This specific heat calculator solves Q = mcΔT for any one unknown — heat, mass, specific heat, or temperature change — with presets for water, ice, aluminum, iron, copper and more.
c Is Heat Capacity per Kilogram — Water Is the Outlier King
Mixtures reaching equilibrium (hot metal into cool water) are solved on our Calorimetry Calculator; this page is the single-substance engine underneath. Part of our Physics Calculators collection.
Worked Example (Verified)
- 2 kg of water warmed 10 °C (defaults): Q = 2 × 4,186 × 10 = 83,720 J ≈ 23.3 Wh — a kettle’s honest invoice for two litres through a small lift; to boiling from 20 °C it’s 8× that
- Why showers dominate energy bills: 40 L × 40 °C ≈ 6.7 MJ ≈ 1.86 kWh before losses — the arithmetic behind tank sizing
- Metal contrast: 2 kg of copper through 10 °C costs 7,700 J — water demands ~11× more heat for the same rise; cookware and coolant choices are this ratio at work
- Solving backwards: 83,720 J into 2 kg of water → ΔT = 10.00 °C, the round trip the solve-for modes automate
Where Q = mcΔT Stops
- Phase changes: at 0 °C and 100 °C water absorbs/releases latent heat at constant temperature — separate constants, no ΔT.
- c itself drifts with temperature (water’s is unusually stable; gases split into cp and cv).
- Mixtures share a final equilibrium temperature; single-substance math per component, then energy balance couples them.
- Real systems leak heat to the room — calorimetry’s eternal correction term.
Related Tools
- Calorimetry Calculator — mixture equilibrium temperatures
- Thermal Expansion Calculator — what the heat does to size
- Physics Calculators — the full collection
Frequently Asked Questions
How do you calculate heat with specific heat?
Q = m × c × ΔT. Two kilograms of water (c = 4,186 J/kg·°C) warmed 10 °C need 83,720 J ≈ 23.3 Wh. This calculator solves for any one of the four quantities with material presets included.
What is the specific heat of water?
4,186 J/kg·°C (1 cal/g·°C by the calorie’s original definition) — among the highest of common substances, courtesy of hydrogen bonding. It’s why coastal climates are mild, why water cools engines, and why heating bathwater is expensive.
Why do metals heat up so much faster than water?
Their c values are 5–30× smaller (copper 385, gold 129 J/kg·°C): per kilogram per degree they bank far less energy, so the same heat input moves their temperature much further. Dulong–Petit regularity hides underneath: per atom, solids store similar heat — heavy atoms just pack fewer per kilogram.
Does Q = mcΔT work for melting ice?
No — phase changes absorb latent heat at fixed temperature. Warming ice to 0 °C uses c(ice) = 2,090; melting it uses the latent heat of fusion (334 kJ/kg) with ΔT = 0; the meltwater then warms with c = 4,186. Three separate line items — the Calorimetry Calculator chains such processes.
What is the difference between heat capacity and specific heat?
Heat capacity (J/°C) belongs to a specific object; specific heat (J/kg·°C) is the per-mass material property tabulated in books — multiply by your object’s mass to get its heat capacity. This calculator works in the specific form throughout.
Is this specific heat calculator free?
Yes — free, instant, no sign-up.