CHM047 · Thermochemistry · Classes 8–12
Specific Heat Comparison
Objective: To compare how different materials warm up when given the same heat.
🧰 Virtual materials and apparatus
- Virtual blocks of water, aluminium, copper and iron
- Equal heater input
📐 Formulas and SI units
ΔT = q / (m c)
c (J/g °C): water 4.18, Al 0.90, Cu 0.385, Fe 0.45
💡 Theory
Specific heat capacity c tells how much energy warms 1 g by 1 °C. With the same heat and mass, a material with a small c warms more: ΔT = q/(mc). Water's high specific heat keeps coastal climates mild and makes it a good coolant; copper warms up quickly.
🪜 Guided virtual procedure
- Give 1000 J to 100 g of each material.
- Compare the glow (temperature rise) of the blocks.
- Read ΔT for aluminium.
- Change the mass and heat.
- Rank the materials.
📋 Observations Simulated values
✅ Result and conclusion
1000 J warms 100 g of aluminium by 11.1 °C, but 100 g of water by only 2.4 °C.
🔬 Real lab vs simulation
Real blocks lose heat to the air while being heated. (Physics link: PHY032.)
⚠️ Safety
Simulated heating only. Hot metal blocks burn; real heating is done only by teachers.
❓ Quick check
1. Which warms most for the same q and m?
2. Why is water used in car radiators?
3. ΔT for 418 J into 10 g water?
🏋️ Practice
EasyΔT for 1000 J into 100 g copper?
Answer: 26.0 °C
MediumHeat to warm 50 g iron by 20 °C?
Answer: 450 J
ChallengeWhich has the highest c here?
Answer: Water