400 mL at 20C
1st, this question isn't very clear. Are you looking for the total vapor pressure? The vapor pressure of the dissolved component? I'm pretty sure it's NaCl in water. I'm guessing that's a tie with Sugar in water. The highest vapour pressure is alcohol in water, followed by benzene in water...followed by water itself. Also, the kind of alcohol is important. (The order of alcohol or benzene depends on the kind of alcohol.) The best way to get a rough idea of the vapor pressure of a substance is to look at their boiling points....which is by definition when the vapor pressure of the liquid is equal to atmospheric pressure....that's why it bubbles.
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.
If a hydrate's vapor pressure is higher than the water vapor in the air, water molecules will evaporate from the hydrate into the air until equilibrium is reached. This process will continue until the vapor pressures are equalized.
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.
To find the partial pressure of water vapor in the vessel, subtract the partial pressure of N2 from the total pressure: Partial pressure of water vapor = Total pressure - Partial pressure of N2 = 2.015 ATM - 1.908 ATM = 0.107 ATM.
Water heated to above the boiling point (steam), or below the vapor pressure for water in the gas sample with water vapor in it.
120 kP
Depending on the pressure, it can be in any of these phases.
The total pressure is the sum of the partial pressure of nitrogen and the vapor pressure of water. Therefore, the partial pressure of nitrogen is the total pressure minus the vapor pressure of water. Given that the total pressure is not provided in the question, we need more information to calculate the partial pressure of nitrogen.
The temperature of the water is 100 degrees celsius.
0.0113 mol oxygen
1st, this question isn't very clear. Are you looking for the total vapor pressure? The vapor pressure of the dissolved component? I'm pretty sure it's NaCl in water. I'm guessing that's a tie with Sugar in water. The highest vapour pressure is alcohol in water, followed by benzene in water...followed by water itself. Also, the kind of alcohol is important. (The order of alcohol or benzene depends on the kind of alcohol.) The best way to get a rough idea of the vapor pressure of a substance is to look at their boiling points....which is by definition when the vapor pressure of the liquid is equal to atmospheric pressure....that's why it bubbles.
At 50 degrees Celsius, a compound with the lowest vapor pressure would be one with strong intermolecular forces like hydrogen bonding, such as water (H2O). These strong forces make it harder for molecules to escape into the gas phase, resulting in a lower vapor pressure compared to compounds with weaker intermolecular forces.
The saturated vapor pressure of water at 50 oC is 123,39 mm Hg.
The vapor pressure of water at 10°C is lower than its vapor pressure at 50°C. As temperature increases, the vapor pressure of water also increases because more water molecules have enough energy to escape into the gas phase.
water at sea level has higher vapor pressure
The vapor pressure of pure water at 25 degrees Celsius is 23.8 torr.