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2 December, 08:42

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?

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  1. 2 December, 10:24
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    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
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