On a phase diagram, this is defined as the maximum temperature above which liquid cannot be formed regardless of pressure.

On a phase diagram, this is defined as the maximum temperature above which liquid cannot be formed regardless of pressure.

• A. Cricondentherm
• B. Critical Temperature
• C. Boiling Point
• D. Triple Point

Answer: (A)

The key idea is the limit where a liquid can exist at all. On a phase diagram, the liquid phase persists only up to the temperature where the liquid–vapor boundary ends—the critical temperature. At and above this temperature, the liquid and vapor phases become indistinguishable, so a true liquid cannot form regardless of pressure. The other terms relate to different ideas: the boiling point depends on pressure, the triple point is where solid, liquid, and vapor coexist, and the cricondentherm is tied to the highest temperature at which liquid and vapor can be in equilibrium along their boundary. The statement described matches the critical temperature most directly.

The key idea is the limit where a liquid can exist at all. On a phase diagram, the liquid phase persists only up to the temperature where the liquid–vapor boundary ends—the critical temperature. At and above this temperature, the liquid and vapor phases become indistinguishable, so a true liquid cannot form regardless of pressure. The other terms relate to different ideas: the boiling point depends on pressure, the triple point is where solid, liquid, and vapor coexist, and the cricondentherm is tied to the highest temperature at which liquid and vapor can be in equilibrium along their boundary. The statement described matches the critical temperature most directly.