States of matter-I-Gases-Key Points

States of Matter – Gases

Key Points:

1. Kinetic Molecular Theory: Explains gas behavior based on molecular motion, postulated by Daniel Bernoulli.
2. Boyle's Law: Volume is inversely proportional to pressure at constant temperature and moles.
   V ∝ 1/P (when T and n are constant)
3. Charles's Law: Volume is directly proportional to absolute temperature at constant pressure and moles.
   V ∝ T (when P and n are constant)
4. Avogadro's Law: Volume is directly proportional to the number of moles at constant temperature and pressure.
   V ∝ n (when P and T are constant)
5. Graham’s Law: Rate of diffusion or effusion is inversely proportional to the square root of molar mass or density.
   r ∝ 1/√d or r ∝ 1/√M
6. Dalton’s Law: Total pressure of a gas mixture equals the sum of partial pressures of individual gases.
7. Absolute Zero: Hypothetical temperature where gas volume becomes zero. Value: -273.16°C or 0 K.
8. Ideal Gas Equation: Represents gas behavior under ideal conditions.
   PV = nRT
9. Van der Waals Equation: Real gas equation accounting for molecular volume and attraction.
   (P + a(n²/V²))(V − nb) = nRT
10. Joule-Thomson Effect: Expansion of compressed gas into low-pressure causes cooling.
11. Ideal Gas: Obeys gas laws at all conditions; no molecular attraction forces exist.
12. Real Gas: Deviates from ideal behavior under high pressure or low temperature.
13. Plasma: Fourth state of matter; consists of positive ions, free electrons, and neutral atoms.

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