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7.0 Explain the definition of rate of reaction correctly

7.1 Determining of rate of reactions by

7.1.1 Classify fast and slow reactions that occur in daily life

7.1.2 Explain the meaning of the rate of reaction

7.1.3 Identify changes which can be observed and measured during chemical reactions through activity

7.1.4 Determine:

i) Average rate of reaction

ii) Instantaneous rate of reaction

7.1.5 Solve numerical problems based on the average and instantaneous rate of reactions

7.2 Factor affecting rate of reactions

7.2.1 i) Size of reactants

ii) Concentration

iii) Temperature

iv) Presence of catalyst

7.3 Application of factors that affect the rate of reaction in daily life

7.3.1 Explain with examples the application of factors that affect the rate of reaction in daily life

7.4 Collision theory

7.4.1 Describe the collision theory

7.4.2 Explain activation energy using examples

7.4.3 Interpret an energy profile diagram for exothermic reaction and endothermic reaction

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Rate of reaction is the changes in the quantity of the reactant per unit time or the changes in the quantity of the product per unit time.

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Observable changes during chemical reaction

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Observable changes during chemical reaction

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Formation of precipitate

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Observable changes during chemical reaction

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Observable changes during chemical reaction

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Decrease in the mass of the reactants

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Observable changes during chemical reaction

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Observable changes during chemical reaction

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Increase in the volume of gases

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Average rate of reaction is the average value for the rate of reaction that occurs in a particular time interval.

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Instantaneous rate of reaction is the rate of reaction at a particular point of time. - determine from experimental data by plotting a graph of changes in the 

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i) Size of reactant

For same amount of reactant, particles with smaller size has bigger total surface area.

The bigger the total surface area, the higher the rate of reaction.

Link youtube video: https://youtu.be/-Q8ZSexABS0?si=XA42kG6R2QXvFeYf

ii) Concentration

The higher the concentration, the higher the rate of reaction.

Link youtube video: https://youtu.be/4xkjF5Z3lyI?si=bJJkG0JOcLO2dx9O

iii) Temperature

Most reactions occur faster at high temperature, that is rate of reaction increases with increasing temperature.

Link Youtube video: https://youtu.be/oeM6hKm6Td4?si=wvXUpyx7znKv3qyT

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iv) Catalyst

Catalyst is a chemical substances that alter the rate of chemical reactions without undergoing any chemical changes at the end of the reaction.

The chemical properties of the catalyst does not change, but its physical properties can change.

Link Youtube vid : https://youtu.be/kV0BqG0On9E?si=IjoZHbKknB3IFW_w

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Manganese (IV) oxide, MnO₂

Decomposition of hydrogen peroxide

Concentrated sulfuric acid

Nitration of benzene

Iron, Fe

Manufacture of ammonia by the Haber process

Vanadium (V) oxide, V₂O₅

Conversion of SO₂ to SO₃ during the Contact Process to make sulfuric acid

Nickel, Ni

Hydrogenation of a C=C double bond

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Antacid tablet are used to treat tablets.

Doctors advise patients to chew the tablet instead of swallowing.

Breaking up the tablet into smaller pieces increases the total surface area exposed and increases the rate of reaction between the medicine and the acid in the stomach.

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Buildings made of iron that are located near the industrial areas will corrode fast due to acid rain.

The atmosphere around industrial areas contains a high concentration of sulphur oxide.

When the concentration of acidic pollutants increases, the level of acid rain increases and the rate of corrosion increases.

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Washing clothes using detergent powder and hot water combines two factors that increases the rate of reaction.

The process of washing clothes will be even quicker in this situation.

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Ethanol C₂H₅OH is produced through the fermentation of glucose with the help of enzyme in yeast as a catalyst at 37oC.

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According to collision theory:

Reactant particles must collide with one another for reaction to occur.

The rate of reaction depends on the frequency of effective collisions.

What happen during collision?

During collision, transfer of energy occurs.

Fast moving particles transfer some of their energy to slow moving particles and increases their kinetic energy.

Not all collision between reactant particles result in reactions and the formation of products.

Only effective collision would cause reaction to occur.

Effective collision is the collision that produces a reaction achieving minimum energy that is sufficient and with the correct orientation of collision.

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The activation energy is the minimum energy that the particles of the reactants 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 low activation energy occurs fast.

Activation energy is represented by the symbol Ea. In the diagram of the 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.

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Exothermic

System release heat energy to surroundings.

Enthalpy change is negative.

Endothermic

System absorb energy from surrounding.

Enthalphy change is positive.

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Effect of concentration and size of reactant

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Effect of concentration and size of reactant

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When the concentration of the reactant of particles increases,

The number of particles per unit volume increases

The frequency of collisions between particle increases

The frequency of effective collisions between particle increases

The rate of reaction increases

When the total surface area of the reactant increases

the total surface area exposed to collisions increases

The frequency of collisions between particle increases

The frequency of effective collisions between particle increases

The rate of reaction increases

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When the temperature of the reactant of particles increases,

The kinetic energy of the reactant particles increases

The frequency of collisions between particle increases

The frequency of effective collisions between particle increases

The rate of reaction increases

In the presence of the catalyst,

The catalyst provides an alternative pathway by lowering the activation energy

More reactant particles can achieve the activation energy

The frequency of effective collisions between particle increases

The rate of reaction increases

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https://padlet.com/alya_khadijahlee/assessments-for-rate-of-reaction-24tp7irquelvmabp

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Find some helpful notes and good practices here.

1. https://drive.google.com/file/d/1QO5BFzJBJnKo93cpNfkabU4R8oEm7lT2/view

2. https://drive.google.com/file/d/1gLqydAlizFX8OLHJ1Zr59poxfaQh8C1I/view