An aluminum cup with mass 0.55 kg holds 0.81 kg of water. Both the cup and the water have a temperature of 25.87 °C. If a 0.67-kg piece of copper at 76.9 °C is added to the cup, what is the final equilibrium temperature in °C? You may assume that the cup, water, and copper are well insulated from anything else.
2007-12-04 11:55:32 · 1 answers · asked by lilprincess_2good4u 1 in Science & Mathematics ➔ Physics
Since no phase change is involved (nothing is melting/freezing, vaporizing/condensing) all you need to worry about is the specific heats of the various parts. You set up an equation where the heat lost by the Cu (Cp of Cu X mass of Cu X delta T) = the heat gained by the Al & water (CpAl X Mass Al X delta T + CpwaterXmass waterXdelta T.
Note that delta T for the Cu will not be the same as delta T for Al & water. Delta T for Al and water will be the same. The final temperature will be the same for all three.
For extra credit (maybe) you could argue that, if the Cu is well insulated from the water and the Al, there will be no change in temperature of anything.
good luck
2007-12-04 12:14:01 · answer #1 · answered by Gary H 7 · 0⤊ 0⤋