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Physical Science
Quarter 3 – Module 5:
Collision Theory & Catalyst
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Physical Science– Grade 11
Alternative Delivery Mode
Quarter 3 – Module 5: Collision Theory & Catalyst
First Edition, 2020
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Physical Science
Quarter 3 – Module 5:
Collision Theory & Catalyst
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Introductory Message
This Self-Learning Module (SLM) is prepared so that you, our dear learners,
can continue your studies and learn while at home. Activities, questions, directions,
exercises, and discussions are carefully stated for you to understand each lesson.
Each SLM is composed of different parts. Each part shall guide you step-bystep as you discover and understand the lesson prepared for you.
Pre-tests are provided to measure your prior knowledge on lessons in each
SLM. This will tell you if you need to proceed on completing this module or if you
need to ask your facilitator or your teacher’s assistance for better understanding of
the lesson. At the end of each module, you need to answer the post-test to self-check
your learning. Answer keys are provided for each activity and test. We trust that you
will be honest in using these.
In addition to the material in the main text, Notes to the Teacher are also
provided to our facilitators and parents for strategies and reminders on how they can
best help you on your home-based learning.
Please use this module with care. Do not put unnecessary marks on any part
of this SLM. Use a separate sheet of paper in answering the exercises and tests. And
read the instructions carefully before performing each task.
If you have any questions in using this SLM or any difficulty in answering the
tasks in this module, do not hesitate to consult your teacher or facilitator.
Thank you.
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What I Need to Know
This learning module was designed to help the students to learn the key concepts of
collision theory and catalyst and its role in the rate of chemical reaction. This
learning module deals with describing and identifying the intermolecular forces occur
between molecules and how these forces affect the properties of substances. To
further enhance the students’ learning, different learning activities are provided in
this module. The lesson is presented in an easy way in order to address the learning
difficulties of the students by using language level at par with their comprehension.
Based on the recent study, students learn more if they are actively engaged in the
textbook they are using. This learning module can help to improve the student’s
academic achievement in this subject. With this material, students can work in less
supervision of the teacher.
The module is contained one lesson.
• Lesson 1 – Collision Theory & Catalyst
The most essential learning competencies for this module.
Use simple collision theory to explain the effects of concentration, temperature, and
particle size on the rate of reaction (S11/12PS-IIIf-23)
Define catalyst and describe how it affects reaction rate (S11/12PS-IIIf-24)
After going through this module, you are specifically expected to:
1. Define collision theory and catalyst;
2. Describe the role of collision theory on concentration, temperature and the
particle size on the reaction rate,
3. Explain the collision theory of reaction,
4. Explain the role of a catalyst in chemical reactions, and
5. Express the rate of chemical reaction.
What I Know
Identify the key term referred in each statement. Write your answer on a
separate sheet of paper.
__________1. A branch of chemistry that deals with rate and factor that influence
the chemical reactions.
__________2. It can be measured in terms of change of concentration of reactant or
product per unit time.
__________3. It states that molecules must collide to each other in order for chemical
changes will occur.
__________4. It increases the speed of the chemical reactions.
__________5. The energy needed for the chemical reaction will take place.
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Lesson
1
Collision Theory & Catalyst
In chemistry, the particles such as atom, ions and molecules must collide before they
can combine with each other. For instance, atoms must in contact to other atoms or
molecules to form a chemical bond. With this idea, the collision theory will help us
to explain why reacting molecules have different rates of reaction depending on
several factors such as the concentration of the reactants, the temperature, the size
of the reacting particles and the significant role of catalyst in chemical reaction.
What’s In
What do you infer from these figures?
+
+
+
+
+
+
Let us say that these figures are particles. Based from the above figures, particles
combined to produce new particles. Some particles separate while other particle’s
partner have exchanged. The particles will collide with each other with required
amount of energy so that the reaction will take place. Thus, the collision theory will
help us to understand the behavior of these reacting particles. The reaction rates
occur faster than others. These rates depend on how these particles will collide, that
would influence by several factors that affect the rate of reaction such as
temperature, concentration and particle size as well as the catalyst.
