Calorimeter
Definition
A calorimeter is a device used to measure the amount of heat transferred to or from an object, often during chemical reactions or physical changes. It typically consists of an insulated container that minimizes heat exchange with the environment.
5 Must Know Facts For Your Next Test
- Calorimeters operate on the principle of conservation of energy, where the heat lost by one substance is equal to the heat gained by another.
- There are different types of calorimeters, including bomb calorimeters for combustion reactions and coffee cup calorimeters for simpler experiments.
- The specific heat capacity of a substance can be determined using a calorimeter by measuring temperature changes when mixing substances with known masses and initial temperatures.
- The formula \( q = mc\Delta T \) is crucial in calorimetry calculations, where \( q \) is the heat absorbed or released, \( m \) is mass, \( c \) is specific heat capacity, and \( \Delta T \) is the change in temperature.
- Calorimeters must be well-insulated to ensure accurate measurements by preventing external heat exchange.
Review Questions
- What principle do calorimeters operate on?
- How can you use a calorimeter to determine the specific heat capacity of a substance?
- Why is insulation important in a calorimeter?
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Related terms
Specific Heat Capacity: The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.
Heat Transfer: The process by which thermal energy moves from one object or substance to another due to temperature differences.
Bomb Calorimeter: A type of constant-volume calorimeter used in measuring the energy produced by combustion reactions.
