Endothermic vaporization
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Gentle masters! Liquefied gases absorb heat during vaporization; theoretically, to what temperature can the ambient temperature be reduced? Please advise, experts
If a drop of water evaporates in a room, will the room’s temperature change? Everything needs to be structured in a systematic way; your problems need to be quantified!
Without power restrictions, it can be reduced to the boiling point of the medium used. Actual considerations include evaporation rate, heat transfer efficiency, indoor air flow, and temperature field
The same question phrased differently, for example, “How much liquefied gas needs to be vaporized in order to reduce a space of a certain volume from the ambient temperature to the desired temperature?” ” To enable everyone to respond accurately.
I want to ask if there is a limit to lowering the temperature? Can it lower the temperature of a substance below the boiling point of the refrigerant?
The scope is too wide; this question doesn’t make much sense
Because in an open system, just like in the atmosphere, the pressure drops to the atmospheric pressure, and the corresponding temperature is the boiling point. If the medium is in a closed system, applying negative pressure with a vacuum pump can further reduce the pressure. Use the correlation to look up the saturation vapor pressure vs. temperature curve
You should first determine the current temperature of your environment, and then figure out how much heat needs to be removed to reach the desired temperature. After that, decide which liquefied gases to use to absorb that heat (calculating the required amount based on their heat of vaporization)