The properties of gases are governed by the following laws.
This law was given by R.Boyles in 1662.
Boyle’s Law states that at a constant temperature, the volume of a fixed amount of gas is inversely proportional to its pressure.
This means that if the pressure of a gas increases, its volume will decrease, and if the pressure of the gas decreases, its volume will increase, as long as the temperature remains constant. This relationship can be expressed mathematically as:
PV = k
where P is the pressure of the gas, V is its volume, and k is a constant value representing the initial conditions of the gas.
Let P be the pressure of a gas, V be its volume, and k be a constant of proportionality. Then, according to Boyle’s Law:
P ∝ 1/V
or
PV = k
To derive this expression, we start with the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the absolute temperature. Assuming that the amount of gas remains constant (i.e., n and R are constant), we can rewrite this equation as:
PV = kT
where k is a constant of proportionality that combines n and R. We can then rearrange this equation to isolate P:
P = kT/V
Now, if we assume that the temperature remains constant (i.e., T is constant), we can rewrite this equation as:
P ∝ 1/V
or
PV = k
This is the expression for Boyle’s Law.