Consider a shallow body of water. Is it possible for this water to freeze during a cold and dry night even when the ambient air and surrounding surface temperatures never drop to \(0^{\circ} \mathrm{C}\) ? Explain.

The transition of matter from one state to another, such as from liquid to solid, is known as a phase change. In the context of water, the phase change we are most interested in is freezing, where water turns into ice. This typically occurs at the freezing point of water, which is conventionally \(0^{\textdegree} \text{C}\) under standard atmospheric pressure. However, several factors can alter this temperature, a concept known as freezing point depression.

During a phase change, the temperature of the substance remains constant while the state change is in progress. This allows for the latent heat, or the hidden energy, to facilitate the change in state rather than altering the temperature. For water to freeze, it must release its latent heat to the environment, which can happen even if the ambient temperature is above \(0^{\textdegree} \text{C}\) under certain conditions, such as a cold and dry night with high rates of evaporation.

Evaporation cooling is a natural phenomenon where a liquid absorbs heat from its surroundings as it transitions into a gas, resulting in a cooler environment. This effect is commonly experienced when sweat evaporates from the skin, making us feel cooler on hot days.

Role in Freezing Water

On a cold, dry night, a shallow body of water can be significantly affected by evaporation cooling. As water molecules at the surface gain enough energy to escape into the air, they take heat with them, which reduces the temperature of the remaining liquid. This process can accelerate the cooling of the water body, potentially bringing its temperature below \(0^{\textdegree} \text{C}\) despite higher ambient temperatures, leading to freezing.

It is important to note that evaporation rate—and thus the cooling effect—is greater when the air is dry because dry air has a higher capacity to take in more water vapor. This is why the problem specified the conditions as 'cold and dry' night, which are ideal for rapid evaporation and subsequent cooling.

Supercooling is a state where a liquid remains liquid below its normal freezing point without becoming a solid. This often happens to pure water, which can be chilled well below \(0^{\textdegree} \text{C}\) without freezing, provided there are no impurities or disturbance to serve as nucleation sites for ice crystals to form.

Water Supercooling

Even in the absence of evaporation cooling, supercooling can occur in a shallow body of water. Factors contributing to supercooling include the absence of impurities and a perfectly still environment. It is a delicate balance because even slight disturbances can cause the supercooled water to suddenly freeze. Supercooling is a common reason why water might freeze at temperatures slightly above \(0^{\textdegree} \text{C}\) or not freeze at temperatures well below it until a disturbance triggers the rapid formation of ice.