The temperature of 100K is over boiling point 90.19 K at standard (air at sea level) pressure (101.325 kPa, 760 mmHg) so liquid oxygen is 'boiling' but not in equilibrium with its pressure = stand. P
To my best knowledge data of 'overheated' (above boiling point) liquid oxygen are not easily available, may be at 'liquid gas manifacturers' sites or data sheets.
high pressure vapor
A mercury thermometer, that is a barometer can be used to measure vapor pressure. Initially, a proper temperature must be recorded. Then the liquid should be injected into the mercury column. This new measurement subtracted from the original will yield the vapor pressure of a liquid.
In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium because the rate of evaporation of liquid equals the rate of condensation of vapor. -KarkatHorns
Vapor pressure of a liquid at its normal boiling temperature is simply the atmospheric pressure, aka 1 atm, 760 torr, etc. This is by definition.
No: Vapor is defined as the gas phase of a substance that is mostly solid or liquid at equilibrium at standard temperature and pressure. Therefore, a liquid itself is never a vapor, but the liquid is in equilibrium with a vapor phase that contains the same chemical substance.
At 125 F it is liquid. (Depending on pressure) At 125 C it is vapor. (Depending on pressure) At 125 Kelvin it is solid.
its boiling
its boiling
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
The Kelvin equation describes the change in vapor pressure due to a curved liquid/vapor interface with radius r. The vapor pressure of a curved surface is higher than that of a flat and non-curved surface.
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.
A liquid or vapor is saturated when it is at the temperature and pressure where it would be in equilibrium with the other phase; saturated liquid at the boiling point or saturated vapor at the dew point. If the pressure is raised, the vapor will condense until the pressure is restored to the original pressure or all the vapor is condensed. If the pressure is dropped, a saturated liquid will boil until the pressure rises back to the original pressure or all the liquid has vaporized. If the temperature is increased, a saturated liquid will boil off completely unless the vaporized liquid raises the pressure enough to establish a new equilibrium. If the temperature is dropped, a saturated vapor will condense until the pressure has dropped enough to establish a new equilibrium.
The Liquid will turn into gas. The boiling point corresponds to the temperature at which the vapor pressure of the liquid equals the atmospheric pressure. If the liquid is open to the atmosphere (that is, not in a sealed vessel), it is not possible to sustain a pressure greater than the atmospheric pressure, because the vapor will simply expand until its pressure equals that of the atmosphere.