Calorimetry involves the use of a calorimeter, which can be either a constant-pressure calorimeter or a bomb calorimeter.
The heat absorbed or released in a reaction can be calculated using the formula $q = mc\Delta T$ where $q$ is heat, $m$ is mass, $c$ is specific heat capacity, and $\Delta T$ is the change in temperature.
In an exothermic reaction, heat is released and the temperature of the surroundings increases; in an endothermic reaction, heat is absorbed and the temperature decreases.
A bomb calorimeter is typically used for combustion reactions and operates at constant volume.
The principle of conservation of energy underlies calorimetry: energy lost by one substance must be gained by another.
Review Questions
What are the two main types of calorimeters used in measuring heat transfer?
How do you calculate the amount of heat transferred using specific heat capacity?
What distinguishes an exothermic reaction from an endothermic reaction in terms of heat transfer?
Related terms
Enthalpy: A thermodynamic quantity equivalent to the total heat content of a system. It is equal to internal energy plus the product of pressure and volume.
Specific Heat Capacity: The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.
Bomb Calorimeter: A device used to measure the energy released during a combustion reaction at constant volume.