The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. Rate of reaction is affected by several factors including surface area, concentration, temperature, catalysts and pressure (for gas reactions). The collision theory is also explained, stating that reactions only occur during effective collisions where particles attain sufficient kinetic energy to overcome the activation energy barrier. Examples of how scientific understanding of rate of reaction enhances quality of life through applications like food storage, cooking and petroleum processing are provided.

1. CHAPTER 1
RATE OF REACTION

2. Contents
1.1 Understanding of Rate of Reaction
1.2 Factors Affecting Rate of Reaction
1.3 Collision Theory
1.4 Scientific Knowledge to Enhance Quality
of Life

3. 1.1 Understanding of Rate of Reaction
 Rate of reaction is defined as the change in the amount
of reactants or products per unit time.
 We usually use water displacement method to collect
gas in school laboratory as shown below:

4. Method of Gas Collection Using a Gas
Syringe System

5. • The reaction is fastest at the start when the reactants are
at a maximum (steepest gradient)
• The gradient becomes progressively less as reactants
are used up and the reaction slows down.
• Finally the graph levels out when one of the reactants is
used up and the reaction stops.
• The amount of product depends on the amount of
reactants used.
• The initial rate of reaction is obtained by measuring the
gradient at the start of the reaction. A tangent line is
drawn to measure rate of reaction at instantaneous time.

6.  Different chemical reactions occur at different rates.
• Fast Reaction
• Slow Reaction
Fast Reaction Slow Reaction
The time taken for a fast reaction is
short.
The time taken for a slow reaction is
long.
The rate of reaction is said to be
high.
The rate of reaction for a slow
reaction is low.
Example:
•Fading of dyes on a shirt under hot
sun
•Cooking a chicken using a
microwave oven
•Burning of petrol in a car engine
•Striking a match
•Ripening of tomatoes
Example:
•A piece of newspaper turning yellow
•The weathering of limestone by acid
rain
•Rusting of a water pipe

7. Fast Reaction

8. Slow Reaction

9. Observable changes for measuring rate of reaction

10. Finding Average Rate Of Reaction

11. Example:
In a chemical reaction, 2.5g of calcium carbonate react
completely with excess hydrochloric acid to produce
600cm³ of carbon dioxide gas in 1.5 minutes. Find the rate
of reaction in term of
a. decreasing mass of calcium carbonate
b. increasing volume of carbon dioxide gas produced
Answer:

12. Finding Average Rate Of Reaction From
Measurable Quantities
 During a chemical reaction, two things happen
1. The quantities of reactants reduce.
2. The quantities of products increase.
 Therefore, the rate of the reaction can be determined by
• measuring the decrease of the amount of the reactants over
time.
• measuring the increase of the amount of the products over time.
 However, the quantity (or change) of the
reactants/product may be measurable or immeasurable.
 The easily measured quantity changes include
• Mass
• Concentration (Conductivity)
• Volume of gas

14. Example:
In a reaction, 5 g of calcium carbonate takes 250 seconds to
completely react with solution of hydrochloric acid. Calculate the
average rate for this reaction in units
a.g s-1
and
b.mol s-1
[ Relative atomic mass: C 12; O, 16; Ca, 40]
Answer:

15. Finding Average Rate Of Reaction From
Immeasurable Quantities

16. Example:
When the aqueous of ethanadioic is mixed with acided potassium
manganate(VII) , the reaction happen slowly at room temperature. The
purple colour of the solution is bleached after 20 seconds. Calculate
the average rate of reaction.
Answer:

17. Analysing Rate of Reaction from Graph
Graph Of Product/Reactant Change Against Time
In a chemical reaction,
• the reactants will decrease over time
• the product will increase over time
the rate of reaction will decrease over time owing to the
decrease in concentration and total surface area of
reactants.
In a graph of quantity of product/reactant over time, the
rate of reaction is equal to the gradient of the graph.

