Heat corresponds to temperature in that a given quantity of heat
must be absorbed or lost for the temperature to change.
The quantity of heat that must be absorbed by an object to raise the temperature by 1 K is called the heat capacity.
Q
C = -----------
(Delta) T
C - Heat Capacity
Q - Quantity of Heat
T - Temperature (Kelvin)
When two items of different temperatures are placed in contact,
the system tends toward a common temperature.
When ice cubes are removed from a -20 C freezer, and placed in a glass of room temperature water, the temperature of the water will cool, and ice cubes will warm up to 0 C, melt, and then continue warming until their temperature equals the temperature of the cooling water.
Two calculations are needed, one to calculate the energy corresponding to the temperature decrease of the cooling water, and the other to calculate the energy corresponding to:
warming the ice cubes up to 0 C,
the energy needed to melt the ice cubes,
the energy needed to warm the water up to the final temperature.
As a problem, assume that 3.000 grams of ice at -20 C are added
to 8.000 ounces of water.