Mix 200g of copper at 90 degrees C with 500g of water at 20 degrees C.?
The final temperature is 22.4 degrees C.
The temperature change of water is -2.44 degrees C and the temperature change of copper is 67.56 degrees C.
How much heat energy (q) did the water gain?
What is the specific heat (c) of copper?
- hcbiochemLv 71 month agoFavourite answer
I think you've got a few typos in your question. The final temperature must be 22.44 C which give the water a temperature change of +2.44 C since it gains heat.
qwater = m c (T2-T1)
q = 500 g (4.184 J/gC) (22.44 - 20.00) = 5104 J
So, the copper must have lost -5104 J.
For the copper:
q = m c (T2-T1)
-5140 J = 200 g (c) (22.44 - 90.00)
c = 0.378 J/gC