This is on a practise exam I have and I cant get part of it, I don't know if it is not only due to my not understanding but to the fact that the first two parts might be wrong. Thanks for your help if you can. Heres the question:

A coffee-cup calorimeter normally consists of two nested styrofoam cups with a lid. A coffee-cup calorimeter of this type contains 125.0 g of water at 20.00 degrees C. A 120.0 g sample of copper metal is heated to 98.50 degrees C by putting it into a beaker of hot water. The copper is then put into the calorimeter and the final temperature of the water and copper is 25.80 degrees C.
A) Calculate the energy change of the copper metal.
For this answer I got -3358.74J
B) Calculate the energy change of the water.
For this I got 3033.40J
C) The difference between the two values is due to energy lost to the styrofoam cups. The heat capacity of a calorimeter is the amount of energy required to change the temperature of the apparatus by 1 degree C. Calculate the heat capacity of the calorimeter in J/degrees C.
This one im stuck.
D) In a typical coffee-cup calorimeter we assumer that the energy change due to the calorimeter is negligible. In this experiment is this a vaild assumption? Exaplin.
I;m assuming this might be easier to asnswer once I get part C

For C, heat capacity = q/delta T.
I will let you ponder D.

Oh I know that much, sorry I didn't clarify that, what I don't know is, do you subtract A from B to get q or vice versa?

Would it matter? You know heat is being added to the cup so you know heat difference must be + so subtract "any old way" and stick a + sign in front of the difference. However, if you want an equation remember that

EH2O + ECu + Ecup = 0
3033.4J - 3358.74 + heatcap x delta T = 0

To clarify with parenthese:
EH2O + ECu + Ecup = 0
3033.4J - 3358.74 + (heatcap x delta T) = 0

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