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Exit to A Level Thermal Physics Hub

Ideal Gas & Thermodynamic Processes Explorer

Compare state changes, p-V graphs, and thermal processes so gas-law shortcuts, work, and internal-energy reasoning stay aligned.

  • GCE A-Level H2 Physics 2027
Learning goals
  • Use thermodynamic temperature and convert between Celsius and kelvin.
  • Use ideal-gas equations with particles, moles and SI units.
  • Apply the kinetic model to gas pressure and mean translational kinetic energy.
  • Derive pV = ⅓Nm⟨c²⟩ from the definition of pressure and a one-dimensional model of molecular collisions extended to three dimensions.
  • Relate microscopic energy, internal energy and thermal equilibrium.

Interactive stageLive model

Loading the interactive model…The interactive model did not load. Try again reloads this page; the explanation and worked content here are still available.

Change one variable at a time and watch the model respond.

Gas setup

Main mode
1.00 mol
320 K
10.0 L
State change controls
Shift factor
1.30×

Thermo checkpoint

What to notice:

Prediction target:

    Practice run

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    Run mode
    Try Ideal Gases Quiz

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    Study lensUse pV = nRT and special gas-law relationships only after checking what stays constant.14 min activity

    Try this

    Ask what is constant first, then decide whether the cleaner route is a named gas-law shortcut or the full ideal-gas relation.

    Learn to

    • Use pV = nRT and special gas-law relationships only after checking what stays constant.
    • Read p-V processes and connect work done by a gas to area under the graph.
    • Apply ΔU = Q − W consistently, including zero-work and zero-change cases.

    Exam transfer

    • Thermal modeling
    • Process interpretation

    Governing idea

    An ideal gas obeys pV = nRT and ΔU = Q − W, where W is work done by the gas. Isothermal, isochoric, isobaric, and adiabatic paths impose different constraints.

    Model boundary

    States are equilibrium states of a calorically perfect diatomic ideal gas with γ = 1.40 and constant heat capacities. Processes are quasi-static; phase changes and intermolecular forces are omitted.

    Avoid this trap

    Isothermal means ΔU = 0 for an ideal gas, not Q = 0. Adiabatic means Q = 0, while an isochoric process has W = 0. At zero state change, W, ΔU, and Q are all zero.

    How to explore

    Read state changes, p-V graphs, and process comparisons without mixing up constants, work, and internal-energy ideas.

    Predict the outcome, change one variable at a time, then interpret the result. Completion records participation only and does not award mastery.

    About this activity

    Compare state changes, p-V graphs, and thermal processes so gas-law shortcuts, work, and internal-energy reasoning stay aligned. A text explanation and no-JavaScript route remain available.

    How this activity affects progress
    Course and syllabus information
    Course
    GCE A-Level H2 Physics
    Edition
    GCE A-Level H2 Physics 2027