Specific heat capacity is the energy needed to warm 1 kg of a material by 1 °C, through Q = m·c·ΔT. Drag the heat energy slider to pour the same energy into 1 kg each of water, aluminium and iron, then watch how differently they warm.
Specific Heat Lab
Pour the same energy into 1 kg of each material and watch how differently they warm. Low specific heat = fast to heat.
Q = m · c · ΔT → ΔT = Q / (m·c). Equal Q and equal mass (1 kg) mean a smaller c gives a bigger temperature rise.
What Is the Specific Heat Simulator?
The specific heat simulator is a free interactive physics lab that runs in your browser — nothing to install and no sign-up. Add the same energy to equal masses of water, aluminium and iron and watch them reach different temperatures.
| Control | Range | Step |
|---|---|---|
| Heat energy added to each 1 kilogram sample | 0 – 50000 J | 500 |
Same Energy, Three Different Temperatures
Pour an identical dose of heat into equal 1 kg blocks of water, aluminium, and iron, and they finish at three different temperatures. That is the whole point of this simulator: the single Heat energy Q slider (in joules) feeds the same Q into all three samples when you press Start heating, and the readouts show how far each one climbs from its shared 20°C start. Nothing else varies. The masses are locked at 1 kg and the materials are fixed, with their specific heat capacities printed beside them: water c = 4186, aluminium c = 900, iron c = 450 J/kg·°C.
The governing relation is Q = m·c·ΔT, rearranged to ΔT = Q/(m·c). Because Q and m are shared, the temperature rise is decided entirely by c: a smaller specific heat yields a larger jump. So iron, with the lowest c, ends up hottest; aluminium lands in the middle; water rises the least. Slide Q higher and every ΔT scales with it, since for a fixed mass the rise is proportional to Q and inversely proportional to c.
Water's large c is why it heats slowly and cools slowly, soaking up plenty of energy per degree, and why it works as a coolant and the ocean tempers coastal climates. Watch the three bars diverge, then check your reading against the specific heat calculator or step sideways into another hands-on model at our collection of physics simulators.
Frequently asked questions
What is specific heat capacity?
Specific heat capacity is the energy needed to raise 1 kg of a substance by 1 °C. It links heat, mass and temperature rise through Q = m·c·ΔT.
Given the same energy and equal masses, which material heats up most?
The one with the lowest specific heat. In this lab iron (c = 450) rises the most, aluminium (c = 900) less, and water (c = 4186) the least, because ΔT = Q/(m·c) — a smaller c gives a bigger temperature rise.
Why does water heat up so slowly?
Its specific heat is high, so it soaks up a lot of energy for each degree of rise — and gives that energy back slowly too. That large capacity is why water is used as a coolant and why the sea moderates coastal climates.
What does the temperature rise depend on?
On the energy added, the mass, and the specific heat: ΔT = Q/(m·c). For a fixed mass, more energy means a bigger rise, while a higher specific heat means a smaller one.
References & formula source
- Halliday, Resnick & Walker — Fundamentals of Physics, Chapter 18 (Temperature, Heat, and the First Law).
- Young & Freedman — University Physics with Modern Physics, §17.5 (Calorimetry and Specific Heat).
- R. Nave — HyperPhysics, Georgia State University, "Specific Heat" section.
- Further reading: Specific heat capacity — Wikipedia