Ideal Gas Law
Definition
The equation PV = nRT relating pressure (P), volume (V), moles of gas (n), the gas constant (R), and temperature (T) for ideal gases.
Why is Ideal Gas Law Important?
Ideal Gas Law is an essential chemistry concept used in laboratories, pharmaceutical development, environmental science, and industrial processes. Understanding this concept is critical for accurate chemical calculations, safe laboratory practices, and optimizing reactions.
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What is the Ideal Gas Law?
The Ideal Gas Law combines Boyle's, Charles's, and Avogadro's laws into one equation: PV = nRT. It describes the behavior of an ideal gas — a theoretical gas of point particles with no intermolecular forces. Real gases approximate ideal behavior at low pressures and high temperatures.
Variables and Units
| Variable | Meaning | SI Unit | Common Unit |
|---|---|---|---|
| P | Pressure | Pascal (Pa) | atm, mmHg, kPa |
| V | Volume | m³ | liters (L) |
| n | Amount (moles) | mol | mol |
| R | Gas constant | 8.314 J/(mol·K) | 0.08206 L·atm/(mol·K) |
| T | Temperature | Kelvin (K) | K (must be absolute!) |
Related Gas Laws
| Law | Relationship | Conditions |
|---|---|---|
| Boyle's | P₁V₁ = P₂V₂ | Constant T, n |
| Charles's | V₁/T₁ = V₂/T₂ | Constant P, n |
| Avogadro's | V₁/n₁ = V₂/n₂ | Constant T, P |
| Gay-Lussac's | P₁/T₁ = P₂/T₂ | Constant V, n |
STP Reference
At Standard Temperature and Pressure (0°C = 273.15 K, 1 atm): 1 mole of any ideal gas occupies 22.4 liters.