Calorimetry calculator

How to use (3 steps)

Select the mode: single object or mixing two substances.
Enter mass, specific heat, temperatures, or heat. Keep units consistent (kg with J/(kg·K) or g with J/(g·K)).
Press Compute to see the solved value, the full table, and the step-by-step energy balance. Copy URL shares the setup.

Default example: heat 0.10 kg of water from 20 °C to 80 °C (solve for Q). The initial calculation runs automatically.

Inputs

Mode

Single: heat, mass, specific heat, temperature change Mixing: final temperature of two substances

Pick the unknown and leave it blank; the other fields should be filled. For ΔT mode, leave Tf empty to solve ΔT (if you enter Tf, it only checks consistency).

Heat Q Mass m Specific heat c Temperature change ΔT (Tf optional)

Mass m kg

Specific heat c J/(kg·K)

Initial temperature Ti °C

Final temperature Tf °C

Heat Q J Solved automatically

Results

Single-object calorimetrySolved Q = 25104 J

Temperature change ΔT60 °C

Heat Q25104 J

Positive Q heats the sample; negative Q means the sample releases heat. Q > 0: heat absorbed.

Single-mode values
Mass m	0.1 kg
Specific heat c	4184 J/(kg·°C)
Temperature change ΔT	60 °C
Heat Q	25104 J

How it's calculated

Use mass m = 0.1 kg, specific heat c = 4184 J/(kg·°C), initial temperature 20 °C, and final temperature 80 °C.
The temperature change is ΔT = 80 − 20 = 60 °C.
Apply Q = m c ΔT, giving Q = 0.1 × 4184 × 60 = 25104 J.

FAQ

Can this handle phase changes such as melting or boiling?

This calculator assumes constant specific heat and no phase change. To model melting or evaporation, add the latent heat separately.

How should I align the units?

Use matching units such as kg with J/(kg·K) or g with J/(g·K). Mixing units (e.g., kg with J/(g·K)) will give incorrect results. Temperatures may be in °C or K because only differences are used, so ΔT is identical.

Does it consider heat loss to the surroundings?

Mixing mode assumes an insulated system with no heat loss to the container or air. Real experiments may differ because of heat loss or the container's heat capacity.

What should I enter first for a calorimetry run?

Start with mass, temperature change, and the known heat or specific heat value. Keep units consistent so the calculated heat capacity or specific heat reflects the experiment setup.

Why can a calorimetry run results differ from nearby tools?

Differences usually come from mass, heat, temperature change, and heat-loss assumptions. Match those assumptions before comparing this result with another CalcBE page, spreadsheet, or external tool.

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