Charles's law, also known as the law of volumes, relates the volume of a gas to its temperature, assuming constant pressure. It states that at constant pressure, the volume of a gas is directly proportional to its temperature.
Boiling point, on the other hand, is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure. It is not directly related to the volume of a gas but rather to the equilibrium between the liquid and gaseous phases.
When pressure is increased, the boiling point of a substance typically increases as well. This relationship is described by the Clausius-Clapeyron equation, which connects the boiling point to the vapor pressure and the molar enthalpy of vaporization.
The reason for this increase in boiling point with increasing pressure can be understood from the perspective of vapor pressure. As pressure increases, the vapor pressure required for a substance to boil and enter the gaseous phase also needs to increase to match the external pressure. This means that a higher temperature is needed to achieve the corresponding vapor pressure, hence the increase in boiling point.
It's important to note that Charles's law is not directly applicable to the relationship between boiling point and pressure. Charles's law specifically relates the volume of a gas to its temperature at constant pressure, while the boiling point depends on the equilibrium between the liquid and gaseous phases, which involves both pressure and temperature.