Matter exists in three states On Earth: solid, liquid and gas, and in every state exhibits different characteristics. Gases do not have fixed shape or volume; as a result, gases respond to change in pressure by altering their volume. Boyle’s law describes the relationship between volume and pressure at a constant temperature for a fixed mass of gas.

Boyle’s law helps to understand the behavior of gas in an enclosed space. Individual molecules regularly hit and bounce off the walls in a closed container. In an elastic container like a balloon, the force of molecules clashing inside the balloon hold it inflated.

The pressure in an enclosed region changes if the following factors occur.

- Volume changes
- The number of molecules decreases or increases
- Temperature changes

**Boyle’s Law Equation**

Boyle’s law specifies how pressure and volume are related when other two factors(temperature & number of molecules) remain constant.

According to Boyle’s law, the amount of gas compressed is proportional to the applied pressure. It can be expressed as:

**P****1****V****1**** = P****2****V****2**

Where,

P1 is pressure of amount of gas with a volume V1

P2 is pressure of the same amount when the volume is V2

This states that the volume of a particular mass of gas is inversely proportional to pressure if nothing else changes.

**Boyle’s law Graph**

The graph between V & P at constant temperature is a smooth curve called as Parabola.

Graph between V and 1/P at constant temperature is a straight line.

If the gas pressure doubles, the volume is decreased by half. When put mathematically,

**PV = C**

The product of pressure and volume is constant.

The relationship among volume and pressure results from the impact of volume on the rate of gas molecules colliding with the walls. The molecules collide the walls more often when the volume decreases. A higher pressure equates to higher number of collisions. Conversely, the rate of collisions and pressure decreases if the volume increases.

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