Heat Transfer Calculator
Find heat transfer using Q = mcΔT.
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Formulas
Q = mcΔTQ = heat (J), m = mass (kg), c = specific heat, ΔT = temperature change
Heat Transfer
Specific heats (J/kg·K): Water: 4186, Aluminum: 897, Iron: 449, Copper: 385, Air: 1005. Heating 1L of water by 100°C requires 418.6 kJ.
How Sensible Heat Is Calculated
The heat required to change the temperature of a substance depends on its mass, its specific heat capacity, and the temperature change:
Q = mcΔTQ is heat energy in joules, m is mass in kilograms, c is specific heat capacity (J/kg·K), and ΔT is the temperature change.
Specific heat is the energy needed to raise one kilogram of a material by one degree. Water's high specific heat (4186 J/kg·K) is why it heats and cools slowly compared with metals.
Worked Example
Heating 2 kg of water from 20 °C to 80 °C (ΔT = 60 K), c = 4186:
Q = 2 × 4186 × 60 = 502320 J ≈ 502 kJ
Specific Heat of Common Materials
| Material | c (J/kg·K) |
|---|---|
| Water | 4186 |
| Aluminium | 900 |
| Steel / iron | 450 |
| Copper | 385 |
| Air | 1005 |
Frequently Asked Questions
Does this include phase changes?
No. Q = mcΔT covers sensible heat (temperature change only). Melting or boiling requires latent heat, calculated separately as Q = mL.
Why does water resist temperature change?
Its high specific heat means a large amount of energy is needed per degree. This stabilises climates and makes water an effective coolant.
What is the difference between heat and temperature?
Temperature measures the average kinetic energy of particles; heat is the total energy transferred. A large cool object can hold more heat than a small hot one.