Issues related to the supercritical temperature and pressure of gases
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As is well known, certain gases such as CO2 and NH3 can be liquefied by applying pressure and lowering the temperature. However, these gases have high boiling points and are relatively easy to liquefy. My question is: for ethylene, whose boiling point is very low at -103°C, it can also be liquefied by applying pressure and lowering the temperature. But suppose we have a 2L stainless steel tank containing ethylene at a pressure of 5 MPa at room temperature; if we then increase the pressure to 10 MPa using N2 while lowering the temperature to 0°C, what percentage of the ethylene in that tank will be liquefied?
Can this amount of liquefaction be calculated? Is there a method for it?
Pressurizing with a permanent gas can indeed prevent the liquid from boiling, but the surface still vaporizes until the partial pressure reaches a fixed value at the current temperature; in other words, the total pressure increases at equilibrium. Steam below the critical temperature cannot be cooled; it also cannot be liquefied merely by \"pressurizing\" it with an inert gas.