Calorimetry heat mixer

Calorimetry measures heat flow by watching temperature changes. In this simulation you mix a hot metal with water inside an insulated calorimeter and track every joule. Learning goals: apply q = mcΔT to both substances in a mixture; use energy conservation to find a final equilibrium temperature; explain why substances with different specific heats behave differently.

Mass of water: 100 gTemperature change: 10 °C

q = mcΔT = 100 × 4.184 × 10 = 4184 J

Heating 100 g of water by 10°C takes 4184 joules — about 1.00 food calories.

Controls

Metal selection: Chooses the metal block; each has its real specific heat.
Metal temperature: Sets the starting temperature of the hot metal.
Water temperature: Sets the starting temperature of the water bath.
Mass sliders: Adjusts the masses of metal and water.

The chemistry

q = mc\Delta T

Heat transferred

q_{\text{metal}} + q_{\text{water}} = 0

Energy conservation in the calorimeter

m_1c_1(T_f - T_1) = -m_2c_2(T_f - T_2)

Heat lost equals heat gained

Assumptions

The calorimeter is perfectly insulated, so no heat escapes.
No phase changes occur during mixing.
Specific heats are constant over the temperature range.

Guided activity

Drop hot copper into cool water and watch the temperatures converge.
Repeat with aluminum and compare the final temperature.
Double the water mass and observe how the result changes.
Predict the final temperature with q = mcΔT before running the simulation.

Challenge questions

Explain why the final temperature is closer to the water's start when water mass is large.
Calculate the heat lost by the metal and show it equals the heat gained by water.
Predict which metal gives the highest final temperature and test it.