GAS LAWS

GAS LAWS

WE ARE GOING TO EXAMINE THE FOLLOWING LAWS UNDER THIS TOPIC

BOYLE’S LAW

CHARLE’S LAW

GENERAL GAS EQUATION

DALTON’S LAW OF PARTIAL PRESSURE

GAY LUSSAC’S LAW

AVOGADRO’S LAW

GRAHAM’S LAW OF DIFFUSION

RELATIVE VAPOUR DENSITY OF GASES
IDEAL GAS EQUATION

BOYLE’S LAW

The relationship between volume and pressure of a gas was first established by Robert Boyle’s in 1662. The law states as follows “that volume of a given mass of a gas is inversely proportional to the pressure, provided the temperature remains constant.

MATHEMATICALLY EXPRESSED

V   inversely  1/P

V= K/P

K= PV

Hence P_1V1=P₂v₂

P₁ initial pressure (mmHg)

V₁ initial volume in (dm3 or cm3)

P₂ final pressure (mmHg)

V₂ final volume in (dm3 or cm3)

HOW KINETIC THEORY EXPLAIN BOYLE’S LAW

In order to explain this phenomenon, let experiment using enclosed vessel where mass of a gas was kept on it, with a malleable piston at a constant temperature with suitable weight on it. The average velocity and collision make will be constant if the weight was removed and light weight was used to replaced.

Observation: we will have observed that the piston will move up and the original volume will be also.

                           While the collision particle will be reduced, therefore the volume of gas increase, pressure decrease and vice versa.  

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