Boyle’s Law Lab 3D

Compress a fixed amount of gas at constant temperature

Paused • 3.00 L

Drag the piston • Drag background to pan • Wheel or pinch to zoom • Tap objects to track

Mission: discover the inverse relationship

Keep temperature and gas amount fixed. Halve the volume and observe what happens to pressure.

Simulation speed1×

Gas controls

Volume3.00 L

Temperature300 K

Hold temperature constant for Boyle’s law

83.1pressure kPa

249.4P × V kPa·L

—wall hits / s

At 3.00 L, molecules have room to travel. Compressing the gas shortens their path, so wall collisions become more frequent and pressure rises.

Quick experiments

Prediction: if volume halves at constant temperature, pressure should double.

Pressure–volume evidence

PressureP × V● current state

Tracked object

No object selected

TipTap piston or molecule

Camera

Zoom100%

Teacher controls

Gas amount0.100 mol

Show force and collision labels

Teacher-guided complete lecture

Language

Voice source

Voice

Narration speed1×

Ready0%

What to watch: the piston, particle spacing, pressure gauge, and graph.

Choose a language and voice, then start the complete lecture. Every chapter controls the simulation and demonstrates the spoken idea on the canvas.

Ready. Narration will not start automatically.

Chapters

Learning objectives

Describe the inverse relationship between pressure and volume.
Use P₁V₁ = P₂V₂ for a fixed gas amount at constant temperature.
Explain pressure using molecular collisions with container walls.
Read a pressure–volume graph and recognize a hyperbola.
Apply Boyle’s law to syringes, breathing, pumps, and diving bubbles.

Key concepts demonstrated

Pressure

Molecules transfer momentum when they strike walls. More frequent impacts per area mean greater pressure.

Volume

The piston changes the space available without changing the amount of gas.

Constant temperature

When temperature is fixed, average molecular kinetic energy stays approximately constant.

Constant product

For an ideal gas with fixed amount and temperature, pressure multiplied by volume is constant.

Plain-language explanation

Reducing volume gives gas molecules less distance to travel before striking a wall. At the same temperature they keep the same average speed, so collisions occur more often. Pressure rises. Expanding the volume does the opposite.

Scientific model: the readout uses the ideal-gas relationship P = nRT ÷ V. The animated particles are a conceptual sample, not the actual number of molecules. Their drawn sizes and speeds are visually scaled.

Suggested experiments

Set 4.00 L, record pressure, then compress to 2.00 L.
Try five volumes and check whether P × V remains nearly constant.
Unlock temperature to see why Boyle’s law requires constant temperature.
Compare the graph path during slow compression and expansion.

Questions for exploration

Why is the pressure change larger near very small volumes?
What happens if the gas amount doubles?
How would real-gas behavior differ at extreme pressure?

Real-world applications

Syringe: pulling the plunger increases volume and lowers internal pressure.
Breathing: chest expansion increases lung volume and lowers pressure, drawing air inward.
Bicycle pump: compression raises gas pressure and temperature.
Diving bubbles: lower surrounding pressure near the surface lets bubbles expand.

Common misconceptions

Molecules do not grow when volume increases; spacing changes.
Pressure does not rise because molecules become heavier.
Boyle’s law does not apply unchanged when temperature or gas amount changes.
The graph is curved, not a straight decreasing line.

Score: 0 / 7