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This simulation shows what happens to oxygen gas (O₂) when you change temperature, volume, or the number of molecules. It’s based on the Kinetic Molecular Theory and the Ideal Gas Law (PV = nRT), which basically describe how gas molecules move and bump into each other.

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Temperature
When the temperature goes up, the molecules move faster. Faster molecules hit the walls more often, which increases the pressure. Even though the slider shows Celsius, the simulation converts it to Kelvin (°C + 273) because that’s what the formulas require.

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Volume
Changing the container size changes how cramped the molecules are. A smaller container means the molecules collide more often, raising the pressure. A bigger container gives them more space, so collisions happen less frequently and the pressure goes down. This is exactly what Boyle’s Law predicts.

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Number of Molecules
Adding more molecules means more collisions and higher pressure. Fewer molecules mean fewer collisions and lower pressure.

What the Moving Dots Represent
Each dot is one oxygen molecule. They move randomly, bounce off the walls, and speed up when the temperature rises. This shows in a very visual way how temperature affects molecular motion.

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Ideal Gas Law in Action
The simulation calculates pressure with the formula:

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p=nRT/V

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• P is the pressure (shown in kPa)

• n is the number of moles of gas (from particle count)

• R is the gas constant

• T is temperature in Kelvin

• V is volume

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When you move the sliders, you can actually see how changing temperature, volume, or number of molecules changes pressure, just like it would in a real lab.

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TL/DR: This simulation makes the gas laws easy to understand. Instead of just reading formulas, you can see molecules move, collide, and respond to changes, which makes the behavior of gases much clearer.