2H2 (g) + 3N2 (g)
 2NH3 (g)
Symbol equation:
H2(g) + N2 (g) 
NH3(s)
Balanced equation:
2H2 (g) + 3N2 (g)
 2NH3 (g)
Symbol equation:
Na (s) + Cl2 (g)
NaCl (s)
Balanced equation:
2Na (s) + Cl2 (g)
2NaCl (s)
Symbol equation:
Na (s) + Cl2 (g)
NaCl (s)
Balanced equation:
2Na (s) + Cl2 (g)
2NaCl (s)
Symbol equation: C
(s) + O2 (g) CO2
Symbol equation: C
(s) + O2 (g) CO2
In a chemical reaction,
reactants usually react to form products
reactants
products
In a reversible reaction, the products
of the reactant can react to produce the
original reactants
reactants
products
The symbol below represents a
reversible reaction
reactants
products
Heating copper sulphate - What happened?
• Hydrated copper sulphate is blue.
• When it is heated it turns into anhydrous copper sulphate (white)
• When this is left to cool it turns back into hydrated copper sulphate.
• The reverse reaction is used as a test for water. When water is added
to anhydrous copper sulphate 2 things happen:
1.) White solid turns blue
2.) Reaction gives out heat.
(Takes in) Heat
Endothermic
Hydrated Copper
Sulphate
(Blue Solid)
(Cool + Steam)
Exothermic
Anhydrous Copper
Sulphate
(White Solid)
P7
Explain what irreversible
and reversible reactions are
1. What is a
reversible
reaction?
2. Draw the symbol
that represents
reversible
reactions:
3. What happens to
blue hydrated
copper sulphate
when it is heated?
4. What happens to
anhydrous copper
sulphate when it is
left to cool and a
little water is
added?
5. What type of
reaction is this?
Types of reactionsreversible or irreversible
Types of reactions- neutralisation
P7
Explain what a
neutralisation
reaction is
Give an example
Write the word
and symbol
equation
•
•
•
•
•
Draw a diagram and explain what a neutralisation
reaction is
Explain if it is reversible or irreversible
Write down the word equation
Copy the symbol equation below and explain
everything that it tells us
H2SO4 (aq) + 2NaOH (aq)  Na2SO4 (aq) + 2H20 (l)
P7
Explain what the
reactivity series
is
Types of reactions- displacement
• Draw the diagram above
• Explain which is the most reactive and
which is the least reactive
P7
Explain what
displacement is
using your
knowledge of the
reactivity series
•
•
•
•
Types of reactions- displacement
Draw a before and after diagram
Explain what happens in this displacement reaction
Explain if it is reversible or irreversible
Copy down the word and symbol equation below
– Fe(s) + CuSO4(aq) --> FeSO4(aq) + Cu(s)
P7
Explain what
displacement is
using your
knowledge of the
reactivity series
Types of reactions- displacement
• Draw a before and after diagram
• Explain what happens in this displacement
reaction
• Explain if it is reversible or irreversible
Displacement experiment
Magnesium
Magnesium Sulphate
Iron Sulphate
Zinc Sulphate
Copper
Sulphate
Iron
Zinc
Copper
Copy the title
Task C2
Equations
C.2
Reaction rates:
a.
Effect of catalysts (lowering the energy needed for a reaction to
occur), surface area, concentration and temperature on rate of
reaction
b.
Use of reaction rate graphs
c.
Collision theory
Factors affecting the rate of a
reaction
P6
Using the
following slides
fill in the
summary sheet
The collision
theory
Explanation of what the collision theory is
Factor
How it affects the rate of
reaction
Temperature
High temperature
diagram
Low temperature diagram
Concentration
High concentration
diagram
Low concentration
diagram
Pressure
High pressure diagram
Low pressure diagram
Surface area
Small surface area:
Volume
Large surface area:
Volume
Catalyst
Diagram of activation energy with and without a
catalyst
The collision theory
Explanation of what the collision theory is
Factor
How it affects the rate of reaction
Temperature
High temperature diagram
Low temperature diagram
Concentration
High concentration diagram
Low concentration diagram
Pressure
High pressure diagram
Low pressure diagram
Surface area
Small surface area: Volume
Large surface area: Volume
Catalyst
Diagram of activation energy with and without a catalyst
Temperature
Changing temperature
Low temp
•
•
•
•
Less energy
Particles move slowly
Less collisions
Slow rate of reaction
high temp
• More energy
• Particles move faster
• More frequent
successful collisions
• faster rate of reaction
Changing temperature
Graphs
Increasing the temperature increases the speed of the reacting particles so
that they collide more frequently and more energetically.
