If you halve the volume at constant temperature, what happens to pressure?

Boyle's Law: PV = const → P doubles.

At 300K the gas occupies 10L. What volume at 600K (constant pressure)?

Charles's Law: V₁/T₁ = V₂/T₂ → V₂ = 20L.

Why does a sealed balloon shrink in a cold room?

Constant n and P → V ∝ T; lower T means smaller V.

Pro 🔒~20 min

Gases: Introduction

Explore pressure, volume, temperature, and the Ideal Gas Law

How it works

The Ideal Gas Law PV = nRT relates pressure, volume, amount (moles), and temperature of an ideal gas. Boyle's Law (constant T): pressure and volume are inversely proportional. Charles's Law (constant P): volume and temperature are directly proportional. Real gases deviate from ideal behavior at high pressures and low temperatures when intermolecular forces become significant.

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Step-by-step

Add or remove molecules using the pump.
Adjust temperature using the heater/cooler.
Change container volume by dragging the wall.
Observe how pressure changes as you hold different variables constant to verify gas laws.

Key formulas

$PV = nRT$ Ideal Gas Law
$P \propto \frac{1}{V}$ Boyle's Law (constant T)
$V \propto T$ Charles's Law (constant P)

Frequently asked questions

If you halve the volume at constant temperature, what happens to pressure?: Boyle's Law: PV = const → P doubles.
At 300K the gas occupies 10L. What volume at 600K (constant pressure)?: Charles's Law: V₁/T₁ = V₂/T₂ → V₂ = 20L.
Why does a sealed balloon shrink in a cold room?: Constant n and P → V ∝ T; lower T means smaller V.