At higher temperature the vapor pressure is higher.
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 water at 50ºC will be greater than that at 10ºC because of the added energy and thus greater movement of the water molecules. If one knows the ∆Hvap at a given temperature, one can calculate the vapor pressure at another temperature. This uses the Clausius-Clapeyron (sp?) equation. It turns out the vapor pressure of water at 10º is 9.2 mm Hg, and that at 50º is 92.5 mm Hg.
10^-10 Pa, it is a refractory material after all
Any time you drop the external temperature, it is going to make it easier for compounds to boil since the atmosphere is no longer exerting as much force down on the liquid. However, whether one or both compounds boils at that temperature depends less on the difference between their two boiling points and more on what their vapor pressure is at whatever temperature they are at. Compounds boil when their vapor pressure (the pressure of the molecules that naturally escape the solid or liquid because they have more energy) is the same as the external pressure. The vapor pressure of a substance depends only on temperature, which is why the point at which something boils is tied to temperature. Take water for instance. Water boils at 100 degrees C at sea level because at that temperature its vapor pressure is 1 ATM (760 mm Hg). At room temperature (25 degrees C) water has a vapor pressure of around 22 mm Hg. Since its vapor pressure at 25 degrees C exceeds 10 mm Hg, it would indeed boil at that pressure. Now if a liquid had a boiling point that was 50 degrees below water's, it would presumably boil at that temperature as well (although not necessarily... depends on other factors). If a liquid had a boiling point that was 50 degrees higher than water, then there is a decent chance it may not boil, but you would really need info on its vapor pressure at room temperature to know.
Use the ideal gas equation to get moles of water vapor. PV = nRT (1 atm)(131.97 L) = n(0.08206 L*atm/mol*K)(298.15 K) = 5.3939 moles H2O (6.022 X 10^23/1 mole H2O) = 3.2482 X 10^24 atoms of water vapor --------------------------------------------------------
Vapor pressure of water at 10 0C is less than that at 50 0C because, like gas pressure, as temperature rises, the kinetic energy of particles increases, thus increasing pressure. So the pressure of water vapor at 50 0C has more vapor pressure than at 10 0C.
Yes, the vapour pressure of water at 10°C is 1.2 kPa and at 50°C is 12.3 kPa.
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 water at 50ºC will be greater than that at 10ºC because of the added energy and thus greater movement of the water molecules. If one knows the ∆Hvap at a given temperature, one can calculate the vapor pressure at another temperature. This uses the Clausius-Clapeyron (sp?) equation. It turns out the vapor pressure of water at 10º is 9.2 mm Hg, and that at 50º is 92.5 mm Hg.
Yes. As long as the pressure is below atmospheric pressure.
10^-10 Pa, it is a refractory material after all
Water vapor can exist at this temperature if it is supercooled (if there is no condensation nuclei for it to form on).
The pressure is greater then 10 mm.
Water vapour.Water vapour.Water vapour.Water vapour.
Any time you drop the external temperature, it is going to make it easier for compounds to boil since the atmosphere is no longer exerting as much force down on the liquid. However, whether one or both compounds boils at that temperature depends less on the difference between their two boiling points and more on what their vapor pressure is at whatever temperature they are at. Compounds boil when their vapor pressure (the pressure of the molecules that naturally escape the solid or liquid because they have more energy) is the same as the external pressure. The vapor pressure of a substance depends only on temperature, which is why the point at which something boils is tied to temperature. Take water for instance. Water boils at 100 degrees C at sea level because at that temperature its vapor pressure is 1 ATM (760 mm Hg). At room temperature (25 degrees C) water has a vapor pressure of around 22 mm Hg. Since its vapor pressure at 25 degrees C exceeds 10 mm Hg, it would indeed boil at that pressure. Now if a liquid had a boiling point that was 50 degrees below water's, it would presumably boil at that temperature as well (although not necessarily... depends on other factors). If a liquid had a boiling point that was 50 degrees higher than water, then there is a decent chance it may not boil, but you would really need info on its vapor pressure at room temperature to know.
10 inches of water column equals to how much gas pressure?
Troposphere