Step-by-step explanation:
The final temperature of the pot will be closer to the initial temperature of the pot rather than the initial temperature of the water. This can be explained by the principle of heat transfer and the equation for heat exchange:
Q = mcΔT
Where:
- Q is the heat transferred.
- m is the mass of the substance.
- c is the specific heat capacity of the substance.
- ΔT is the change in temperature.
Since the specific heat capacity of the metal pot is much lower than that of water, \(c\) is smaller for the metal pot than for water. Therefore, when heat is transferred from the hot water to the cold metal pot, the pot will heat up (or cool down) more quickly than the water will. This means that the final temperature of the pot will be closer to its initial temperature than to the initial temperature of the water.
In practical terms, this behavior is commonly observed when you put a hot metal pot under running cold water to cool it down quickly. The pot cools down faster than the water heats up because the metal has a lower specific heat capacity, allowing it to change temperature more rapidly.