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The critical temperature of a gas provides insight into the strength of the intermolecular forces of attraction that its particles are subject to. For example, a gaseous substance with relatively weak intermolecular forces will be harder to liquefy than a gaseous substance featuring stronger intermolecular forces of attraction.
The liquid–vapor critical point in a pressure–temperature phase diagram is at the high-temperature extreme of the liquid–gas phase boundary. The dashed green line shows the anomalous behavior of water. For simplicity and clarity, the generic notion of critical point is best introduced by discussing a specific example, the vapor–liquid ...
In fact, for every substance, there is some temperature above which the gas can no longer be liquefied, regardless of pressure. This temperature is the critical temperature (Tc), the highest temperature at which a substance can exist as a liquid.
Table A–1 Molar mass, gas constant, and critical-point properties Table A–2 Ideal-gas specific heats of various common gases Table A–3 Properties of common liquids, solids, and foods Table A–4 Saturated water—Temperature table Table A–5 Saturated water—Pressure table Table A–6 Superheated water Table A–7 Compressed liquid water Table A–8 Saturated ice–water vapor
13 Νοε 2022 · At temperatures below 31°C (the critical temperature), CO 2 acts somewhat like an ideal gas even at a rather high pressure (). Below 31°, an attempt to compress the gas to a smaller volume eventually causes condensation to begin.
The following table lists the critical temperatures and critical pressures for some well-known gases and liquids. Such data are often quite useful. Many gases are sold commercially in strong steel cylinders at high pressures.
The Ideal Gas Law relates the pressure, temperature, volume and moles of a gas through the gas constant “R.”. The ideal gas law reduces to the other gas laws when you start holding different variables constant. The Ideal Gas Law can also relate density and molar mass with the gas constant “R.”.
