Boyle law,Density,Thermal Expansion & Kinetic Theory

What is the Boyle law

There are three different types of states materials have, they include Solids,liquids and Gases; each state of matter goes through different characteristics. Gasses for example, they do not have a fixed volume,basically this means that u can compress gases. This is shown when a plane takes off or lands and the air pockets in your ears pop. boyle's law describes the relationship between pressure and volume at constant temperature for a fixed mass;the number of molecules of a gasTo understand Boyle's law, it helps to visualize the behavior of gas particles (or molecules) in an enclosed space. In a closed container, individual molecules are constantly hitting and bouncing off the container walls. Each time a gas molecule bounces, it imparts a force on the wall.1 In a flexible container such as a balloon, the force of the molecules hitting the inside of the balloon hold the balloon inflated. The force of each impact is small, but the sheer number of collisions create enough force to keep the balloon open.

Pressure in a closed container changes if temperature changes,number of molecules +- and if volume changes.

Boyle’s Law deals with number 3; the relationship between volume and pressure when - the other two remain constant.According to Boyle’s Law, the amount a gas will compress is proportional to thepressure applied. Its mathematical expression is: P1V1=P2V2Where, P1 is the pressure of a quantity of gas with a volume of V1 and P2 is the pressure of the same quantity of gas when it has a volume of V2. This means that if nothing else changes, the volume of a given mass of gas is inversely proportional to pressure it is under. It is a linear relationship. If pressure on a gas doubles, its volume will decrease by 1/2. An alternative expression of the law is: PV = CThe product of the volume and pressure equals a constant.The relationship between pressure and volume results from the influence volume has on the rate at which gas molecules collide with the container walls. If the volume decreases, the molecules encounter the container walls more often. This is true even though the speed (temperature) of the individual molecules has not changed. An increased number of collisions equates to higher pressure. Conversely, if volume increases, the rate of collisions and the pressure decreases.


Here is an example of boyle's law