Calorimetry
1.0 Introduction
1.0 Introduction
Heat
Two bodies at a different temperature, when brought into contact, the hot body loses its hotness and the cold body loses its coolness.
Thus there may be an energy transfer between the layers in contact. The energy is transferred between the layers or the bodies at different temperature due to the difference in their temperature is called heat.
Therefore, heat is a form of energy. It is the energy which is transferred whenever temperature difference exists. As the transfer is finished, it becomes the internal energy of the body. We should clearly understand, that the word "heat" is meaningful only as long as the energy is being transferred.
The unit of heat is $Joule$ in SI system.
In CGS system, it is measured in $Calorie$.
The calorie is defined as " the amount of heat needed to raise the temperature of 1$g$ of water from ${14.5^o}C$ to ${15.5^o}C$ at an atmospheric pressure of $1 atm$.
Generally, we will define the calorie as, the amount of heat required to raise the temperature of 1$g$ of water through ${1^o}C$,
A calorie is also represented as $Cal$.
$$1\;calorie = 4.186\,joule$$
Calorimetry
The process of measurement of heat exchange between the bodies and the system is called calorimetry.
A simple calorimeter is a vessel generally made of copper with a stirrer made of same material. The vessel is generally kept in a wooden box to isolate it thermally from the surroundings.
