Safety boundary
Use virtual calorimetry or teacher-supervised water-based calorimetry only. No unsupervised flames, reactive chemicals, or improvised heat sources.
Explicit chemistry instruction
For a substance with approximately constant specific heat, q=mcΔT.
Mass must match the units of specific heat, and ΔT=T_final−T_initial.
In simple calorimetry, heat lost by one part is approximated as heat gained by another when container/environment losses are negligible.
Vocabulary: calorimetry; specific heat; temperature change; energy conservation.
Worked example
100 g water warms by 5.0°C. With c=4.18 J/(g·°C), q=100×4.18×5.0=2090 J.
Guided question
A 50 g water sample cools by 8°C. Calculate q for the water and interpret the sign.
Independent work
- Solve four q=mcΔT problems.
- Perform a unit/sign audit.
- Write one assumption behind ideal calorimetry.
Misconception check
A negative ΔT does not mean negative temperature; it means the sample cooled.
Formative check
What determines the sign of q in q=mcΔT?
Reveal response
The sign of ΔT under the chosen convention.
Mentor evidence conference
Ask Archaemenes to audit signs, units, system boundaries, and whether the evidence supports the energy claim.
Teacher guidance
Foundation: Use a calculation scaffold.
Core: Solve and interpret calorimetry data.
Extended: Estimate uncertainty from temperature resolution.