GAS LAWS

1. Boyle’s Law

This law was given by Boyle in 1662. According to this law,

At constant temperature, the volume of a given mass of a gas is inversely proportional to its pressure.

V    1/P   (when T  =Constt.)

PV = CONSTANT

Boyle’s law can be derived by Kinetic Gas Equation

PV =1/3(mNv2)                                         (i)

PV =(2/3). (1/3)(mNv2)                           (ii)

= 2/3 Ek

Ek = Average kinetic energy.

1/2 mNv2     T

1/2 mNv2 =KT                                     (iii)

K  is proportionality constt.

Compare Eq. (2) & (3)

PV = 2/3 KT

PV = constt.

V   1/P                              (At Constt. T) Boyle’s law

1. Charle’s Law

This law was given by charles in 1787 According to this law,

At constant pressure, the volume of given mass of a gas is directly proportional to its absolute temperature (T).

V    T                               (  at constt. Pressure)

V =KT

V/T = constt.

If the volumes of given mass of a gas are V1 & V2 at constt pressure & absolute temperatures T1 & T2

According to Charle’s law-

V1/T1 = V2/T2

(Absolute Temperature = 273 + temperature in c)

Berzelius presented a hypothesis & Avogadro modified, well tested & verified & then gave a law i-e Avogadro’s law.

According to this law,

‘Equal volumes of all gases under similar conditions of temperature & pressure contain equal number of molecules’.

For two gases, kinetic gas equation can be written as,

P1V1 =1/3 (m1 .N1 .v12) =2/3.1/3 .(m1 .N1 .v12)

P2V2 =1/3 (m2 .N2 .v22) =2/3.1/3 .(m2 .N2 .v22)

because, P1.V1 =P2.V2

1/2 m1. N1.v12 =1/2 (m2 .N2 .v22)

If temperature is constt, the average kinetic energy per molecule must be the same.

1/2 m1.v12 =1/2 m2.v22

The important conclusions of this law-

1. The proportion of volumes of gases in the gaseous reaction is the same as the proportion of their molecules or moles.

Ex.  N2  + 3H2 —–.>   2NH3

one mole of N2 combines with 3 moles of H2 to produce 2 moles of NH3