Calorimetry is a quantitative measurement technique used to assess the amount of heat absorbed or released during a chemical reaction or a physical change. It is fundamental in thermodynamics, allowing scientists to understand the energy exchanges that occur. By measuring temperature changes in a controlled setting, calorimetry provides insights into reaction enthalpies, specific heat capacities, and other thermodynamic properties. This technique is widely applicable, including in reactions involving solids, liquids, and gases, making it essential for studying both endothermic and exothermic processes.
The other options focus on aspects unrelated to heat exchange. For instance, measuring temperature changes in solids only would limit the scope of calorimetry, as it applies to all states of matter. Determining the concentration of a solution is related to analytical chemistry but does not involve calorimetric principles. Analyzing the composition of a gas also deviates from the calorimetric purpose, which specifically concentrates on thermal energy changes rather than chemical composition. Ultimately, the primary function of calorimetry is to track the thermal energy changes associated with reactions, confirming that measuring heat absorbed or released truly captures the essence of the technique.