🌡️ Gas Laws Virtual Lab

Boyle · Charles · Real-time graphs

📘 Boyle's Law: Pressure & Volume

📐 Boyle's Law (Robert Boyle, 1662) — Complete Theory

Statement: For a fixed amount of gas at constant temperature, the absolute pressure is inversely proportional to the volume.

P₁V₁ = P₂V₂  →  P × V = constant (k)

Mathematical Derivation: From Ideal Gas Law PV = nRT, if T and n are constant, then PV = constant. Therefore, P ∝ 1/V.

Molecular Interpretation: When volume decreases, gas particles collide with walls more frequently, increasing pressure. The P-V graph is a rectangular hyperbola.

📈 Graphical Forms:

- P vs V : Hyperbola (P = k/V)
- P vs 1/V : Straight line through origin
- log P vs log V : Straight line slope -1

🔬 Experimental Verification:

Using a J-tube and mercury column, volume changes inversely with applied pressure.

🧪 Formula Summary: P₁V₁ = P₂V₂ | k = nRT | At constant T, P₂ = P₁ × (V₁/V₂)

📊 Real-world Applications: Syringes, breathing mechanism, scuba diving (pressure affects lung volume), bicycle pumps.

Volume (V)

10.0 L

Pressure (P)

1.00 atm

Boyle's Law: P × V = k

1.00 × 10.0 = 10.0

2 L11 L20 L
0.5 atm2.75 atm5 atm

📊 Real-time Hyperbolic Graph

Pressure vs Volume — Hyperbolic curve (P = k/V)

Pressure vs 1/Volume — Straight line (Proof)

📋 Recent measurements

Volume (L)Pressure (atm)P × V