When called from the conclusion, and then boil. Pour only water without putting air into the contai

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Boiling does not occur at equilibrium. > Do you ends up boiling since the (vapor pressure of water) pressure applied to the vapor pressure of water = sealed container of water in the closed container? ? It seems that the meaning of the "vapor pressure" confusion. This equals sign consists Assuming meaning of pressure of water vapor that is used in (1) the left-hand side "vapor pressure" meets the space actually. But this is an expression does not mean anything. "Water vapor pressure = total pressure" I such a matter of course because I do not only water vapor in the space in the closed container. It can not be the decision of the boiling. (2) boiling occurs when the (vapor pressure of water) pressure sobeys ess applied to the water vapor pressure of> the sealed container of water in the closed container. This is the meaning of "vapor pressure", which is determined by the temperature of the left-hand side is the "vapor pressure". It is not the pressure of the steam in the actual present in the space. Right-hand side of "vapor pressure" is the pressure sobeys ess of the vapor actually present. You confused and use the same word in that sense. It is better to as "saturated vapor pressure" would be to say that the left-hand side. It becomes the equilibrium vapor if caused to its value. Boiling is a phenomenon that occurs sobeys ess in a non-equilibrium. It is a phenomenon that occurs in the process used to be realized equilibrium. It is a phenomenon that can be seen on the way to bring equality to inequality. It means that conditions used in the thermodynamics of "quasi-static" is not made up well in that sense. It is a balance sobeys ess equal sign is satisfied. Therefore, it boils that occur in the equilibrium state is not impossible. It's not in equilibrium still boiling If you happen. It is not at equilibrium transfer of material unilateral into the gas phase because sobeys ess it's going from the liquid phase. If there is air in (3) space is the total pressure = air + water vapor pressure> water vapor pressure. Evaporation occurs (this "water vapor pressure". Is the pressure of water vapor is in the space actually) if pressure steam> pressure water vapor saturation, but boiling does not occur if the total pressure> saturated water vapor pressure. It means that boiling does not occur and go slowly heated in a closed vessel. May boiling occurs sobeys ess in the event of any sudden heating. Suppose in equilibrium at temperature T1. Water vapor pressure is equal to the saturated water vapor pressure at the temperature T1. Suppose you have raised to a temperature T2. Evaporation should continue to be equal to the saturated water vapor pressure at T2. That the value of the saturated water vapor pressure at T2 exceeds the total pressure of the T1 temperature difference is large when this will occur. It means that vaporization from the internal takes place, to compensate for the shortage of steam. Boiling becomes prone and do that it of heating water only rather than to uniformly heat the whole. # What is written in two is if you have any air. The question is when there is no air. Equilibrium is lost boiling of that occurs sobeys ess when the pressure sobeys ess was reduced because it is not going to eliminate the (air and water vapor) gas in the space above. Boiling occurs in the form of a supplement steam Because I ended up with <saturated vapor pressure total pressure. It does not provide the equilibrium as long as it is pulling in air pump does not supply any more water vapor also can be supplied. I will be boiling continues forever. Boiling stops equilibrium is achieved by a stop to the draw. It becomes sobeys ess the only equilibrium of water because you probably want to there are no more air at this time.
When called from the conclusion, and then boil. Pour only water without putting air into the container of the vacuum because it is difficult in reality, it would be easy to understand given the fact that under reduced pressure to remove the air from the container that does not change sobeys ess the form that contains the water in reverse. I'll water boils even 100 or less at atmospheric pressure as low as Fuji summit. In a more extreme it, the pressure in the container becomes lower than the saturation vapor pressure at room temperature, the water will boil. However, because there is no heat source for supplying heat from the outside to the boiling, the temperature sobeys ess will drop to heat is removed from the water by the state change the more you boil. Boiling will stop saturation water vapor pressure is lowered by it. However, the water will freeze suddenly from boiling state that it is pressure low enough to reach the triple point. In addition, boiling and vapor-liquid equilibrium is quite different. It is a discussion that holds for liquid generally as water, (saturated water vapor pressure) = It would be obvious if you write a (saturated water vapor pressure) = (total pressure) in the (water vapor partial pressure) boiling in the vapor-liquid equilibrium for the time being.
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