18. Example:
The reaction between dilute hydrochloric acid and excess
marble will produce calcium chloride and gas of carbon
dioxide. Sketch the graph of
1. the mass of the marble against time.
2. the volume of carbon dioxide against time.
3. the concentration of hydrochloric acid against time.
4. the concentration of calcium chloride against time.
Answer:
1.

19. 2.
3. 4.

20. Finding The Average Rate Of Reaction From A Graph
Example:
In a reaction between calcium carbonate and liquid hydrochloric acid,
carbon dioxide gas that is released is collected in a burette. The
graph shows the volume of carbon dioxide collected over time. Find
the average rate of reaction in the first 60s.

21. Answer:
https://www.youtube.com/watch?v=knAjEa4-0KM

22. Finding Instantaneous Rate Of Reaction From A Graph
 The rate of reaction changes from time to time as the
reaction happens.
 The rate of reaction at a particular time is called the
instantaneous rate.
 The instantaneous rate of a reaction is equal to the
gradient of tangent at a particular time.

23. Example:
The graph shows the volume of carbon dioxide gas
released over time in a chemical reaction. Find the
rate of reaction at t = 40s

24. Answer:

25. 1.2 Factors Affecting Rate of Reaction

26. 1. Size of Solid Reactants/Total Surface Area
The smaller the size of the particle, the bigger
the total surface area.
The bigger the total surface area, the higher the
rate of reaction.

27. Experiment 1
25 cm3
of 0.5 mol dm–3
hydrochloric acid + calcium carbonate chips. The
carbon dioxide gas released is collected in a burrete. The volume of
the gas released is recorded in every 30s. The result is plotted in a
graph.

28. Experiment 2
25 cm3
of 0.5 mol dm–3
hydrochloric acid + calcium carbonate powder.
As in experiment 1, the carbon dioxide gas released is collected in a
burrete and the volume of the gas released is recorded in every 30s.
The result is plotted in the same graph in experiment 1.

29. Conclusion
• The gradient of the curve for experiment 2 is greater than the curve for
experiment 1. This indicate that the rate of reaction in experiment 2 is
higher than experiment 1.
• We can conclude that, the smaller the particle size of the reactant, the
bigger the total surface area, and the bigger the total surface area, the
higher the rate of the reaction will be.

30. 2. Concentration Of Reactants
Experiment
By measuring the time taken for the formation of sulphur
precipitate (yellow solid) when sulphuric acid, H2SO4 reacts
with sodium thiosulphate(VI), Na2S2O3 of different
concentration , we can investigate the effect of
concentration of the reactant on the rate of reaction.
 The higher the concentration of the solution, the higher
the rate of reaction.

31. Procedure:
•50 cm3
of 0.2 mol dm-3
sodium thiosulphate solution + 10 cm3
of 0.5 mol
dm-3
sulphuric acid.
•
from view is recorded.
•The experiment is repeated by using sodium thiosulphate solution with
concentration 0.4 mol dm-3
, 0.6 mol dm-3
, 0.8 mol dm-3
and 1.0 mol dm-3
.

32. Conclusion 1:
•The graph for concentration of sodium thiosulphate (VI), Na2S2O3 against
time taken for the sulphur precipitate to formed is plotted.
•As the concentration of sodium thiosulphate solution decreases, the

33. Conclusion 2:
•The graph for concentration of sodium thiosulphate (VI),
Na2S203 against 1/time taken is plotted.
•As the concentration of sodium thiosulphate increases, the value of
1/time increases. We should note that 1/time = rate of reaction.
•The higher the concentration of sodium thiosulphate solution, the
higher the rate of reaction.

34. 3. Temperature Of The Reactant
Experiment
By measuring the time taken for the formation of sulphur
precipitate (yellow solid) when sulphuric acid, H2SO4 reacts
with sodium thiosulphate(VI), Na2S2O3 of different
temperature, we can investigate the effect of temperature
of the reactant on the rate of reaction.
The higher the temperature of the
solution, the higher the rate of reaction.

