The vapor pressure (in mmHg) of acetic acid at 20C is approx. 26.
Vapor pressure of water at 30.9 dgCelsius is 4471 Pa ( or 0.04413 atm or 455.9 kgf/m^2 )
747 mmHg
757.2 mmHg is almost atmospheric pressure (P = 760 mmHg) and therefore the vapour pressure is very close to the normal boiling point.According to the boiling temperature is T = 353.14 K = 79.99 °C at P = 757.2 mmHg.
The partial pressure of oxygen in expired air is 109 mmHg. Partial pressure is calculated at the proportion of oxygen in the air, so at 1 atmosphere for dry air pressure is 713 mmHg (which is 760 total pressure - 47 mmHg water vapor) and oxygen is 21% of the dry gas concentration so inspired pO2 is 150 mmHg.
Do you mean, how does the pressure of water vapor at 10˚C compare with its pressure at 50˚C?The vapor pressure of water is the pressure at which steam is saturated. Above this pressure, the water would begin to condense. In a gas mixture saturated with water vapor, the vapor pressure is equal to the partial pressure. The vapor pressure is a function of temperature. Many equations of state can predict vapor pressures of liquids but the best ones are also rather complex and require considerable expertise to use. For most purposes, there are several simpler empirical equations which can estimate the vapor pressures of liquids with sufficient accuracy for most purposes.One of the simplest is the Antoine equation which has the form:log10Pvap = A - B/(C+T) where the Pressure (P) is in mmHg and the Temperature (T) is in °C.For water in the range from 1 °C to 100 °C, the constants have the values:A = 8.07131B = 1730.63C = 233.426Using these values, the vapor pressure of water can be estimated as:Pvap(@10 °C) = 9.158817 mmHgPvap(@50 °C) = 92.29989 mmHg... so the vapor pressure of water at 50 °C is roughly 10 times the vapor pressure at 10 °C.
The vapor pressure of PCl3 at 298K is approximately 52.8 mmHg.
Vapor pressure of water at 30.9 dgCelsius is 4471 Pa ( or 0.04413 atm or 455.9 kgf/m^2 )
39330 j.mol-1
747 mmHg
Depends on temperature. For ASTM D323 the RVP of water is ~49.5 mmHg (torr) gauge or ~809 mmHg absolute (assuming standard pressure). FYI - ASTM D323 is measured at 100F.
757.2 mmHg is almost atmospheric pressure (P = 760 mmHg) and therefore the vapour pressure is very close to the normal boiling point.According to the boiling temperature is T = 353.14 K = 79.99 °C at P = 757.2 mmHg.
== Vapor Pressure Of Ethanol== According to Shuzo Ohe's conmputation program it's 102.65 mmHg.
The partial pressure of oxygen in expired air is 109 mmHg. Partial pressure is calculated at the proportion of oxygen in the air, so at 1 atmosphere for dry air pressure is 713 mmHg (which is 760 total pressure - 47 mmHg water vapor) and oxygen is 21% of the dry gas concentration so inspired pO2 is 150 mmHg.
400 mmHg pressure can be converted to KP to be 53.33.
Do you mean, how does the pressure of water vapor at 10˚C compare with its pressure at 50˚C?The vapor pressure of water is the pressure at which steam is saturated. Above this pressure, the water would begin to condense. In a gas mixture saturated with water vapor, the vapor pressure is equal to the partial pressure. The vapor pressure is a function of temperature. Many equations of state can predict vapor pressures of liquids but the best ones are also rather complex and require considerable expertise to use. For most purposes, there are several simpler empirical equations which can estimate the vapor pressures of liquids with sufficient accuracy for most purposes.One of the simplest is the Antoine equation which has the form:log10Pvap = A - B/(C+T) where the Pressure (P) is in mmHg and the Temperature (T) is in °C.For water in the range from 1 °C to 100 °C, the constants have the values:A = 8.07131B = 1730.63C = 233.426Using these values, the vapor pressure of water can be estimated as:Pvap(@10 °C) = 9.158817 mmHgPvap(@50 °C) = 92.29989 mmHg... so the vapor pressure of water at 50 °C is roughly 10 times the vapor pressure at 10 °C.
253 mmhg (torr)
taken up; -5 mmHg