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Calorimetry
Beginner
Heat lost equals heat gained in an isolated mixture.
In an insulated mix, heat lost by hot parts equals heat gained by cold parts: Σmc ΔT = 0. It lets you find specific heats or final temperatures.
200 g of water at 80 °C mixed with 300 g at 20 °C: T_f = 44 °C.
Remember to include the calorimeter's heat capacity.
In more detail
Calorimetry measures heat transfers by mixing substances at different temperatures and applying energy conservation. The heat lost by hot objects equals the heat gained by cold ones.
Real-world uses
- Food scientists measure energy content of foods using calorimeters.
- Labs use calorimetry to measure reaction energies.
- A student mixes hot and cold water in a calorimeter to measure the specific heat of a metal.
Open the interactive lesson, with simulation and quiz →
Frequently asked questions
What is the key assumption?
That no heat is lost to the surroundings, which real experiments try to minimise.
How do I set up a calorimetry problem?
Write heat lost equals heat gained, using mass times specific heat times temperature change for each.
What assumption does calorimetry rely on?
That the mixture is isolated, so all the heat lost by one part is gained by the other, with no heat leaking away.
Related topics in Heat & Thermodynamics
Specific heat capacity · Molar heat capacity · Latent heat · Phase diagrams · Triple and critical points · Conduction