Temperature of water and copper?

Question

Type of metal: Copper

Mass of metal: 104g

Initial temperature of metal: 98.9 degrees C

Mass of water and calorimeter: 65.0g

Mass of empty calorimeter: 2.0g

Initial temperature of water: 22.0 degrees C

Final temperature of water: 33.5 degrees C

a. what was the final temperature of the copper object? Explain this answer as I do not understand.

b. Determine the temperature change, ANGLE t, of the copper object

c. dtermine the temperature change, ANGLE t, of the water.

d. if the specific heat capacity of water is 4.19 J/g- degrees C, what is the energy absorbed by the water? I am really confused!

e. determine the experimimental specific heat capacity of the copper.

Answer 1

The water takes 4.19 joules of energy to raise its temperature one degree C per gram of water.

There are 63 grams of it.

Its temperature was raised 11.5 degrees C.  That's the answer to c.

Therefore, it received 63 X 11.5 X 4.19 = 3036 joules of energy from a hot piece of copper.  That's the answer to d.

Take this amount of energy, divide it by the listed (in the textbook) specific heat capacity for copper, divide this result by 104 grams of copper, and you will have the "delta T;" the temperature drop experienced by the hot piece of copper.  That's the answer to b.

Subtract that delta T from 98.9 degrees, and you have the answer to a; the final temperature of the copper.

What apparently is not explicitly stated, is that the final temperature of both water and copper are the same; 33.5 degrees C.

If you think that the problem is worded to imply that the final temperature of the copper is (likewise) 33.5 degrees C, then you have sufficient information to solve for the answer to e.  Otherwise, you must use the textbook's value to get the answer to a.