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What’s New
Have you ever tried or experienced balancing chemical equations?
In a balanced chemical equation, it shows chemical reactions which occur at
different rates or speeds. However, in chemical reactions do not show to us how fast
the reaction rate in forming a product. In some cases, reactions happen very quickly
such as burning of alcohol. Some reactions happen slowly like rusting of iron in
damp air.
An area of chemistry that deals with how fast chemical reaction occurs and
the factors that influence the rate of reaction is called Chemical Kinetics.
Collision theory
The chemical reactions occur at different speeds, may be at fast or slowly rates. The
collision theory will help us to understand why chemical reactions takes place at
different speeds. In any chemical reaction, the collision theory assumes that the
particles either atoms, ions and molecules must collide in order for the chemical
change will take place. During the reaction, the colliding particles must have enough
energy so that electrons will change their position, old chemical bonds are broken
and new bonds are formed. The collision of atoms, ions and molecules must be strong
enough to destroy the old chemical bonds of the colliding particles. The collisions
between reactants must be effective, they must have enough energy called activation
energy. The activation energy is the minimum energy required for a reaction to
proceed.
Effect of concentration on the rate of reaction
As the concentration of one or more reactants is increased, the rate of reaction is
also increases. For instance, the concentration of gas reactant is expressed in terms
of the mass or number of moles of reactant per unit volume. The concentration of
gas reactant can be increased by decreasing the space of the gas container. In
contrary, allowing the gas to expand into a greater volume will decrease the
concentration of the gas. The higher frequency of the colliding particles will result to
a higher rate of reaction.
Effect of temperature on the rate of reaction
As the temperature increases, the rate of the chemical reaction is also increased. For
many cases of chemical reactions, in every 10 0C increased in the temperature
approximately the rate of reaction will double. This rule only applies to a chemical
reaction that will take for 1 or 2 seconds. When the temperature of a chemical
reaction is increasing, at the same time the energy of the colliding particles increases
as well. Moreover, the rise in temperature, it will also increase the collision frequency
and collision energy that will result to the rise of the speed of reaction.
Effect of particle size on the rate of reaction
The speed of a chemical reaction is affected by the particle size of the reactant. The
smaller the particles size of the reactant the faster the reaction takes place. Since,
the particle’s size is small the surface area becomes wide. The movement of particles
in a collision is higher and it will result to faster rate of reaction.
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Presence of Catalysts
A catalyst is a substance that increases the rate of chemical reaction. By adding this
substance, it will speed up the chemical reaction without being consumed in any
given reaction. This process is catalysis. In biology, lactase is an enzyme that breaks
lactose into simple sugar unit, is a specific example of a catalyst.
Catalysts can be divided into two, Homogenous and Heterogeneous. In
Homogeneous, reactants are in the same phase. For instance, liquid catalyst is in
liquid system and gas catalyst is in a gaseous system. While, in heterogeneous the
reactants are in different phase. For example, manganese dioxide (MnO 2), is a solid
used to speed up the decomposition of hydrogen peroxide (H 2O2) which is a liquid.
The rate of reaction is the change in the concentration of a reactant or a product per
unit time. The rate of reaction can be expressed in terms of rate of disappearance of
reactants and or the rate of appearance of the product per unit time.
The rate of this reaction can be expressed as
Rate = Change in concentration of reactant or product
Time it takes for the change to occur
Let X as represent of a reactant or product
Rate =
(X)
t
Where:
delta sign means “change in”
(X) given reactant or product
(t)
change in time
Note: (-) negative sign before concentration of reactants decrease
with time. The rate of reaction is always positive. The rate is
determined by the decrease in concentration of a reactant over
time or the increase in concentration of a product over time,
always end up with positive sign.
The fast or slow of the rate of chemical reaction can be affected by the following
factors.
