The evaporation of the liquid by heating.
The higher the vapor pressure of a liquid at a given temperature, the lower the normal boiling point (i.e., the boiling point at atmospheric pressure) of the liquid.
its boiling
its boiling
The higher the vapor pressure of a liquid at a given temperature, the lower the normal boiling point (i.e., the boiling point at atmospheric pressure) of the liquid.
Increased heat or reduced pressure or both.
The pressure exerted by the gas in equilibrium with a solid or liquid in a closed container at a given temperature is called the vapor pressure
Vapor pressure increases over a liquid in a closed container until the amount of vapor molecules rejoining the liquid equals the number leaving the liquid to form vapor. This is the characteristic vapor pressure of the substance.
If the temperature of the liquid is raised, more molecules escape to the vapor until equilibrium is once again established. The vapor pressure of a liquid, therefore, increases with increasing temperature.
The temperature at which the vapor pressure of a liquid is equal to the external pressure is the boiling point. Evaporation is when vaporization of an uncontained liquid occurs.
The temperature at which the vapor pressure of the liquid equals the atmospheric pressure is called THE BOILING POINT.
The weaker the intermolecular forces, the easier the liquid evaporates. Higher vapor pressure the faster it evaporates. Thus, the weaker the attractive forces, the higher the vapor pressure and vice versa.
When water vapor is cooled it turns into liquid.