How is condensation related to vaporization?
824019
As explained by previous responders, condensation is the reverse of vaporisation. However it is important to realise that vaporisation is the transition to a gaseous state and condensation is the transition from a gaseous state. \n\nThere are substances and conditions where a liquid state never occurs. For example carbon dioxide (dry ice) at one atmosphere of pressure passes from solid to gas without becoming a liquid. This is still called vaporisation. It passes from gas to solid without becoming a liquid and this is still called condensation. By far the more common transition is from and to a liquid state.
309679
condensation.  the cold glass provides a surface for water to collect into liquid form.
1081964
they are all fases of the water cicle. First the water evaporates (goes from being in a liquid state to being in a gasy state) due to the heat coming from the sun, the water vapor rises up in the air and condensates (takes a more dense state but still remains being water vapor) then after a lot of water vapor is concentrated (humidity) a cloud forms and it gets bigger and bigger as more and more water vapor concentrates until the amount of humidity is to large and the water vapor turns into water and precipitates wich would conclude the cicle in this last fase ,wich goes by the name of precipitaion, and then to start all over again.
357469
Raoult's Law describes a colligtive property.  It states that the more particles that are in solution, the lower the vapor pressure of the solution is.  For example, if I had a beaker of water out and I poured some salt in, the vapor pressure of the salt water would be lower than pure water's vapor pressure.  \n\nMathematically:\nVapor Pressure of the solution = (mole fraction of the solvent) * (Vapor pressure of the pure solvent)\n\nThe mole fraction of the solvent is found by dividing the number of moles of solvent by the total number of particles in solution.  \n\nRaoult's Law works because as more particles are added to the solvent, those particles that are being added block the vapor of the solvent from rising and escaping.  That means that the more particles added, the more vapor pressure blocking, and the lower the vapor pressure of solution.  \n\nRaoult's Law can also alternately apply to when two volatile substances (two liquids that evaporate readily) are mixed together. All you do to calculate total vapor pressure over the mixture is add the two vapor pressures together for the substances.
38126
A gas can also flow and wet through condensation.
413571
Boyles law related the pressure and volume of a gas, as pressure goes up volume goes down and vice-versa. Charles law related temperature and volume, as temp goes up so does volume and vice versa.\n\nThe collapsing can demo really does not show either of these laws. If you boil a small amount of water in a can for a few minutes the water will turn to water vapor and expel most of the air out of the can. Then you need to invert the can and place it in cold water. This will seal the opening AND cause the water vapor in the can to condense. After the vapor condenses to liquid water, it takes up less space--- this decreases pressure inside the can, and higher air pressure outside the can crushes it. Not related to either law because they deal with gasses only, not gasses that change state to a liquid.
615392
I assume that you are talking about a knock out pot. \n\nAtmosperic air naturally contains moisture, and we know that the condensation temp of waters is increased at higher pressure. That means that an increase in pressure means that the moisture in the air will tend to condense at a higher temperature. So the fist step in seperation is to cool the compressed air, this cause a lot of the moisture to condense and it can be collect at a low point in the system. \nThe next step is a knock out pot. The air usually enters about half way up this cylinder and exits at the top. The moisture exits at the bottom. In this pot at the top is a baffle plate. The purpose of this is to change the air flow direction several times suddenly, and the heavier mositure droplets gets knocked out and fall to the bottom.\n\nFor a dust slightly higher than atmospheric pressure the result will be the same, but less water would be seperated
83902
Certainly.  RH is the amount of water vapor in the air divided by the maximum amount possible (before condensation occurs) given the temperature.  The maximum possible increases with increasing temperature, so if you heat air in a closed container the RH decreases, and if you cool it enough the RH increases until reaching 100%, when condensation begins.
754142
It seems like you could figure the relative humidity based on the pressure, temperature, specific volume, etc.  After that you could figure the volume of condensation on a per cubic meter basis.  You would need a total volume to come up with the total mm/day.  Hope that helps get you going on the right path to an answer.  If not, you should re-post your question with additional information- I get the feeling you left something out.
503418
vaporization, change of a liquid or solid substance to a gas or vapor. There is fundamentally no difference between the terms gas and vapor, but gas is used commonly to describe a substance that appears in the gaseous state under standard conditions of pressure and temperature, and vapor to describe the gaseous state of a substance that appears ordinarily as a liquid or solid. Although most substances undergo changes of state in the order of solid to liquid to gas as the temperature is raised, a few change directly from solid to gas in a process known as sublimation.\n\nLiquids can also change to gases at temperatures below their boiling points. Vaporization of a liquid below its boiling point is called evaporation, which occurs at any temperature when the surface of a liquid is exposed in an unconfined space. When, however, the surface is exposed in a confined space and the liquid is in excess of that needed to saturate the space with vapor, an equilibrium is quickly reached between the number of molecules of the substance going off from the surface and those returning to it. A change in temperature upsets this equilibrium; a rise in temperature, for example, increases the activity of the molecules at the surface and consequently increases the rate at which they fly off. When the temperature is maintained at the new point for a short time, a new equilibrium is soon established.\n\nThe pressure exerted by the vapor of a liquid in a confined space is called its vapor pressure. It differs for different substances at any given temperature, but each substance has a specific vapor pressure for each given temperature. At its boiling point the vapor pressure of a liquid is equal to atmospheric pressure. For example, the vapor pressure of water, measured in terms of the height of mercury in a barometer, is 4.58 mm at 0°C and 760 mm at 100°C (its boiling point).
253266
the greater the intermolecular forces the stronger the surface tension the more energy it takes to evaporate.\nso the heat of vaporization would be higher as well.
988557
Do you mean water cycle?\n\nWater vapor in the air is part of the water cycle. Water vapor is a gas. Water vapor is a variable gas in the atmosphere being higher in places near water sources esp. the ocean.
95618
basically you're talking about distilling water, which is a purification technique.  collect the water vapor and let it condense. the result is pure water.
786378
evaporation is when the liquid form of water eevaporates or becomes water vapor. evaporation is one part of the water cycle and is a very large one. evaporation puts water into the air as a gas called water vapor. this then condenses into tiny droplets, forming clouds. \n\nhope this helps
1163335
Wrong. There is the critical temperature/pressure up to which gas and liquid behave differently. Above these conditions, there cannot exist a liquid phase. Rather than speaking about gaseous phase, this state is called fluid. This state is also called supra-critical.\n\nBasically what happens is that the attractive forces in the liquid diminish as the critical point is approached, until the liquid behaves just like the vapour. The evaporation heat becomes zero.
503063
I think condensation.
385865
the height at which condensation takes place