1st Year Chemistry Chapter 3 Notes
Important Complete Computerized Notes of 1st Year Chemistry Chapter 3 Notes written by Honorable Professor Mr. Faraz Qadir Suib. These notes are very helpful in the preparation of 1st Year Chemistry Chapter 3 Notes for the students of the intermediate and these are according to the paper patterns of all Punjab boards.
Summary and Contents:
Topics which are discussed in the notes are given below:
- Statement of Boyle’s Law with its expression
- The value of k is different for the different amounts of the same gas.
- Experimental Verification of Boyle’s Law
- Graphical Explanation of Boyle’s Law
- Plot of pressure and volume at 25 ⁰C
- Plot of PV and P
• Plot a graph between pressure on x-axis and the product PV on Y-axis.
• A straight line parallel to the pressure axis is obtained.
• This straight line indicates that 'k' is a constant quantity.
• At higher constant temperature, the volume increase and value of product PV should increase
due to increase of volume at same pressure, but PV remains constant at this new temperature and
a straight line parallel to the pressure axis is obtained.
- Experimental Verification of Charles’s Law
- Derivation of Absolute Zero
- Quantitative Definition of Charles’s Law
- General Equation for Calculating Volumes
- Celsius Scale does not Obey Charles’ Law
- Charles’s law is not obeyed if temperature is measured on Celsius scale
- Kelvin Scale Obeys Charles’s Law
- General Gas Equation using (i) Boyle’s Law (ii) Charles’s Law (iii) Avogadro’s Law
- State and Explain Dalton’s Law of Partial Pressures
- Calculation of Partial Pressure of a Gas
- Applications of Dalton’s Law of Partial Pressures
- State and explain Graham’s Law of Diffusion
- History of Kinetic Molecular Theory of Gases
- Postulates of Kinetic Molecular Theory: 1. Every gas consists of a large number of very small particles called molecules. Gases like He, Ne, Ar have
monoatomic molecules.
2. The molecules of a gas move haphazardly, colliding among themselves and with the walls of the container
and change their directions.
3. The pressure exerted by a gas is due to the collisions of its molecules with the walls of a container. The
collisions among the molecules are perfectly elastic.
4. The molecules of a gas are widely separated from one another and there are sufficient empty spaces among
them.
5. The molecules of a gas have no forces of attraction for each other.
6. The actual volume of molecules of a gas is negligible as compared to the volume of the gas.
7. The motion imparted to the molecules by gravity is negligible as compared to the effect of the continued
collisions between them.
8. The average kinetic energy of the gas molecules varies directly as the absolute temperature of the gas.
- Explanation of Gas Laws from Kinetic Theory of Gases
- Kinetic Interpretation of Temperature
- Linde’s Method of Liquefaction of Gases with its principle and working
- Van der Waals Equation for Real Gases
- Definition of Plasma State and Formation of Plasma
- Natural and Artificial Plasma
- Plasma State: Plasma is the “fourth state of matter”. Plasma was identified by the English scientist William Crookes in 1879.
Definition
The ionized gas mixture, consisting of ions, electrons and neutral atoms is called plasma.
OR
Plasma is a distinct state of matter containing a significant number of electrically charged particles a number
sufficient to affect its electrical properties and behaviour. When more heat is supplied, the atoms or molecules may be ionized. The atom loses one electron and develops
a net positive charge. It becomes an ion. In a sufficiently heated gas, ionization happens many times, creating
clouds of free electrons and ions. All the atoms are not ionized, and some of them remain completely intact with
no net charge.