Measure the heat energy released by burning food samples (peanuts, candles) using a simple calorimeter.
Observe how different fuels release different amounts of energy.
Calorimeter Setup
25°C
Peanut
Candle
Observation:
Select a fuel source to burn and measure its heat of combustion.
The Science Behind Calorimetry
Calorimetry Principle:
q = m × c × ΔT
Where:
q = heat energy (J)
m = mass of water (g)
c = specific heat capacity of water (4.18 J/g°C)
ΔT = temperature change (°C)
Experimental Setup:
Known mass of water in calorimeter
Measure initial temperature
Burn known mass of fuel beneath calorimeter
Measure temperature change
Calculate energy released per gram of fuel
Typical Energy Values:
Fuel Source
Energy (kJ/g)
Composition
Peanut
~24
Fats, proteins, carbohydrates
Candle Wax
~42
Long-chain hydrocarbons
Wood
~16
Cellulose, lignin
Coal
~30
Carbon, hydrocarbons
Key Concepts:
Heat of Combustion: Energy released when 1g of substance burns completely
Exothermic Reaction: Releases heat energy to surroundings
Energy Content: Depends on chemical bonds in the fuel
Calorimeter: Device that measures heat changes
Real-World Applications:
- Food energy content (nutrition labels)
- Fuel efficiency comparisons
- Bomb calorimetry for industrial testing
- Energy content of biofuels
- Fire safety and flammability testing
