.:The Introduction to Calorimeter:.

A calorimeter is a device for calorimetry, the science of measuring the heat of chemical reaction or physical changes as well as heat capacity. The word calorimeter is derived from the Latin word 'calore', meaning heat. Differential scanning calorimeters, isothermal calorimeters, titration calorimeters and accelerated rate calorimeters are among the most common types. A simple calorimeter just consists of a thermometer attached to a metal container full of water suspended above a combustion chamber.

To find the enthalpy change per mole of a substance A in a reaction between two substances: A and B, the substances are added to a calorimeter and the initial and final temperatures (before the reaction started and after it has finished) are noted. Multiplying the temperature change by mass and specific heat capacities of the substances gives a value for the energy given off or absorbed during the reaction. Dividing the energy change by how many moles of A were gives its enthalpy change of reaction. This method is used primarily in academic teaching as it describes the theory of calorimetry. It does not account for the heat loss through the container or the heat capacity of the thermometer and container itself. In addition, the object placed inside the calorimeter show that the object transferred their heat to the calorimeter and into the liquid, and the heat absorbed by the calorimeter and the liquid is equal to the heat given off by the metal.

Figure: Bomb Calorimeter