Vapor pressure
Vapor pressure is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system. Vapor pressure is also known as equilibrium vapor pressure.
equal to the sum of the atmospheric pressure and the pressure due to the weight of the liquid above the point of interest.
Yes, vapor pressure can occur in an open container. Vapor pressure is the pressure exerted by a vapor in equilibrium with its condensed phase in a closed system. In an open container, vapor can still form above a liquid or solid substance, but it will not reach equilibrium as it can escape into the surrounding environment.
At a constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid. See the link below for more information.
It's called the boiling point. It is the temp where the vapor pressure of the "liquid" is equal to the air pressure around (above) it. This is when the liquid [water] reaches 100 degrees Cecilius [at sea level].
in a state of dynamic equilibrium at a constant temperature. At this point, the rate of vaporization equals the rate of condensation, resulting in a constant pressure above the liquid known as the vapor pressure.
Vapor pressure is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system. Vapor pressure is also known as equilibrium vapor pressure.
When a gas is dissolved in a liquid, the partial pressure of the gas above the liquid decreases due to the gas molecules entering the liquid phase. According to Henry's Law, the amount of gas that dissolves in the liquid is proportional to the partial pressure of the gas above it. As more gas dissolves, the equilibrium is established, which can lead to a decrease in the overall pressure of the gas in the system. However, if the temperature or other conditions change, the pressure may fluctuate again.
In an open system, the vapor pressure is equal to the partial pressure of the vapor above the liquid at a given temperature. Unlike in a closed system, where vapor pressure can reach a dynamic equilibrium with the liquid phase, in an open system, vapor can escape, preventing the establishment of equilibrium. Therefore, the vapor pressure is not fixed and can vary depending on conditions such as temperature and the amount of vapor present.
At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
When a liquid and a gas are in equilibrium, the rate of evaporation of the liquid equals the rate of condensation of the gas. This means that the number of molecules transitioning from the liquid phase to the gas phase is equal to the number transitioning from the gas phase back to the liquid. As a result, the properties of the system, such as pressure and temperature, remain constant over time. Additionally, the concentration of the vapor above the liquid stabilizes at a specific value known as the vapor pressure.
The highest point above the equilibrium position is called the amplitude. It represents the maximum displacement from the equilibrium position in either direction.
equal to the sum of the atmospheric pressure and the pressure due to the weight of the liquid above the point of interest.
Yes, vapor pressure can occur in an open container. Vapor pressure is the pressure exerted by a vapor in equilibrium with its condensed phase in a closed system. In an open container, vapor can still form above a liquid or solid substance, but it will not reach equilibrium as it can escape into the surrounding environment.
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. PTo 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.
Saturated steam is gas-phase water in equilibrium with liquid water at the same temperature and pressure. If the temperature is above the saturation point and/or the pressure is below the saturation pressure, the steam is "superheated steam". In either case it is a gas. There are some conventions where saturated steam along with some fraction of liquid water in equilibrium with it is still referred to as steam even if not all of it is gas, as long as at least some of it is gas.
At a constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid. See the link below for more information.