CBSE Class 11 Chemistry States Of Matter Notes Set 03

1. Change in state : It is over all effect of Intermolecular forces, molecular Interactional energy & thermal energy:

2. Measurable properties of gases : P,V, T, n, Viscosity, specific heat are some measurable properties.

3. Gas Laws : The quantitative relationship b/w any two of the variables (V, n, P,T) when other two are constant.

4. Boyle’s Law : The pressure of fixed msss of gas varies inversely with the volume at constant T. P α 1/V(n,T const.)

P₁V₁ = P₂ V₂

5. Charle’s Law : At constant P, the volume of fixed amount of gas varies directly with its absolute temperature.

V α T or    V/ T  =constant , V₁ /T₁ = V₂/ T₂ 

6. Gay lussac’s Law : At constant V, The pressure of fixed amount of gas varies directly with its absolute temperature.

P α T or  P/T = Const , P₁ /T₁ = P₂ /T₂ 

7. Ideal gas equation : The relationship b/w P, V and T by Gas Laws PV= nRT.

8.Avogadro’s Law : At given T and P, the volume of gas

varies directly to the amount of gas . V α n ( P, T constant)

9. Dalton’s Law of partial persure : The pressure enerted by a mixture of non reacting gases is equal to the sum of their partial pressure at constant (V,T)

P (total ) = P1 + P2 + P3 + ………. (T, V, constant)

10. Kinetic Molecular theory :

a. Gases consist of large number of identical particles (atoms or molecules) that are so small that the actual volume of the molecules is negligible in comparison to the empty space between them.

b. There is no force of attraction between the particles of a gas at ordinary temperature and pressure

c. Particles of a gas are always in constant and random motion

d. Pressure is exerted by the gas as a result of collision of the particles with the walls of the container

e. Collisions of gas molecules are perfectly elastic

f. At any particular time, different particles in the gas have different speeds and hence different kinetic energies

g. Average kinetic energy of the gas molecules is directly proportional to the absolute temperature

11. Real Gases : The gases which deviates from Ideal behavior at higher pressure and low temperature b/c of force of attraction b/w molecules increases .

12. Compressibility factor (Z) : It determine extent of devation of real gases from Ideal gas behavior : Z =  PV/n.R.T. for ideal gas Z=1, for Nonideal gas Z< 1, Z > 1

13. Vander waal’s Equation : . ( P+ n²α / V² ) V -nb =nRT.

14. Critical Temperature : (Tc) The temperature above which a gas cannot be liquefied whatever high pressure may be

15. Critical Pressure : The minimum pressure required to liquity a gas at its critical temperature.

16. Critical Volume : The volume of 1 mole of gat at Tc, Pc.

17. Super cooled liquids : The liquids which are cooled to a temperature below its freezing point without freezing . 

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