Ideal gas laws |Boyle’s law | Charles Law
The Ideal gas laws that states that the products of the absolute temperature of the gas and the universal gas constant is equal to the product of the pressure and volume of a single gram of an ideal gas.
Boyle’s law :
The law of Boyle is a gas law that states that the pressure exerted by a gas (of a given mass, sustained at a constant temperature) is inversely proportional to the volume it occupies. In other words, a gas’s pressure and volume are inversely proportional to each other as long as the temperature and gas quantity remain constant.
The relation between volume and pressure (at constant mass and temperature) can be mathematically expressed as follows:
P ∝ (1/V)
Where P is the pressure exerted by the gas and V is the volume occupied by it. This proportionality can be converted into an equation by adding a constant, k.
P = k (1/V)
PV = k
In Boyle’s Law, the product of pressure and volume at constant temperature is a constant for an ideal gas
Charles Law :
Charles Law states that for an ideal gas the volume is proportional to the absolute temperature at constant pressure. The rule also states that when the pressure exerted on a sample of a dry gas is kept constant the Kelvin temperature and volume should be in direct proportion.
Charles law also sometimes called volume law provides a detailed account of how gas expands as the temperature increases. Conversely, as when temperature decreases it leads to volume decrease.
V / T = Constant
The laws of Boyle and Charles can be merged into the ideal equation for gases:
PV = (a constant) x T
PV = nRT
The constant ‘n’ is number of moles and R is the specific gas constant,