1. Presence of a Catalyst, by speeding up the
consuming itself.
2. Reaction Temperature. The higher temperature,
faster.
3. Concentration of reactants. More concentration
chemical reaction will occur.
4. Nature of reactants. The rate of a chemical
depending on the nature of the reactants.
chemical reaction without
rate of chemical reaction is
of reactants, the faster the
reaction can be increased
Let’ s try this!!!
1. When the reaction in a 1.0 L flask, 8.0 x 10 -4 mol of Cl2 is formed during the first
5.0 s of reaction. What is the rate of reaction of Cl 2?
Since, the concentration of Cl2, at the start of reaction is zero, so Cl 2 = 0
M.
After the formation of 8.0 x 10-4 mol in a 1.0 L flask, then….
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Cl2 = 8.0 x 10-4 mol/1.0 L or 8.0 x 10-4 M
Change of concentration of Cl2= 8.0 x 10-4 M – 0 M = 8.0 x 10-4 M
Rate of reaction = Change in concentration of reactant or product
Time it takes for the change to occur
= 8.0 x 10-4 M
5.0 s
= 1.6 x 10-4 M/s
Express the rate of the following reactions.
1. Use this reaction as your reference, hydrogen reacts with chlorine
H2 + Cl2
2HCl
From the above example, each mole per L of H 2 produces 2 moles per L of HCl,
meaning the rate of HCl produces is double as fast as H 2 disappears. The rate of
reaction can be expressed as:
Rate of reaction = - (H2) = - (Cl2) = 1/2 (HCl)
t
t
t
2. When hydrogen combined with nitrogen, then the product formed is ammonia,
3H2 + N2
2NH3
Rate of reaction = -1/3
(H2) = - (N2) = 1/2 (NH3)
t
t
t
What is It
After reading the text in What’s new. Let us see how far you have learned this topic.
Match the term in Column A to Column B. Use a separate sheet of paper for
your answer.
A
B
a. An energy needed for the
chemical reaction to take
place.
_____1. Homogeneous
_____2. Catalyst
_____3. Collision theory
b. A reactant is at different
phase.
_____4. Heterogeneous
c. A reactant is in the same
phase.
_____5. Activation energy
d. It increases the rate of
chemical reaction.
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e. A particle must bump each
other then, chemical reaction
will occur.
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Answer the following questions comprehensively. Use a separate sheet of paper
for your answer.
1. Why do adding catalysts increase the rate of reaction?
2. Why do increasing the concentration of reactants increase the rate of a reaction?
3. Why do increasing the temperature of reactions increase the rate of reaction?
What’s More
Give the rate of expression of the following chemical equations. Use a separate
paper for your solution and answer.
1. 2KClO3
2. 2Na + Cl2
3. 2NH3
4. 4Na + O2
5. H2 + Br2
2KCl + 3O2
2NaCl
N2 + 3H2
2Na2O
2HBr
What I Have Learned
1. The collision theory helps us understand why chemical reasons occur at
different rates.
2. The catalyst is the substance that increases the rate of chemical reaction.
3. The rate of reaction can be measured in two ways: the speed will the reactant
disappears and the speed will the product appears.
4. In order, a collision to proceed it requires an energy which is activation energy.
5. In every increase of 100C in the temperature will double the rate of reaction.
6. The smaller the particle size, the faster the chemical reaction will occur.
7. The higher frequency of the colliding particles will result to a higher rate of
reaction.
8. The rate of reaction can be calculated through this equation:
Rate = Change in concentration of reactant or product
Time it takes for the change to occur
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What I Can Do
Answer the following questions using the given chemical equation below. Use
another sheet of paper for your solution and answer.
KNO3
KNO2 + O2
1. Balance the given chemical equation.
2. Write the rate of expression of the chemical equation.
3. How fast is KNO3 decreasing when oxygen (O2) is increasing at 1.75 x 10-3
mol/L.s?
