ibdp chemistry chapter name Rate of reaction.ppt

RATES OF
RATES OF
REACTION - 1
REACTION - 1
A guide for A level students
A guide for A level students
2015
2015
SPECIFICATIONS
SPECIFICATIONS
KNOCKHARDY PUBLISHING
T1
T2
T3
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

INTRODUCTION
This Powerpoint show is one of several produced to help students understand
selected topics at AS and A2 level Chemistry. It is based on the requirements of
the AQA and OCR specifications but is suitable for other examination boards.
Individual students may use the material at home for revision purposes or it
may be used for classroom teaching if an interactive white board is available.
Accompanying notes on this, and the full range of AS and A2 topics, are
available from the KNOCKHARDY SCIENCE WEBSITE at...
www.knockhardy.org.uk/sci.htm
Navigation is achieved by...
either clicking on the grey arrows at the foot of each page
or using the left and right arrow keys on the keyboard
RATES OF REACTION
RATES OF REACTION

RATES OF REACTION
RATES OF REACTION
CONTENTS
• Prior knowledge
• Collision Theory
• Methods for increasing rate
• Surface area
• Temperature
• Catalysts
• Light
• Pressure
• Concentration
• Check list

Before you start it would be helpful to…
• know how the energy changes during a chemical reaction
• know the basic ideas of Kinetic Theory
• know the importance of catalysts in industrial chemistry
RATES OF REACTION
RATES OF REACTION

CHEMICAL KINETICS
CHEMICAL KINETICS
Introduction
Chemical kinetics is concerned with the dynamics of chemical reactions
such as the way reactions take place and the rate (speed) of the process.
One can look at the QUALITATIVE and the QUANTITATIVE aspects of how
the rate (speed) of a reaction can be changed.
Chemical kinetics plays an important part in industrial chemistry because
the time taken for a reaction to take place and the energy required are of
great economic importance. The kinetic aspect of chemistry is often at
odds with the thermodynamic side when considering the best conditions
for industrial production.
The concepts met in this topic can be applied throughout the theoretical
and practical aspects of chemistry.
The basis of the study is COLLISION THEORY
COLLISION THEORY...

COLLISION THEORY
COLLISION THEORY
Collision theory states that...
• particles must COLLIDE before a reaction can take place
• not all collisions lead to a reaction
• reactants must possess at least a minimum amount of energy – ACTIVATION
ENERGY
plus
• particles must approach each other in a certain relative way - STERIC
EFFECT

COLLISION THEORY
COLLISION THEORY
Collision theory states that...
• particles must COLLIDE before a reaction can take place
• not all collisions lead to a reaction
• reactants must possess at least a minimum amount of energy – ACTIVATION
ENERGY
plus
• particles must approach each other in a certain relative way - STERIC
EFFECT
According to collision theory, to increase the rate of reaction you need...
more frequent collisions increase particle speed or
have more particles present
more successful collisions give particles more energy or
lower the activation energy

INCREASING THE RATE
INCREASING THE RATE
• INCREASE THE SURFACE AREA OF SOLIDS
• INCREASE TEMPERATURE
• SHINE LIGHT
• ADD A CATALYST
• INCREASE THE PRESSURE OF ANY GASES
• INCREASE THE CONCENTRATION OF REACTANTS
The following methods may be used to
increase the rate of a chemical reaction

INCREASING SURFACE AREA
INCREASING SURFACE AREA
• Increases chances of a collision - more particles are exposed
• Powdered solids react quicker than larger lumps
• Catalysts (e.g. in catalytic converters) are finely divided for this reason
+
In many organic reactions there are two liquid layers, one aqueous, the other
non-aqueous. Shaking the mixture increases the reaction rate as an
emulsion is often formed and the area of the boundary layers is increased
giving more collisions.
CUT THE SHAPE
INTO SMALLER
PIECES
1
3
1
SURFACE AREA
9+9+3+3+3+3 = 30 sq units
SURFACE AREA
9 x (1+1+1+1+1+1) = 54 sq units
1
1
1
3

Effect increasing the temperature increases the rate of a reaction
particles get more energy so can overcome the energy barrier
particle speeds also increase so collisions are more frequent
INCREASING TEMPERATURE
ENERGY CHANGES
DURING A REACTION
As a reaction takes place the enthalpy of
the system rises to a maximum, then falls
A minimum amount of energy is required to
overcome the ACTIVATION ENERGY (Ea).
Only those reactants with energy equal to,
or greater than, this value will react.
If more energy is given to the reactants then
they are more likely to react.
Typical energy profile diagram
for an exothermic reaction

According to KINETIC THEORY, all particles must have energy; the greater their
temperature, the more energy they possess. The greater their KINETIC ENERGY the
faster they travel.
ZARTMANN heated tin in an oven and directed the gaseous atoms at a rotating disc
with a slit in it. Any atoms which went through the slit hit the second disc and solidified
on it. Zartmann found that the deposit was spread out and was not the same thickness
throughout.
This proved that there was a spread of velocities and the distribution was uneven.
ZARTMANN’S
EXPERIMENT