This increases the rate of reaction
Changing temperature Summary
Concentration
Magnesium and hydrochloric acid
Changing concentration
Increasing the concentration of reactants in solutions increases the
frequency of collisions and so increases the rate of reaction.
Low conc
• Less frequent
collisions
• Slower rate of
reaction
High conc
• More frequent
successful collisions
• Faster rate of reaction
Changing concentration
Pressure
Effect of pressure on rate of reaction
As the pressure increases, the space in which the
gas particles are moving becomes smaller.
The gas particles become closer together, increasing the
frequency of collisions.
This means that the particles are more likely to react.
lower pressure
higher pressure
Surface area
Changing surface area
Increasing the surface area of solid reactants increases the frequency of
collisions and so increases the rate of reaction.
Changing surface area
Catalysts
What are catalysts?
Catalysts are substances that change the rate of a
reaction without being used up in the reaction.
energy (kJ)
Catalysts never produce more product – they just
produce the same amount more quickly.
Ea without
catalyst
Different catalysts work
in different ways, but
most lower the reaction’s
activation energy (Ea).
Ea with
catalyst
reaction (time)
P6
Copy the graph and explain
what it shows
A rate of reaction
graph
P6
Explain why the rat graph
curves
A rate of reaction
graph
Copy the title
Task C3
Industrial processes
M5
Answer the questions in
full sentences
Rates and industryMargarine
Margarine is made in food factories from vegetable oils. Hydrogen gas is
bubbled through the liquid oil. When the hydrogen reacts with the liquid
vegetable oil it hardens to form a solid fat. This process is hydrogenation.
At room temperature there is no reaction and hydrogenation doesn’t happen.
But the rate of reaction can be increased by using:
• A nickel catalyst (lowers activation energy and speeds up the reaction)
• A temperature of 175-190C (which increased the number of successful
collisions)
• A high pressure (which increases the number of successful collisions)
The higher the temperature, pressure and catalyst increase the rate of reaction
1.
2.
3.
4.
What raw product is used to make margarine?
What happens when hydrogen is bubbled through he liquid oil?
What 3 factors can increase the rate of reaction?
Explain how each of these factors increases the rate of reaction
M5
Answer the questions in
full sentences
Rates and industryMaking smells
The chemical Methanol CH3OH is used to make a compound that smells like apple
and pineapple.
The way that Methanol is made is below
Carbon monoxide + Hydrogen  methanol
CO (g) + 2H2 (g)  CH3OH (l)
The rate of reaction can be increased by
• Increasing the temperature to 250 C (this increases the chance of successful
collisions)
• A pressure of 50-100 atmospheres (this forces the reactants to collide more often
as they are pushed closer together)
• Using a catalyst made from copper zinc oxide and aluminium oxide (this lowers
the activation energy and increases the rate of reaction)
1. Why is methanol useful?
2. Write down the word and symbol equations. And explain which one are
reactants and products
3. What happens when hydrogen is bubbled through he liquid oil?
4. What 3 factors can increase the rate of reaction?
5. Explain how each of these factors increases the rate of reaction
M5
Answer the questions in
full sentences
Rates and industry- The
HABER PROCESS for
producing AMMONIA
The production of ammonia is a very important process as it is used to
make fertilizers to grow more food crops.
The Haber Process
H
is a reversible
N
reaction where
Ammonia is made from:
H
H
both reactants and
N
N
• nitrogen, which is removed from the air
the product are
• hydrogen, made from methane (natural gas) H H GASES.
•To give the best yeild of ammonia a temperature of 450°C and a
pressure of 200 atmospheres is used.
1.
2.
3.
4.
What is the formula for ammonia?
Why is ammonia important?
What are the 2 reactants for making ammonia?
What are the 2 conditions to make the most amount of ammonia?
HYDROGEN &
NITROGEN
IN
hydrogen +
nitrogen
ammonia
HYDROGEN
NITROGEN
AMMONIA
TEMPERATURE
and PRESSURE of
the reaction
vessel can be
controlled
UNUSED
HYDROGEN &
NITROGEN
RECYCLED
% YIELD =
% AMMONIA in
main reaction
vessel
M5
Copy the diagram
LIQUID
AMMONIA
REMOVED
Mixture cooled here.
AMMONIA
condenses
M6
Copy the 2 key words
down
Key definitions
Yield –
• The amount of product made in the
reaction
Atom economy –
• A way of measuring the amount of
atoms in the reactants that become
useful products