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Specific Heat Calculator

Find how much heat it takes to warm something (Q = m × c × ΔT), or solve for mass, specific heat or temperature change, with typical material values.

Level: Grades 9–10

Printable worksheet

Specific Heat Calculator

Know the answer you need? Pick an input to work backward.

Inputs
Solve for

Typical values near room temperature. Choose “Enter a specific heat” for an exact figure from your data sheet.

Final temperature minus starting temperature. Negative for cooling.

Result

Heat energy

627.6 kJ

Heat energy is 627.6 kJ.

In joules
627,600 J
In calories (thermochemical)
150,000 cal
In kilocalories
150 kcal
In watt-hours
174.3333 Wh
In kilowatt-hours
0.1743 kWh
In british thermal units (it)
594.85 BTU

See the step-by-step solution ↓

Step-by-step solution

  1. Look up a typical specific heat (c) for liquid water: the energy to warm 1 kg by 1 degree

    c=4,184 J/(kg·K)

  2. Multiply the mass (m) by the specific heat (c) and the temperature change (ΔT) to get the heat taken in (Q)

    2×4,184×75=627,600 J

  3. Change the answer to kJ, the unit you picked: divide by 1,000

    627,6001,000=627.6 kJ

Test yourself

20 quick questions built from this calculator's formula: work out results, predict what happens when an input changes, and work backward from an answer. Every answer comes with the working.

What this calculator does

Find out how much energy it takes to heat something up, or how much it will warm from the heat you give it. Specific heat capacity is the energy needed to warm one kilogram of a substance by one degree. Water's is unusually high, about 4,184 joules per kilogram per kelvin. That's why a pot of water takes so long to boil. It's also why lakes and oceans keep nearby weather milder. Metals, on the other hand, warm up quickly from very little energy.

This calculator uses the basic heat equation Q = m × c × ΔT. Q is the heat energy, m is the mass, c is the specific heat and ΔT ("delta T") is the temperature change. You can solve for any one of the four. Choose from typical values for common materials, or enter your own. Energy can be shown in joules, calories, kilowatt-hours or BTU.

Where it's used

Why this math matters outside the classroom:

  • Boiling water. Heating 1 kg of water from 20 °C to 100 °C takes about 1 × 4,186 × 80 ≈ 335 kJ.
  • Cooking. Cooks notice a metal pan heats far faster than the water in it because metal's specific heat is much lower.
  • Coastal climates. Geography classes explain mild coastal climates by water's high specific heat, which slows temperature swings.
  • Calorimetry. Chemistry students find a metal's specific heat by dropping it hot into water and recording the temperature rise.

Grade level and standards: Grades 9–10; Common Core State Standards for Mathematics HSA.CED.A.4. © Copyright 2010. National Governors Association Center for Best Practices and Council of Chief State School Officers. All rights reserved.

How to use it

  1. Choose which value to solve for.
  2. Pick a material for its typical specific heat, or choose to enter a specific heat yourself.
  3. Enter the other values you know, with their units. For cooling, use a negative temperature change or heat.
  4. Choose the unit for the answer. The result is also listed in other units.

What the inputs mean

Material
Preset values are typical figures near room temperature, and they're labeled that way. Specific heat changes with temperature and with the exact alloy or mixture. So use a data-sheet value when precision matters.
Heat energy (Q)
Positive heat means energy flows into the material. Negative means it flows out as the material cools.
Temperature change (ΔT)
A change of 1 °C is exactly the same size as a change of 1 K (one kelvin), so either works. A change of 1 °F is 5/9 of a kelvin. Enter the change, not the final temperature. For 20 °C to 95 °C, enter 75.

Formula and method

Q = m × c × ΔT
m = Q ÷ (c × ΔT)
c = Q ÷ (m × ΔT)
ΔT = Q ÷ (m × c)
1 cal = 4.184 J;  1 kWh = 3,600,000 J

Q is the heat energy, m is the mass, c is the specific heat and ΔT is the temperature change. The middle three lines are the same equation, turned around to solve for each of the others. The heat needed grows in step with the mass, the specific heat and the temperature change. Double any one of them, and the energy doubles.

Everything is changed to joules, kilograms and kelvins before the math. One calorie per gram per degree Celsius is 4,184 J/(kg·K). One BTU per pound per degree Fahrenheit is 4,186.8 J/(kg·K). That's why both are close to the value for water.

Worked example

How much energy does it take to heat 2 kg of water from 20 °C to 95 °C, as in an electric kettle?

  1. ΔT = 95 − 20 = 75 °C, which is 75 K.
  2. Q = m × c × ΔT = 2 × 4,184 × 75 = 627,600 J.
  3. In kilojoules: 627,600 ÷ 1,000 = 627.6 kJ.

Result: Heating the water takes 627.6 kJ, which is 150 kcal or about 0.174 kWh. That ignores heat lost to the kettle and the air.

Understanding the result

A large specific heat means a material stores a lot of energy per degree, so it heats and cools slowly. Water stores about ten times as much heat per kilogram per degree as copper.

If you know the energy a heater delivers, solving for ΔT shows the best-case temperature rise. Real rises are lower, because some heat always escapes.

Assumptions and limitations

  • The material doesn't melt, freeze, boil or condense over the temperature range.
  • The specific heat stays the same over the range.
  • All the heat goes into the material, with none lost to the surroundings.
  • Changes of state, such as melting or boiling, also need latent heat (energy that changes the state without changing the temperature). For example, it takes about 334 kJ/kg to melt ice, or about 2,260 kJ/kg to boil water. This equation doesn't include that.
  • Typical preset values can differ from your own sample by several percent.
  • For gases, the specific heat depends on whether the gas is held at constant pressure or constant volume. The air and steam presets are constant-pressure values.

Frequently asked questions

Why does water have such a high specific heat?

Water molecules are held to each other by hydrogen bonds. Much of the added energy goes into stretching and breaking those bonds, rather than speeding the molecules up. So the temperature rises slowly.

What is the difference between specific heat and heat capacity?

Specific heat is per kilogram (or gram), so it's a property of the material. Heat capacity is for a whole object: its mass times its specific heat. A full bathtub and a cup of water have the same specific heat. But their heat capacities are very different.

How do I find the final temperature?

Solve for the temperature change, then add it to the starting temperature. For cooling, the change is negative, so the final temperature is lower.

Can I use this for mixing hot and cold water?

Not directly, but it helps. In a mix, the heat lost by the hot water equals the heat gained by the cold water. When the specific heats are equal, the final temperature is a weighted average of the two starting temperatures. Each one counts in proportion to its mass.

How this calculator is checked

Method: Sensible-heat (calorimetry) equation Q = mcΔT. Thermochemical calorie 4.184 J and IT BTU 1,055.05585262 J (exact definitions). The calculation is covered by automated tests with known reference values and edge cases. Last updated 2026-10-18. Found a problem? Tell us.

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