CP12 Particle model mind map

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Density

States: Solid fixed / close; liquid flows / close; gas spaced / compressible
Equation: ρ = m/V; kg/m³ or g/cm³; 1 g/cm³ = 1,000 kg/m³
Mass / volume: Mass conserved; expansion lowers density; ice is less dense than water
Solid practical: Mass by balance; regular dimensions / submerged displacement
Liquid practical: Subtract container mass; measure volume at eye level; repeat
Example: 54 g ÷ 20 cm³ = 2.7 g/cm³ = 2,700 kg/m³

Heating

Temperature / energy: Mean kinetic energy / total particle kinetic + potential energy
Heat capacity: c in J/(kg K); ΔQ = mcΔθ; 1 °C change = 1 K change
Comparison: 0.5 × 4,200 × 10 = 21,000 J; greater c needs more energy
Water practical: Insulate / lid; measure m, Δθ and E = VIt; c = E/(mΔθ)
Measurement limits: Stir, immersed low-voltage heater; heat loss can overestimate c
Ice graph: Near 0 °C while pure ice melts; afterwards water warms

State changes

Physical processes: Melt / freeze; vaporise / condense; sublime / deposit
Plateau: Pure sample: potential energy changes, temperature constant
Latent heat: L in J/kg; Q = mL; fusion / vaporisation differ
Stages: Warming: mcΔθ; state change: mL; add separate energies
Cooling / escape: Freeze / condense release energy; evaporation only at surface

Gas pressure

Wall collisions: Pressure Pa = force/area; particles strike walls
Fixed volume: Higher T → faster particles → more frequent / stronger impacts
Absolute zero: Ideal extrapolation ≈−273 °C = 0 K; real gases condense
Kelvin: T = θ + 273; 20 °C ≈293 K; differences do not need +273
Limits: Finite particles, attractions and phase changes limit simple model

Connections

Density → Gas pressure: Particle motion and spacing explain state and pressure.
Heating → State changes: Heating changes temperature or causes a state change.