4. How fast is oxygen (O2) is increasing when KNO2 is increasing at 2.25 x10-4
mol/L.s?
Assessment
Multiple Choice. Read and analyze each question. Write the letter that
corresponds to your answer on a separate sheet of paper.
1. What is the catalyst?
a. A substance added to slow
down the chemical reaction.
b. A substance added to speed
up the chemical reaction.
c. A substance added to form
hydrogen bond in a chemical
reaction
d. A substance added to disrupt
the bonded atoms.
2. What is the collision theory?
a. The reacting particles must
be in contact with one another.
b. The reacting particles are
stationary.
c. The reacting molecules
should be in high rate of
concentration.
d. The colliding molecules
should precipitate the reactants
in a chemical
reaction.
3. The minimum amount of energy required to start up the chemical reaction?
a. Reaction energy
c. Activation energy
b. Mechanism energy
d. Effective energy
4. Which of the following factors would not affect rate of reaction?
a. Nature of reactants
c. The climate
b. Temperature
d. Addition of catalyst
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5. What would you do, if you want to have more space for the particle size to collide?
a. Increase the concentration
c. Increase the volume
b. Increase the temperature
d. Increase the surface area
6. If you want to increase the concentration of a gas reactant, what would you do?
a. Decrease the space of the gas
c. Expand the surface are of the
container.
gas container.
b. Increase the space of the gas
d. Remove the cover of the gas
container.
container.
7. In chemistry, ( ) this symbol has a meaning of__________.
a. Remove in
c. Final in
b. Change in
d. Reaction in
8. Explain why the temperature of reaction increases and the rate of reaction
increases as well.
a. The particles are in contact
c. The reactant molecules
and have less activation energy.
collide more frequently and with
b. The activation energy is
high energy per collision.
decreased
d. The reactant molecules
collide less frequently and with
low high energy per collision
9. The rate of reaction can be expressed through______.
a. Change in concentration
c. Change in concentration in
reactant or product over time.
time over volume.
b. Change in concentration
d. Change in concentration
reactant
or
product
over
collision or energy over volume.
volume.
10 What will happen if there is 100C increase in temperature?
a. It will triple the rate of
c. It will remain the rate of
reaction.
reaction.
b. It will double the rate of
d. It will decrease the rate of
reaction.
reaction.
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Additional Activities
Answer the following word problems below. Use another sheet of paper for your
solution and answer.
When water breaks into its components, the products are hydrogen and oxygen.
1. Based on the above decomposition process, present and balance the chemical
equation.
2. Write the rate of expression of the chemical equation.
3. How fast is water (H2O) decreasing when oxygen (O2) is increasing at 2.5 x 10-3
mol/L.s?
4. How fast is oxygen (O2) is increasing when hydrogen (H2) is increasing at 4.25
x10-4 mol/L.s?
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What’s more:
Additional activities:
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Assessment:
What can I Do:
1. B
2. A
3. C
4. C
5. D
6. A
7. B
8. C
9. A
10. B
What is It:
1.
2.
3.
4.
5.
C
D
E
B
A
1. Chemical
kinetics
2. Rate of reaction
3. Collision theory
4. Catalyst
5. Activation energy
1. Based from the
above figures,
particles combined
to produce new
particles. Some
particles separate
while other particle’s
partner have
exchanged.
What I Know:
What’s In
Answer Key
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References
Chang, R. Chemistry 8th Edition. McGraw-Hill Companies, Inc., 1221 Avenue of the
Americas, New York, NY 10029, 2005.
David, B. Study Guide to Accompany Atkits and Beran: General Chemistry
2nd Edition. W.H. Freeman and Company, 41 Madison Avenue, New York, New
York 10010, 1995.
Dorin, H., Demmin, P.E., & Gabel D.L. Prentice Hall Chemistry: The Study of
Matter 3rd Edition. Prentice Hall, Inc. Needham, Massachusetts Englewood
Cliffs, New Jersey, 1990.
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