Gas Laws

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. (P1V1 = P2V2)

Charles's Law states that the volume of a gas is directly proportional to its temperature in Kelvin when pressure is held constant. (V1/T1 = V2/T2)

The Ideal Gas Law is an equation of state for an ideal gas, represented as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin.

As the volume of a gas decreases, the pressure increases, provided the temperature remains constant (Boyle's Law).

As the temperature of a gas increases, the volume increases, provided the pressure remains constant (Charles's Law).

As the temperature of a gas increases, the pressure increases, provided the volume remains constant (Gay-Lussac's Law).

The gas constant (R) is 0.0821 L·atm/(K·mol) or 8.314 J/(K·mol), depending on the units used.

To convert Celsius to Kelvin, add 273.15 to the Celsius temperature (K = °C + 273.15).

Pressure is defined as the force exerted by gas particles colliding with the walls of their container, typically measured in atmospheres (atm) or pascals (Pa).

Volume is the amount of space that a gas occupies, typically measured in liters (L) or cubic meters (m³).