This is the temperature which relates to the maximum pressure above which gas cannot be formed regardless of temperature.

This is the temperature which relates to the maximum pressure above which gas cannot be formed regardless of temperature.

• A. Cricondentherm temperature
• B. Cricondenbar temperature
• C. Critical temperature
• D. Boiling temperature

Answer: (B)

In this context, two special points define the limits of liquid–gas equilibria on a pressure–temperature diagram. The cricondenbar marks the highest pressure at which a liquid and gas can coexist at any temperature. Above that pressure, only a single supercritical phase exists, so a separate gas or liquid cannot form regardless of how you vary the temperature. The temperature that corresponds to reaching that maximum pressure is the cricondenbar temperature—it's the temperature along that boundary where the two-phase region ends on the high-pressure side. This is different from the cricondentherm, which concerns the highest temperature at which liquid and gas can coexist at any pressure, or from the critical temperature, which is the temperature above which a gas cannot be liquefied by pressure alone (a different boundary on the phase diagram). Boiling temperature is simply the phase change between liquid and vapor at a specific pressure.

In this context, two special points define the limits of liquid–gas equilibria on a pressure–temperature diagram. The cricondenbar marks the highest pressure at which a liquid and gas can coexist at any temperature. Above that pressure, only a single supercritical phase exists, so a separate gas or liquid cannot form regardless of how you vary the temperature. The temperature that corresponds to reaching that maximum pressure is the cricondenbar temperature—it's the temperature along that boundary where the two-phase region ends on the high-pressure side.

This is different from the cricondentherm, which concerns the highest temperature at which liquid and gas can coexist at any pressure, or from the critical temperature, which is the temperature above which a gas cannot be liquefied by pressure alone (a different boundary on the phase diagram). Boiling temperature is simply the phase change between liquid and vapor at a specific pressure.