What occurs if a liquid temperature is below the superheat limit?

When the temperature of a liquid is below the superheat limit, the correct response is that energy is released from vapor expanding above the liquid. In this context, the superheat limit refers to the maximum temperature that a liquid can reach before it begins to undergo a phase change into a gas, or vapor. If the temperature remains below the superheat limit, the vapor that exists above the liquid does not have enough energy to convert the liquid into gas rapidly.

In this situation, vapor can exist in equilibrium with the liquid, and when it expands, it can release energy back into the liquid. This process can help maintain the stability of the system and prevent rapid vaporization or boiling, which occurs when the temperature exceeds the boiling point. The equilibrium between the liquid and vapor phase allows for energy transfer without leading immediately to a volatile reaction, such as an explosion, as seen in superheated states.

The other options do not accurately describe the dynamics of temperature below the superheat limit. Rapid vaporization would only happen once the boiling point is reached, while boiling is not impossible; it just requires specific conditions that might not exist at lower temperatures. Cooling is not initiated due to lowered temperature; instead, it refers to a different physical process altogether.