This NIST table lists water’s saturation pressure as a function of temperature, showing that saturation pressure is tabulated by temperature rather than by total air pressure. The table is a thermophysical property reference for water and supports the statement that, at a given temperature, water has a specific saturation pressure value.

The paper presents simple expressions for saturated vapour pressure over water and over ice and analyzes their behavior. Saturation vapour pressure is treated as a temperature-dependent property of water/ice, not as a function of the total air pressure at fixed temperature.

The saturation vapor pressure above argon depends significantly on temperature. The article states that an increase in temperature causes an increase in vapor pressure, and that this holds for vapor pressure above the liquid and above the solid.

The text defines saturation as the state when air contains the maximum amount of water vapor possible for its given temperature, such that condensation equals evaporation. It states: "The amount of water vapor that the atmosphere can contain depends on temperature. Lower temperature air cannot contain as much water vapor as higher temperature air." It further explains that saturation vapor pressure refers to the pressure exerted by water vapor over a surface of liquid water and that "Temperature is the primary factor determining water vapor saturation." A graph based on the Clausius-Clapeyron equation shows saturation vapor pressure as a function of temperature only.

Total atmospheric pressure is the sum of the partial pressures of all the constituents.[2] For water vapor, the partial pressure is called the vapor pressure, e.[2] Let e_s represent the saturation vapor pressure at equilibrium over pure water having a flat surface.[2] Liquids boil when the saturation vapor pressure e_s equals the ambient pressure P of the atmosphere: P = e_s.[2] Exposition: At saturation for this T, water-vapor partial pressure is only 4.3% of total pressure P ≈ 101.3 kPa.[2] Although any portion of water vapor can be held in air, it is rare for the vapor pressure to be more than 1% greater than the saturation value.[2]

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature. At a given temperature, it is an equilibrium property of the substance rather than a property of the surrounding air pressure.

Total atmospheric pressure is the sum of the partial pressures of all the constituents.[5] For water vapor, the partial pressure is called the vapor pressure, e.[5] At this critical value, the air is said to be saturated, and the vapor is in equilibrium with liquid water.[5] Exposition: At saturation for this T, water-vapor partial pressure is only 4.3% of total pressure P≈101.3 kPa.[5] The relationship between saturation vapor pressure and the absolute humidity is given by the ideal gas law for water vapor: e_s = ρ_v · ℜ_v · T.[5] "Temperature to which a given air parcel must be cooled at constant pressure and constant water-vapor content in order for saturation to occur."[5]

The primary unit used to measure moisture in a gas is vapor pressure and Dalton law of pressures can be applied as long as the saturated vapor pressure remains unexceeded.[3] In environmental contexts, relative humidity is commonly employed as a unit. This metric represents the percentage ratio of the actual vapor pressure present in a gas to the saturation pressure at the corresponding temperature.[3] Consequently, it varies with temperature but remains unaffected by the pressure of the gas carrying it.[3] Moreover, it's observable that the saturated vapor pressure increases dramatically—by an order of magnitude—every 15 to 20 degrees.[3]

Lower temperatures are saturated with respect to water vapor at lower vapor pressures, while higher temperatures need higher vapor pressures to be saturated. The amount of water vapor that the atmosphere can contain depends on temperature. The saturation vapor pressure value at 100 °C is 101.325 kPa, the same value as the atmospheric surface pressure.

This application note states: "The air temperature dictates the maximum partial water vapor pressure in air, in other words, the water vapor saturation pressure. The ability of water to be in gaseous form is strongly dependent on its temperature (see Figure 1: Water vapor saturation pressure curve). The higher the temperature, the higher the partial pressure of the water vapor." It further notes that "The partial water vapor pressure in the immediate presence of liquid water equals the saturation pressure at that specific temperature." A separate remark points out: "The density of air varies with pressure, so the absolute humidity depends quite strongly on the gas pressure," distinguishing between saturation vapor pressure (temperature-controlled) and absolute humidity (which depends on total pressure via density).

The National Weather Service calculator describes that one can obtain the saturated vapor pressure by "enter[ing] the air temperature" and labels the output as "saturated vapor pressure." The tool does not require total atmospheric pressure as an input; the saturation value is computed solely from temperature, consistent with the standard meteorological definition that saturation vapor pressure of water is a function of temperature only.

