KINETIC THEORY OF MATTER AND GAS LAW

 

Week:   FIVE                         Date:                                                   Time:

Period:                                   Duration:                                           Average age of learners:

Subject:                               CHEMISTRY                                                         Class:  SS ONE

Topic:                                                    KINETIC THEORY OF MATTER AND GAS LAW

Sub – Topic:  Kinetic theory of matter and kinetic theory of gas

Reference materials:

(1) ESSENTIAL CHEMISTRY, TONALD PUBLISHERS, I. O ODESINA[ 4th Edition]  pg72-76

(2) NEW SCHOOL CHEMISTRY, AFRICAN FIRST PUBLISHERS, OSEI YAW ABABIO

(3) INTERNET

Instructional materials: stone,  and water

Entry behavior: The students have been familiar with state of matter

Behavioural objective: At the end of the lesson the students should be able to:

1st PERIOD

Explain kinetic theory of matter

Differentiate the properties of the three states of matter

2nd  PERIOD

Explain change of state

 differentiate between vapourization and sublimation

 3rd PERIOD

State the kinetic theory of gases

Mention the natural  phenomena that explain kinetic theory of gas

The Kinetic Theory of Matter and Gas law

1st PERIOD

STEP I:  The teacher explains kinetic theory of matter

The kinetic theory of matter recognizes that matter is composed of very small particles (ions, atoms and molecules) whose different pattern of arrangements and motions result in the different possible states in which matter can occur. The kinetic theory of matter postulates that these particles are continually in motion and so possess kinetic energy.

 

 

 

 

 

 

 

 

 

STEP II: The teacher explains the three state of matter

Comparison of the properties of the states of matter.

Properties

Solid

Liquid

Gas

Arrangement of particles

Closely packed together in an orderly manner

Close together in a disorderly manner , in clusters

Far  apart in a random manner

Forces between particles

Very strong

Strong

Negligible

Movement

Vibration about fixed positions increase as temperature increase

Vibrations and movement throughout the liquid

Vibrations and movement anywhere

Energy of particles

Less energy

More than in solid

More than in liquid

Density

High (particles close together)

High (particles close together)

Low (particles far apart)

compressible

No

No

Yes

 

  EVALUATION

The teacher assesses the lesson by asking the following questions:

Briefly explain Kinetic theory of matter.

Compare the three states of matter with two distinct properties

2nd  PERIOD

STEP I: The teacher explain change of state of matter

Change of state is brought about by a change in temperature i.e heating and cooling. When a substance is heated, its constituent particle acquire Kinetic energy. When cooled they become less energetic.

There are six distinct changes of phase which happens to different substances at different temperatures. The six changes are:

Freezing: the substance changes from a liquid to a solid.

Melting: the substance changes back from the solid to the liquid.

Condensation: the substance changes from a gas to a liquid.

Vaporization: the substance changes from a liquid to a gas.

Sublimation: the substance changes directly from a solid to a gas without going through the liquid phase.

Deposition: the substance changes directly from a gas to a solid without going through the liquid phase.

                Evaporation: This is the process of vaporization of liquids at all temperatures. The rate of evaporation increases with increase in temperature.

                Boiling: When a liquid is heated, the rate of evaporation increases and the value of the saturated vapour pressure of the liquid rises until a temperature is reached at which the saturated vapour pressure of the liquid equal the prevailing atmospheric pressure.

  EVALUATION

The teacher assesses the lesson by asking the following questions:

What bring about the change of state of matter

What is the different between vapourization and sublimation

 ASSIGNMENT

What is the different between evaporation and Boiling

3rd PERIOD

STEP I: The teacher explains the kinetic theory of gases

The kinetic theory of gases explains the empirical laws (i.e. Boyle’s law, Charles’ law, Graham’s law of diffusion, Dalton’s law of partial pressure and Avogadro’s law), which govern the behavior of gases.

STEP II: The teacher states the assumptions of the theory of gases

The theory is based on the following assumptions about perfect or ideal gases (these are gases whose behaviors can be explained by the kinetic theory - they have no real existence):

1.  Gases are composed of discrete particles called molecules which are in rapid, random motion, moving at high speed in straight lines - this is the reason gases can diffuse very rapidly.

2.  The molecules are so small, and at low pressures are so far apart, such that on the average, the actual volume of their molecules is negligible compared with the volume of their container

- this is the reason gases do not have fixed volume, but take up the volume of the container in which they are kept.

3.  The molecules exert no force of attraction or repulsion upon one another. I.e., the molecules are independent of each other - this is the reason gases do not have definite shape.

4. Upon collision with one another, or with any surface, they rebound without any loss in the total kinetic energy of the system. In other words, the molecular collisions are perfectly elastic.

5.  The pressure of the gas results from the impacts of the molecules upon the walls of the containing vessel. The pressure exerted by a gas confined within a fixed volume is proportional to nEk , i.e., the number of molecules per unit volume (n) times their average kinetic energy (Ek).

6. The average kinetic energy of all the molecules is assumed to be directly proportional to the absolute temperature of the gas. This means that molecules of different gases at the same temperature have the same average kinetic energy. The kinetic energy of a moving molecule, like that of any moving object, is the energy associated with its motion.

Note: at ordinary temperature and pressure, real gases approximately fulfill the above assumptions.

Application of the Kinetic Theory of Matter to Explain the Nature of Gases

The three properties of gases that are especially important are diffusibility, thermal expansion and compressibility.

STEP III: The students chorus the assumption

  EVALUATION

The teacher assesses the lesson by asking the following questions:

Explain the kinetic theory of gas

State three assumption of kinetic theory of gas

 

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