A 0.10 kg piece of copper at an initial temperature of 95°c is dropped into 0.20 kg of water contained in a 0.28 kg aluminum calorimeter. the water and calorimeter are initially at 15°c. what is the final temperature of the system when it reaches equilibrium? show your work.
(cp of Copper = 387J / kg times degrees C; cp of Aluminum = 899 J / kg times degrees C; cp of Water = 4186J / kg times degrees C) 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,
