Calorimetry Heat Transfer Calculator
Calculate heat absorbed or released using q = mcΔT.
Supports coffee-cup calorimetry for reactions.
Includes common specific heat values.
Heat Transfer
Calorimetry measures heat flow in chemical and physical processes.
The fundamental formula:
q = m × c × ΔT
Where:
- q = heat transferred (joules, J)
- m = mass (grams)
- c = specific heat capacity (J/g·°C)
- ΔT = T_final − T_initial (degrees Celsius or Kelvin — same difference)
Coffee-cup calorimetry: For a reaction occurring in aqueous solution:
q_reaction = −q_solution = −m_solution × c_solution × ΔT
Assuming c_solution ≈ 4.18 J/g·°C (dilute aqueous solution ≈ water).
Specific heat capacities (c) at 25°C:
| Substance | c (J/g·°C) |
|---|---|
| Water (liquid) | 4.184 |
| Ice | 2.09 |
| Steam | 2.01 |
| Ethanol | 2.44 |
| Aluminum | 0.897 |
| Iron | 0.449 |
| Copper | 0.385 |
| Lead | 0.128 |
| Gold | 0.129 |
| Glycerol | 2.43 |
| Sand/silica | 0.835 |
Sign convention:
- q > 0: system absorbs heat (endothermic)
- q < 0: system releases heat (exothermic)
Converting units:
- 1 calorie (cal) = 4.184 J
- 1 food Calorie (kcal) = 4184 J
- 1 BTU = 1055.06 J
Molar enthalpy: If the number of moles is known, the molar enthalpy change:
ΔH = q / n (kJ/mol)