How does pressure affect the phase transition from gas to liquid?

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Pressure significantly influences the phase transition from gas to liquid, as increasing pressure can lead to liquefaction at specific temperatures. The temperature of the resulting liquid depends on the substance and the pressure applied, particularly in relation to the triple and critical points. At temperatures above the triple point but below the critical point, gas and liquid phases can coexist under certain pressures. If temperature is held constant during compression, the gas will transition to liquid at a defined pressure. Understanding these dynamics is crucial for applications in thermodynamics and material science.
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If I Press gas to a pressure in which it changes to liquid. What would be temperature of this liquid after?
 
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Unary phase diagram:

http://wikis.lib.ncsu.edu/images/9/9c/CH434_575px-Phase-diag.svg.png

At any temperature higher than the triple point temperature (but below the critical point), there is some pressure at which the gas and liquid will coexist. The exact curve depends on the substance you are compressing.

So if you fix the temperature, you can compress the gas until it liquifies. If you are not holding the temperature fixed, the behavior has to depend on whatever constraints you are imposing.
 

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