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Above the surface of liquid water is a layer of water vapor. It has pressure. The atmosphere also has pressure. It pushes against the water vapor. The water vapor pushes against the atmosphere. It is called vapor pressure. It is related to temperature. When the vapor pressure equals barometric pressure, water boils. Normally this occurs at 100C or 212F. If you reduce the barometric pressure, you can reduce the boiling point of water. So when the barometric pressure is lower, the water vapor above the water has an easier time mixing with the atmosphere. As it mixes with the atmosphere, it is replaced by vapor from the water. It evaporates.
High pressure is associated with cool, dense air--which can hold LESS wator vapor than warm air. Low pressure would be "moister" than high pressure--meaning it would carry a higher percentage of water vapor or have a higher relative humidity.
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.
Warmer air has higher saturation mixing ratios then cold air does. So therefore because of this 100% humidity in cold air is not 100% humidity in warmer air. The warmer the temperature, the more water vapor in the air. The colder the temperature, the less water vapor in the air.
The solution's vapor pressure will be lower.
water at sea level has higher vapor pressure
At higher temperature the vapor pressure is higher.
a solid compound which contains water molecules in its crystalline structure
The vapor pressure of 1 m sucrose (C12H22O11) is higher than the vapor pressure of 1 m NaCl where the solvent is water Sea water has a lower vapor pressure than distilled water. The vapor pressure of 0.5 m NaNO3 is the same as the vapor pressure of 0.5 m KBr, assuming that the solvent in each case is water The vapor pressure of 0.10 m KCl is the same as the vapor pressure of 0.05 m AlCl3 assuming the solvent in each case is water The vapor pressure of 1 m NaCl is lower than the vapor pressure of 0.5 m KNO3, assuming that the solvent in each case is water The vapor pressure of 0.10 m NaCl is lower than the vapor pressure of 0.05 m MgCl2 assuming the solvent in each case is water.
A solution has a higher vapor pressure than a pure solvent. This is why salt water boils faster than pure water.
Water evaporates at almost any temperature. However, at higher temperatures, the vapor pressure is higher. It is said to be boiling when the vapor pressure is equal to the atmospheric pressure.
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A liquid boils when the vapor pressure of the liquid is equal to the atmospheric pressure. The presence of salt in the water reduces the vapor pressure of the water at the temperature at which plain or distilled water will boil. Since the temperature of the salt water must be higher to reach the same vapor pressure as the atmosphere, it takes longer to boil.
Water usually boils at 212F or 100C at sea level. As you go higher up in the atmosphere (higher altitude), the amount of atmosphere pushing down on you decreases, hence the pressure decreases. Water boils when the vapor pressure of the water equals the atmospheric pressure. Vapor pressure increases with increasing temperature, so when there is less atmospheric pressure, a smaller vapor pressure is required to get the water boiling, hence a lower boiling temperature.
The anhydrous molecule or species. e.g. CuSO4.5H2O (hydrate) + heat ----> CuSO4 (anhydrous) + water vapor
The boiling of any liquid is tied in to the atmospheric pressure, in an open system. Every liquid has it's own vapor pressure, that is the balance between the vapor and liquid phase. When atmospheric pressure decreases, the vapor pressure increases since now there is greater space for the molecules of the liquid to come into vapor phase. At higher altitudes, the atmospheric pressure is lesser, that is, the air is thinner. Thus the liquid can attain higher vapor pressure faster and boil at a lower temperature.
higher then the normal boiling point of water