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A simple calorimeter, such as the one shown in Figure 12-7, is a device used to measure changes in Insulated outer thermal energy A calorimeter is carefully insulated container so that heat transfer to the external world is kept to a minimum A measured mass of a substance that has been heated to a high temperature is placed in the calorimeter The calorimeter also contains a known mass of cold water at a measured temperature The heat released by the substance is transferred to the cooler water The change in thermal energy of the substance is calculated using the resulting increase in the water temperature More sophisticated types of calorimeters are used to Inner measure chemical reactions and the energy content container of various foods The operation of a calorimeter depends on the conservation of energy in an isolated, closed system Energy can neither enter nor leave this system As a result, if the energy of one part of the system increases, the energy of another part of the system must decrease by the same amount Consider a system composed of two blocks of metal, block A and block B, shown in Figure 12-8a on the next page The total energy of the system is constant, as represented by the following equation Conservation of Energy EA EB constant



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And the code:

Figure 12-7 A calorimeter provides an isolated, closed system in which to measure energy transfer

In an isolated, closed system, the thermal energy of object A plus the thermal energy of object B is constant

Figure 12-8 A system is composed of two model blocks at different temperatures that initially are separated (a) When the blocks are brought together, heat flows from the hotter block to the colder block (b) Total energy remains constant





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Suppose that the two blocks initially are separated but can be placed in contact with each other If the thermal energy of block A changes by an amount EA, then the change in thermal energy of block B, EB, must be related by the equation, EA EB 0 Thus, EA EB The change in energy of one block is positive, while the change in energy of the other block is negative For the block whose thermal energy change is positive, the temperature of the block rises For the block whose thermal energy change is negative, the temperature falls Assume that the initial temperatures of the two blocks are different When the blocks are brought together, heat flows from the hotter block to the colder block, as shown in Figure 12-8b The heat flow continues until the blocks are in thermal equilibrium, which is when the blocks have the same temperature In an isolated, closed system, the change in thermal energy is equal to the heat transferred because no work is done Therefore, the change in energy for each block can be expressed by the following equation: E Q mC T

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