Specific Heat Converter
Convert between different units of specific heat capacity for various materials
Select Material
Conversion Formula:
cal/(g·°C) = J/(g·°C) × 0.239
Thermal Properties:
Extremely high specific heat (approaching or exceeding water)
Application Example:
To heat 100g of this material by 50°C would require:
Calculated using the formula: Energy = Specific Heat × Mass × Temperature Change
Common Material Conversions
Understanding Specific Heat
Specific heat capacity is the amount of energy needed to raise the temperature of 1 gram of a substance by 1 degree Celsius. Materials with high specific heat (like water) require more energy to heat up and retain heat longer.
Practical Applications:
- Water has an exceptionally high specific heat (4.18 J/g°C), making it excellent for cooling systems and heat regulation
- Metals generally have low specific heat, heating up and cooling quickly
- Building materials like concrete and brick store heat well due to moderate specific heat
- Specific heat affects cooking times and heating/cooling efficiency
- Thermal mass in architecture relies on specific heat of materials
- Computer heat sinks use metals with low specific heat for rapid cooling
Formula and Units:
- Q = mc∆T where:
- Q = energy (joules)
- m = mass (grams)
- c = specific heat
- ∆T = temperature change (°C)
- SI unit: J/(g·°C) or J/(kg·K)
- Other common units: cal/(g·°C), BTU/(lb·°F)
- Water's specific heat is the reference point (4.18 J/g°C)
Thermal Engineering Tips:
Understanding specific heat is crucial for designing efficient:
Heating/Cooling Systems
Lower specific heat materials heat/cool faster but don't retain temperature
Energy Storage
Higher specific heat materials store more thermal energy per unit mass
Climate Control
Material selection impacts heating/cooling costs in buildings
Heat Exchange
Specific heat affects efficiency of heat exchangers in industry
Specific Heat by Material Category
Building Materials
Gases
Liquids
Metals
Minerals
Solids
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Thermal Response Visualized
Thermal Property
Exceptional thermal storage. Water has the highest common specific heat.
To heat 100g by 50°C requires:
Water has the highest common specific heat capacity
Heating/Cooling Comparison
This animation shows how quickly different materials change temperature
Common Applications
Ideal for: Heat sinks, rapid thermal response applications
Examples: Mercury thermometers, gold jewelry (heats/cools quickly)
Ideal for: Cookware, heating elements, radiators
Examples: Copper cookware, iron radiators, silver tableware
Ideal for: Building materials, thermal storage with moderate response
Examples: Concrete floors, brick walls, aluminum frames
Ideal for: Thermal regulators, heat storage, insulation
Examples: Water heating systems, ice thermal storage, ethanol cooling
Ideal for: Climate control, thermal buffering, heat capacity batteries
Examples: Water heating/cooling systems, thermal regulation
Used in heating/cooling systems, thermal regulation, climate control
Heating Time Comparison
Time needed to heat equal masses by 50°C with the same energy input:
Materials with lower specific heat require less energy to change temperature
Mobile tip: Swipe left or right on the unit dropdown to quickly change units, or use the arrow buttons
About the Specific Heat Converter
Convert between different units of specific heat capacity for various materials All conversions run instantly in your browser and nothing you enter is sent to a server.
Common Conversion Formulas
| From | To | Formula |
|---|---|---|
| Joules per gram-°C (J/(g·°C)) | Calories per gram-°C (cal/(g·°C)) | cal/(g·°C) = J/(g·°C) × 0.239 |
| Joules per gram-°C (J/(g·°C)) | Joules per kilogram-K (J/(kg·K)) | J/(kg·K) = J/(g·°C) × 1000 |
| Energy (Q) | Specific Heat (c), Mass (m), Temperature Change (ΔT) | Q = c × m × ΔT |