35. Procedure:
•50 cm3
of 0.2 mol dm-3
sodium thiosulphate solution at 30ºC + 10 cm3
of
0.5 mol dm-3
sulphuric acid.
•
from view is recorded.
•The experiment is repeated by using sodium thiosulphate solution with
temperature 35ºC, 40ºC, 45ºC and 50ºC.

36. Conclusion 1:
• The graph for temperature of sodium thiosulphate (VI),
Na2S2O3 against time taken for the sulphur precipitate to formed is
plotted.
• As the temperature of sodium thiosulphate solution decreases, the

37. Conclusion 2:
• The graph for temperature of sodium thiosulphate (VI),
Na2S203 against 1/time taken is plotted.
• As the temperature of sodium thiosulphate increases, the value of
1/time increases. We should note that 1/time = rate of reaction.
• The higher the temperature of sodium thiosulphate solution, the
higher the rate of reaction .

38. Pressure Of Gas
 For reactions involve gas, the rate of reaction is affected
by the pressure of the gas.
 Pressure DOES NOT affect the rate of reaction where
the reactants are in the form of solids or liquids.
 The higher the pressure of the gas, the higher the rate of
reaction
The higher the pressure of the gas, the higher
the rate of reaction

39. 4. Catalyst
 Catalyst is a chemical substance that change the rate of
chemical reaction
 Characteristics of catalyst:
Catalyst
Only a small amount of catalyst is
needed to increases the rate of
reaction. An increase in the
quantity of catalyst will increase
the rate of reaction but only a very
slight increase
During a reaction, catalyst remains
chemically unchanged but may
undergo physical changes. For
example, catalyst may turn into
powder during the reaction
Alters the rate of
reaction
Does not change the
quantity of products formed
It is specific in its action. It can
only catalyse a particular
reaction

40. Catalysts provide a different reaction path with a low activation energy

41. List of Reactions and the Catalyst
Chemical Reaction Catalyst
Decomposition of hydrogen peroxide:
2H2O2 → 2H2O + O2
Manganese(IV) oxide, MnO2
Lead(II) oxide, PbO
Lead(IV) oxide, PbO2
Reaction between Zinc and
Hydrochloric Acid:
Zn + 2HCl → ZnCl2 + H2
Manganese (IV) oxide, MnO2
Copper (II) oxide, CuO
Zinc Oxide, ZnO
Silicon (IV) oxide, SiO2
Decomposition of Potassium Chlorate
(V):
2KClO3 + 2KCl → 3O2
Copper (II) sulphate, CuSO4
Copper (II) chloride, CuCl2
Copper (II) nitrate, Cu(NO3)2
Haber Process
N2 + 3H2 → 2NH3
Iron
Contact Process
2SO2 + O2 → 2SO Vanadium(V) oxide, V2O5
Ostwald Process
4NH3(g) + 5O2(g) 4NO(g) + 6H2O(1)
Platinum

42. Factors Affecting Catalyst
A catalyst is a substance which can
change the rate of reaction.
There are 2 types of catalyst:
• Positive catalyst – Increase the rate of
reaction.
• Negative catalyst – Reduce the rate of
reaction.

43. Copper(II) sulphate acts as a catalyst to increase the rate of reaction between
zinc and hydrochloric acid
Conclusion
The presence of catalyst increases the rate of reaction.

44. Manganese(IV) oxide acts as a catalyst to increase the rate of reaction
between zinc and hydrochloric acid
Conclusion:
The presence of catalyst increases the rate of reaction

45. Application of Catalysts in Industry
Haber Process (Produces Ammonia)
• In the Haber process, a mixture of nitrogen and hydrogen in
the ratio 1:3 is conducted through the powdered iron as
catalyst at a temperature of 450°C to 550°C and a pressure of
200 to 300 atmospheres with molybdenum as a promoter.
• Powdered iron is used as the catalyst to raise the rate of
reaction.
• Also, the reaction is conducted at high temperature to increase
the rate of reaction.

