Lab 09: Specific Heat Capacity and Calorimetry
Learning Objectives
- Determine the specific heat capacity of a metal sample or liquid.
- Apply conservation of energy to heat exchange in a calorimeter.
- Measure temperature change accurately and consistently.
- Identify heat losses to the surroundings and calorimeter as sources of error.
This placeholder is prepared for a complete laboratory experiment on calorimetry. It can be adapted for a metal-sample calorimetry activity, mixture method, electrical heating method, or cooling-curve comparison.
Heat transfer
Heat gained or lost by a body is related to mass, specific heat, and temperature change.
Variables
| Symbol | Description | Unit |
|---|---|---|
| heat transferred | J | |
| mass | kg | |
| specific heat capacity | J/(kg·K) | |
| change in temperature | K or °C |
Heat exchange principle
In an ideal insulated system, heat lost by the hot body equals heat gained by the cold body.
Suggested Apparatus
Placeholder procedure outline
- Measure the mass of the calorimeter, water, and test sample as required.
- Record the initial temperature of the water in the calorimeter.
- Heat the metal sample or test liquid to a known temperature.
- Transfer the hot sample quickly into the calorimeter.
- Stir gently and record the final equilibrium temperature.
- Use heat exchange equations to solve for the unknown specific heat capacity.
- Repeat trials and compare with reference values if available.
Data Table Placeholder
Safety note
Handle hot water, heated metals, and glassware carefully. Use tongs or insulated gloves when transferring heated samples.
To complete this lab
Add the calorimeter correction method if required, sample calculation, expected reference values, and post-lab questions about heat loss and thermal equilibrium.