Saturation vapor pressure (es) is a function of temperature only.["KNOWLEDGE_BASE"] It describes the maximum partial pressure of water vapor that can exist in equilibrium with liquid water at a given temperature.["KNOWLEDGE_BASE"] The total air pressure is the sum of the partial pressures of dry air and water vapor, but changing the total pressure does not change es, which depends solely on temperature.["KNOWLEDGE_BASE"]

The page presents the ideal gas law in the form pV = nRT and emphasizes that the pressure of a gas depends on its temperature, volume, and amount (moles). In mixtures, each gas obeys the ideal gas law via its partial pressure. This framework underlies psychrometric analysis: for a fixed temperature and fixed volume, changing the total pressure by adding or removing other gases changes their partial pressures, but the equilibrium saturation vapor pressure of water at that temperature is determined by its own thermodynamic properties and is not directly altered by the presence of other gases.

Vapor pressures are dependent only on temperature and nothing else. The vapor pressure of a liquid does not depend on the amount of liquid in the container; at the same temperature, samples of different sizes have the same vapor pressure.

Relative humidity is the amount of water vapour in the air, expressed as a percentage of the maximum amount that the air could hold at that temperature.["KNOWLEDGE_BASE"] As the temperature increases, the air can hold more water vapour and so the relative humidity falls if the amount of water vapour remains the same.["KNOWLEDGE_BASE"] Relative humidity is defined by the ratio of the actual vapour pressure to the saturation vapour pressure at the same temperature; this saturation vapour pressure is determined by temperature, not by the total air pressure.["KNOWLEDGE_BASE"]

The saturated vapor pressure of any substance depends on its temperature. At higher temperatures, more molecules have sufficient kinetic energy to break from the liquid surface into the vapor phase. Under these conditions, equilibrium is reached at a higher pressure.

The static vapor pressure method at constant temperature is described as an equivalent method. The entry defines vapor pressure in terms of a confined environment and distinguishes it from the total atmospheric pressure.

The table shows water’s vapor pressure rising from 4.6 torr at 0 °C to 760 torr at 100 °C. These values illustrate that the saturation vapor pressure of water changes strongly with temperature.

In thermodynamics, the saturation vapor pressure of water is primarily a function of temperature. At fixed temperature, changing the surrounding air pressure does not materially change the equilibrium saturation vapor pressure of pure water; it changes the relative humidity threshold mainly through the total pressure of the gas mixture, not the saturation vapor pressure itself.

A physics discussion thread explains: "The saturated vapour pressure is the pressure being exerted by a single component vapour, that is the definition of partial pressure." It continues: "The saturation pressure is the partial pressure of vapor that is in equilibrium with its own liquid. The pressure, temperature, and number density that govern condensation remain unchanged, no matter what other species are present." This argument appeals to Dalton's law and equilibrium thermodynamics to justify that saturation vapor pressure of water at a fixed temperature is independent of the total air (barometric) pressure, although the presence of other gases reduces the volume available so saturation is reached with fewer water molecules.

The water starts to evaporate until it is either all gaseous, or the vapor pressure of the water is its saturation pressure.[1] The total pressure in the flask at equilibrium is the sum of the partial pressures of the air and the water vapor.[1] Therefore, the final total pressure in the flask will equal the saturation vapor pressure of the water plus the partial pressure of the air.[1] Since the water vapor will exert its own pressure (the saturation vapor pressure), and the air still contributes its own pressure, we can express the total pressure as follows: P_total = P_air + P_vapor.[1]

The saturation vapor pressure of water increases with increasing temperature and can be determined with the Clausius–Clapeyron relation. The boiling point of water is the temperature at which the saturated vapor pressure equals the ambient pressure.

Dalton's law states that the partial pressure of water vapor or any substance does not depend on air pressure at all, and the relevant temperature is that of the liquid. The page also notes that vapor pressure is the pressure of a vapor in thermodynamic equilibrium with its condensed phases at a given temperature.

The vapour pressure of water is the pressure at which water vapour is in thermodynamic equilibrium with its condensed state. At higher pressures water would condense, and at this equilibrium condition the vapor pressure is the saturation pressure.

Saturation vapor pressure is the maximum vapor pressure possible at a given temperature. The lesson states that saturation vapor pressure depends on temperature and increases as temperature increases.

The presenter explains that saturation vapor pressure depends on temperature and not on total pressure: 'if we keep total pressure of air, change it, this variable es saturation vapor pressure turns out depends on temperature.'