Question

Equal amounts of heat are added to equal masses of ice and iron at the same initial temperature. Which substance will have the higher final temperature?

How much greater will that temperature change be than the temperature change of the other substance?
larger ΔT / smaller ΔT =

Answer 1

i got u

Step-by-step explanation:

The iron will have the higher final temperature. This is because the specific heat capacity of iron is much lower than the specific heat capacity of ice. Specific heat capacity is the amount of heat energy required to raise the temperature of a substance by a certain amount, and it varies from substance to substance. Since the specific heat capacity of iron is lower, it means that it takes less heat energy to raise the temperature of iron than it does to raise the temperature of ice by the same amount. Therefore, when equal amounts of heat are added to equal masses of ice and iron at the same initial temperature, the iron will have a higher final temperature than the ice.