Simulations

Simulations of Thermodynamics

First Law of Thermodynamics

Process type

Heat in (Q)200 J
Work out (W)80 J

Heat (Q)

+200 J

Work (W)

+80 J

ΔU (internal energy)

+120 J

300 KgasQ inW outΔU = Q − W

ΔU = 200 − 80 = +120 J

Gas heats up — internal energy increases

Overview

Explore the First Law of Thermodynamics ($\Delta U = Q – W$) by adjusting heat and work on a gas-filled cylinder. This core principle explains how car engines and refrigerators operate.

Controls

Select a thermodynamic process (General, Isothermal, Adiabatic, or Isochoric) and use the sliders to add or remove Heat (Q) and Work (W).

Observations

Watch the piston physically expand and compress, observe gas temperature and color shifts, and track the real-time balancing of the energy equation.

Conduction, Convection, and Radiation

Toggle mechanisms and adjust fire intensity to observe the physics of heat movement.

Active Mechanisms

Loading active physics data…

Overview

Explore the three mechanisms of heat transfer (conduction, convection, and radiation) by interacting with a digital campfire. This fundamental physics concept explains how thermal energy moves through solids, fluids, and open space.

Controls

Toggle specific heat transfer methods (Conduction, Convection, Radiation) on or off, and use the slider to adjust the overall fire intensity.

Observations

Watch heat travel progressively through the solid metal rod, observe cyclic fluid currents rising above the flames, and track infrared energy waves radiating outward as the fire's intensity changes.

The Ideal Gas Law

Calculated Pressure (P)
0.00 atm
Formula used: P = (n × R × T) / V
Constant R = 0.0821 L·atm/(mol·K)

Overview

Explore the relationships of the Ideal Gas Law P = nRT/V using an interactive gas-filled container with a movable piston. This simulation demonstrates how changing volume, temperature, and molecular amount dynamically impacts pressure.

Controls

Use the sliders to adjust the gas Volume (V), system Temperature (T), and the overall Amount of Gas (n) in moles.

Observations

Watch the piston physically compress or expand the chamber, observe gas particles speed up or slow down with temperature shifts, and track real-time changes to the calculated pressure reading.

Kinetic Theory of Gases

Kinetic Theory of Gases — Isolated Component
Molecular motion
Pressure
Speed distribution
Light vs heavy
Temperature
300 K
Avg speed
511 m/s
Molecules
60
Wall hits
0
Temperature
300 K
Pressure
1.0x
Temp300 K Count60
Temp300 K Count40
Temp300 K Gas
Same temperature, different mass — lighter = faster
What you see: each dot is a molecule bouncing inside a container. Raise the temperature — they speed up. This random motion is kinetic theory.
Pressure = molecules hitting walls. Red flash = wall collision. More molecules or higher temp = more hits = higher pressure.
Maxwell-Boltzmann: not all molecules move at the same speed. The curve shows how speeds are distributed. Dashed line = RMS speed.
Same energy, different speed. Blue = H₂, coral = CO₂. Lighter molecules move much faster at the same temperature.

Overview

Explore the Kinetic Theory of Gases through an interactive simulation of molecular motion. This tool visualizes how temperature and mass dictate the speed of individual molecules and how their constant collisions generate pressure.

Controls

Toggle between four distinct views (Molecular Motion, Pressure, Speed Distribution, and Light vs Heavy). Use the interactive sliders to adjust the Temperature and Molecule Count, or use the dropdown menu to select different real-world gas types.

Observations

Watch molecules visibly accelerate as temperature increases, observe the red flashes as wall collisions actively generate pressure, and study the Maxwell-Boltzmann curves to see exactly why lighter gases travel significantly faster than heavier ones at the same temperature.

Second Law of Thermodynamics

Hot reservoir temperature (K)
800 K
Cold reservoir temperature (K)
300 K
Carnot efficiency
62.5%
η = 1 − Tc/Th
Work output (per 100J)
62.5 J
W = η × Qh
Waste heat (per 100J)
37.5 J
Qc = Qh − W
No real engine can exceed Carnot efficiency. A perfect 100% efficient engine would require the cold reservoir to be at absolute zero (0 K), which is physically impossible.

Overview

Explore the thermodynamics of a theoretical Carnot Heat Engine by altering reservoir temperatures. This simulation demonstrates maximum theoretical engine efficiency eta =T_c/T_h and illustrates how energy splits into useful work versus unavoidable waste heat.

Controls

Use the interactive sliders to adjust the Hot Reservoir Temperature T_h and the Cold Reservoir Temperature T_c.

Observations

Watch the engine's thermal efficiency shift dynamically as the temperature gap changes, observe real-time recalculations of work output versus waste heat per 100 Joules, and track the shifting energy division on the visual bar graph.

Note: More categories coming soon

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