Experiments showed that, due to the many collisions taking place between
molecules, there is a spread of molecular energies and velocities.
no particles have zero energy/velocity
some have very low and some have very high energies/velocities
most have intermediate velocities.
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

Increasing the temperature alters the distribution
• get a shift to higher energies/velocities
• curve gets broader and flatter due to the greater spread of values
• area under curve stays constant - corresponds to the total number of particles
T1
T2
TEMPERATURE
T2 > T1
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

Decreasing the temperature alters the distribution
• get a shift to lower energies/velocities
• curve gets narrower and more pointed due to the smaller spread of values
• area under curve stays constant
T1
T3
TEMPERATURE
T1 > T3
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

REVIEW
no particles have zero energy/velocity
some particles have very low and some have very high energies/velocities
most have intermediate velocities
as the temperature increases the curves flatten, broaden and shift to higher energies
T1
T2
T3
TEMPERATURE
T2 > T1 > T3
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

Ea
ACTIVATION ENERGY - Ea
The Activation Energy is the minimum energy required for a reaction to take place
The area under the curve beyond Ea corresponds to the number of molecules with
sufficient energy to overcome the energy barrier and react.
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
NUMBER OF
MOLECULES WITH
SUFFICIENT
ENERGY TO
OVERCOME THE
ENERGY BARRIER
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

Explanation
increasing the temperature gives more particles an energy greater than Ea
more reactants are able to overcome the energy barrier and form products
a small rise in temperature can lead to a large increase in rate
T1
T2
TEMPERATURE
T2 > T1
Ea
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY
EXTRA
MOLECULES WITH
SUFFICIENT
ENERGY TO
OVERCOME THE
ENERGY BARRIER

• Catalysts provide an alternative reaction pathway with a lower Activation Energy (Ea)
• Decreasing the Activation Energy means that more particles will have sufficient
energy to overcome the energy barrier and react
• Catalysts remain chemically unchanged at the end of the reaction.
ADDING A CATALYST
ADDING A CATALYST
WITHOUT A CATALYST WITH A CATALYST

If a catalyst is added, the Activation Energy is lowered - Ea will move to the left.
MOLECULAR ENERGY Ea
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
NUMBER OF
MOLECULES WITH
SUFFICIENT
ENERGY TO
OVERCOME THE
ENERGY BARRIER
ADDING A CATALYST
ADDING A CATALYST
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

Lowering the Activation Energy, Ea, results in a greater area under the curve after Ea
showing that more molecules have energies in excess of the Activation Energy
Ea
MAXWELL-BOLTZMANN
DISTRIBUTION OF
MOLECULAR ENERGY
ADDING A CATALYST
ADDING A CATALYST
EXTRA MOLECULES
WITH SUFFICIENT
ENERGY TO OVERCOME
THE ENERGY BARRIER
MOLECULAR ENERGY
NUMBER
OF
MOLECUES
WITH
A
PARTICULAR
ENERGY

• work by providing an alternative reaction pathway with a lower Activation Energy
• using catalysts avoids the need to supply extra heat - safer and cheaper
• catalysts remain chemically unchanged at the end of the reaction.
Types Homogeneous Catalysts Heterogeneous Catalysts
same phase as reactantsdifferent phase to reactants
e.g. CFC’s and ozone e.g. Fe in Haber process
CATALYSTS -
CATALYSTS - A REVIEW
A REVIEW

• work by providing an alternative reaction pathway with a lower Activation Energy
• using catalysts avoids the need to supply extra heat - safer and cheaper
• catalysts remain chemically unchanged at the end of the reaction.
Types Homogeneous Catalysts Heterogeneous Catalysts
same phase as reactantsdifferent phase to reactants
e.g. CFC’s and ozone e.g. Fe in Haber process
CATALYSTS DO NOT AFFECT THE POSITION OF ANY EQUILIBRIUM
• but they do affect the rate at which equilibrium is attained
• a lot is spent on research into more effective catalysts - the savings can be dramatic
• catalysts need to be changed regularly as they get ‘poisoned’ by other chemicals
• catalysts are used in a finely divided state to increase the surface area
CATALYSTS -
CATALYSTS - A REVIEW
A REVIEW

Catalysts are widely used in industry because they…
CATALYSTS -
CATALYSTS - WHY USE THEM?
WHY USE THEM?

allow reactions to take place at lower temperatures SAVE ENERGY (lower Ea)
REDUCE CO2 OUTPUT
CATALYSTS -
WHY USE THEM?

REDUCE CO2 OUTPUT
enable different reactions to be used BETTER ATOM ECONOMY
REDUCE WASTE
CATALYSTS -
WHY USE THEM?