48. 1.3 Collision Theory
 The collision theory states
that:
• The particles of the reacting
need to touch to enable
formation or breaking of the
bonds for a reaction to
happen.
• Collisions of particles of a
reacting substance need to
achieve a certain minimum
energy (Activation Energy) in
order to produce a reaction.
• Particles that collide also need
to have the correct orientation
of collision.

49.  According to collision theory, atoms, ions, and molecules
can react to form products when they collide with one
another, provided that the colliding particles have
enough kinetic energy.
Effective Collision
Ineffective Collision

50.  Activation Energy
• The activation energy is the minimum energy that the reactants
particles must achieve at the time of collision in order for a
chemical reaction to take place.
• The value of the activation energy is different for different
reactions.
• A reaction with high activation energy occurs slowly whereas a
reaction with a low activation energy occurs fast.

51. Energy Profile Diagram
In the diagram of energy profile, the activation energy is shown by the
difference in energy between the peak of the graph and the level of the
energy of the reacting substance.
Exothermic Reaction Endothermic Reaction

52. Factors Affecting Rate Of Reaction -
Explanation By Collision Theory
 Total Surface Area of Reactants
• When the size of the solid substance that reacts is smaller, its total
surface area exposed becomes larger.
• This causes the collisions frequency between the reactants increases.
• As a result, the frequency of effective collisions also increases and
hence increases the rate of reaction.

53.  Presence of Catalyst
• When a positive catalyst is used in a reaction, the catalyst
prepares an alternative path with lower activation energy for the
reaction.
• As a result, the frequency of effective collisions increases and
hence increases the rate of reaction.

54.  Concentration
• Solution with higher concentration has more particles per unit
volume in the solution.
• As a result, the collisions frequency between the reactants
increases.
• Consequently, the frequency of effective collisions also
increases and hence the rate of reaction increases.

55.  Temperature
• When the temperature of a reaction increases, the particles of
the reacting substances move faster.
• This causes the collisions frequency between the reactants
increases.
• As a result, the frequency of effective collisions also increases
and hence increases the rate of reaction.

56. Pressure of Gas
• For a reaction that involves a gas, when pressure increases,
the particles of gas are compressed to fill the spaces which are
small. This makes the number of particles of gas per unit of
volume to increase.
• This causes the collisions frequency between the reactants
increases.
• As a result, the frequency of effective collisions also increases
and hence increases the rate of reaction

57. 1.4 Scientific Knowledge to
Enhance Quality of Life
1. Keeping food in a refrigerator
• If food is kept in the fridge, the food will keep longer because
the low temperature will slow down the rate of the chemical
reaction which destroys food.

58. 2. Cooking food in a pressure cooker
• In a pressure cooker, the high pressure causes the water in the
cooker to boil at a temperature of more than 100°C.
• At a higher temperature, the time for the food to get cooked is
decreased.

59. 3. Cooking Food in Small Pieces
• Food in the shape of big pieces has a surface area per volume
which is small, so the heat takes a longer time to reach the
inside of the food. So, to cook faster, the food needs to be cut
into smaller pieces.

60. 4. Making Margarine
• Vegetable oil is an organic compound that is not saturated and
exists in liquid state at room temperature.
• Through investigation and continuous development, vegetable
oil can be changed to margarine through the process of
hydrogenation using nickel as catalyst at a temperature of
180°C

61. 5. Breakdown of
Petroleum
• Big molecules of
hydrocarbon obtained
during fractional
distillation of petroleum
have been found to be
less useful than small
molecules of
hydrocarbon.
• The breakdown process
with the use of the
catalyst alumina
produces smaller
hydrocarbons.

62. 6. Burning of Coal
• Coal contains the element carbon. Burning of coal in air that is
in excess will produce carbon dioxide, water, and heat energy.
• A big piece of coal takes a long time to burn because the total
surface area that is touched by the fire is small.
• The rate of burning pieces of coal which are small is higher
because the total surface area is bigger. With this, it provides a
lot of heat energy in a short period of time.

63. • http://cikguwong.blogspot.my/p/chemistry-spm
• http://documents.mx/documents/chemistry-form
• http://spmchemistry.onlinetuition.com.my/2013