Final answer:
The question involves principles of heat transfer and thermal equilibrium in physics, where a hot pan and cold water reach the same temperature. The specific heat of water causes it to absorb more heat for a smaller temperature change, which explains why the equilibrium temperature will be closer to that of the water.
Step-by-step explanation:
The concept in question relates to the principles of heat transfer and the achievement of thermal equilibrium. When a hot material and a cold one come into contact in an insulated environment, they exchange heat energy until they reach the same temperature. This is a physical manifestation of the Law of Conservation of Energy, which states that energy cannot be created or destroyed in an isolated system.
Temperature Equilibration Example
Suppose you pour 0.250 kg of 20.0°C water into a 0.500-kg aluminum pan off the stove with a temperature of 150°C. In this scenario, the water will receive heat from the hot pan until both the water and pan reach the same temperature - that's when we say they've reached thermal equilibrium. The specific heat of water, which is high compared to many other substances, means that it absorbs more heat for a smaller change in temperature. This is why the equilibrium temperature will be closer to the initial temperature of the water than that of the pan.