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Asked by Rajaram Last Modified
Answer Ice at 273 K (0°C) is more effective in cooling than water at the same temperature because of the process of phase change involved.
When ice absorbs heat energy, it undergoes a phase change from solid to liquid, known as melting. This process requires a significant amount of energy, known as the latent heat of fusion, to break the hydrogen bonds holding the water molecules together in the solid state. As a result, the ice absorbs heat energy from its surroundings to undergo this phase change, leading to cooling of the surroundings.
On the other hand, water at the same temperature does not undergo a phase change when it absorbs heat energy. Instead, it absorbs the heat energy primarily through an increase in temperature, which leads to a relatively smaller decrease in the temperature of the surroundings compared to the phase change involved in melting ice.
Therefore, ice at 273 K is more effective in cooling than water at the same temperature because it absorbs more heat energy from its surroundings due to the phase change involved in melting, whereas water primarily absorbs heat energy through an increase in temperature.
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