- Gases: The gas laws
- The kinetic theory of gases elementary denotation.
- Deduction of the gas laws
- Molecular speeds
- Deviations from ideal gas behavior
- Vander waal’s modification
1.Physical chemistry from Tertiary Institutions (Year one Edition) by John A. Ibemrsi
2. Physical chemistry for Tertiary Institution by John A. Ibemesi
3. Chemistry: The study of matter and it’s changes by James E. Brady and John R. Holy
4. Principles of General Chemistry (2nd edition) by Martin’s Silber berg
GASES: Matter exist as either gas, liquid, or solid. The state of matter is largely dependent on the conditions surrounding it, such as temperature and pressure. Eg water which could exist as either ice, water or vapour. Differences between each state of matter is based on physical properties.
I) Volume and shape
(III) compressibility (change in volume)
Volume and shape
Solids – fixed volume and shape , Liquids – fixed volume but not shape, Gases – takes volume of its container but not shape.
Solids – none
Liquids – slowly
Gases – Extreme.
Solids – compressible
Liquids – incompressible
Gases – Easily compressible
Solids – most dense, insensible to changes in temperature and pressure, Liquids – Denser, insensible to changes in temperature and pressure, Gases – less dense, very sensitive to changes in temperature and pressure.
Solids – definite form because molecules are ordered and tightly packed.
Liquids – intermediate between two extremes where there is a certain degree of order and a certain degree of molecular chaos.
Gases – Molecular chaos and negligible intermolecular forces.
Point to note – Liquids and gases have ability to flow hence both are referred to as fluids.
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