REDUCE CO2 OUTPUT
REDUCE WASTE
are often enzymes GENERATE SPECIFIC PRODUCTS
OPERATE EFFECTIVELY AT ROOM TEMPERATURES
CATALYSTS -
WHY USE THEM?

REDUCE CO2 OUTPUT
REDUCE WASTE
have great economic importance in the industrial production of POLY(ETHENE)
SULPHURIC ACID
AMMONIA
ETHANOL
CATALYSTS -
WHY USE THEM?

REDUCE CO2 OUTPUT
REDUCE WASTE
have great economic importance in the industrial production of POLY(ETHENE)
SULPHURIC ACID
AMMONIA
ETHANOL
can reduce pollution CATALYTIC CONVERTERS
CATALYSTS -
WHY USE THEM?

• shining a suitable light source onto some reactants increases the rate of reaction
• the light - often U.V. - provides energy to break bonds and initiate a reaction
• the greater the intensity of the light, the greater the effect
Examples a) the reaction between methane and chlorine - see alkanes
b) the darkening of silver salts - as used in photography
c) the reaction between hydrogen and chlorine
Equation H2(g) + Cl2(g) ———> 2HCl(g)
Bond enthalpies H-H 436 kJ mol-1
Cl-Cl 242 kJ mol-1
Mechanism Cl2 ——> 2Cl• - - - - - INITIATION
H2 + Cl• ——> HCl + H• - - - - - PROPAGATION
H• + Cl2 ——> HCl + Cl•
2Cl• ——> Cl2 - - - - - TERMINATION
2H• ——> H2
H• + Cl• ——> HCl
SHINING LIGHT
SHINING LIGHT
certain reactions only

• increasing the pressure forces gas particles closer together
• this increases the frequency of collisions so the reaction rate increases
• many industrial processes occur at high pressure to increase the rate... but
it can adversely affect the position of equilibrium and yield
The more particles there are in a given volume, the greater the pressure
The greater the pressure, the more frequent the collisions
The more frequent the collisions, the greater the chance of a reaction
INCREASING THE PRESSURE
INCREASING THE PRESSURE

Increasing concentration = more frequent collisions = increased rate of reaction
INCREASING CONCENTRATION
INCREASING CONCENTRATION
However, increasing the concentration of some reactants
can have a greater effect than increasing others
Low concentration = fewer collisions Higher concentration = more collisions

Reactions are fastest at the start and get slower as the reactants concentration drops.
In a reaction such as A + 2B ——> C the concentrations might change as shown
RATE CHANGE DURING A REACTION
RATE CHANGE DURING A REACTION
Reactants (A and B)
Concentration decreases with time
Product (C)
Concentration increases with time
• the steeper the curve the faster the
rate of the reaction
• reactions start off quickly because
of the greater likelihood of collisions
• reactions slow down with time as
there are fewer reactants to collide TIME
CONCENTRATION
B A
C

Experimental Investigation
• the variation in concentration of a reactant or product is followed with time
• the method depends on the reaction type and the properties of reactants/products
e.g. Extracting a sample from the reaction mixture and analysing it by titration.
- this is often used if an acid is one of the reactants or products
Using a colorimeter or UV / visible spectrophotometer.
Measuring the volume of gas evolved.
Measuring the change in conductivity.
More details of these and other methods can be found in suitable text-books.
MEASURING THE RATE
MEASURING THE RATE

RATE How much concentration changes with time. It is the equivalent of velocity.
MEASURING THE RATE
MEASURING THE RATE
y
CONCENTRATION
gradient = y
x
x
TIME
• the rate of change of concentration is found from the slope (gradient) of the curve
• the slope at the start of the reaction will give the INITIAL RATE
• the slope gets less (showing the rate is slowing down) as the reaction proceeds
THE SLOPE OF THE GRADIENT OF THE
CURVE GETS LESS AS THE
REACTION SLOWS DOWN
WITH TIME

REVISION CHECK
REVISION CHECK
What should you be able to do?
Recall and understand the statements in Collision Theory
Know six ways to increase the rate of reaction
Explain qualitatively how each way increases the rate of reaction
Understand how the Distribution of Molecular Energies is used to explain rate increase
Understand how the importance of Activation Energy
Recall and understand how a catalyst works by altering the Activation Energy
Explain how the rate changes during a chemical reaction
CAN YOU DO ALL OF THESE?
CAN YOU DO ALL OF THESE? YES
YES NO
NO

You need to go over the
You need to go over the
relevant topic(s) again
relevant topic(s) again
Click on the button to
Click on the button to
return to the menu
return to the menu

WELL DONE!
WELL DONE!
Try some past paper questions
Try some past paper questions

ibdp chemistry chapter name Rate of reaction.ppt

More Related Content

Similar to ibdp chemistry chapter name Rate of reaction.ppt (20)

More from Ankit mistry (7)

Recently uploaded (20)

ibdp chemistry chapter name Rate of reaction.ppt