With all other conditions unchanged, if pressure is reduced alone, will the temperature rise as a result?
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With all other conditions unchanged, if pressure is reduced alone, will the temperature rise as a result?
According to PV=nRT, when all other conditions remain constant (that is, the substance remains the same, the amount in moles remains constant, and the volume stays unchanged), a lower pressure results in a lower temperature.
I think it will rise; for example, such an increase occurs during the actual operation of the tower.
To be honest, what you say might be hard for me to understand due to your way of thinking. Since it has already been said that all other conditions remain unchanged, and that the pressure is reduced, I really don’t know how to answer whether the temperature condition will change (increase). In an ideal adiabatic model, assuming that only temperature and pressure can change, if the pressure decreases, then according to PV=nRT, the temperature will drop rather than rise. For reference.
For an ideal gas, according to PV=nRT, when all other factors remain constant (i.e., the amount of substance remains fixed, the moles remain fixed, and the volume remains unchanged), a decrease in pressure results in a decrease in temperature； There may be no such relationship for liquids
The temperature will drop; it definitely won’t rise.
I agree with what was said on floor 6: for volatile liquids, a decrease in pressure increases their volatility; the process of vaporization is endothermic, which also leads to a drop in temperature