a 0.10kg piece of copper at an initial temperature of 95C is dropped into 0.20kg of water contained in a 0.28kg aluminum calorimeter. the water and calorimeter are initially at 15C. what is the final temperature of the system when it reaches equilibrium?

Use the law of conservation of energy and assuming no heat loss to the surroundings, then

Heat given up by copper = heat absorbed by water + heat absorbed by calorimeter

Working formula is

Q = heat = MCp (delta T)

where

M = mass of the substance

Cp = specific heat of the substance

delta T = change in temperature

Heat given up by copper = 0.10 (387) (95 - T)

Heat absorbed by water = 0.20 (4186) (T - 15)

Heat absorbed by calorimeter = 0.28 (899) (T - 15) /

where

T = final temperature of the system

Substituting appropriate values,

0.10 (387) (95 - T) = 0.20 (4186) (T - 15) + 0.28 (899) (T - 15)

38.7 (95 - T) = 1088.92 (T - 15)

3676.50 - 38.7T = 1088.92T - 16333.8

1127.62T = 20010.3

T = 17.75 C