Gas Laws Flashcards
Grade 10 · Science · Flashcards
Core formulas, definitions, and key concepts for understanding the behavior of gases and their quantitative relationships.
Flashcards
- Boyle's Law
- P₁V₁ = P₂V₂; pressure and volume are inversely proportional at constant T and n
- Charles's Law
- V₁/T₁ = V₂/T₂; volume and absolute temperature are directly proportional at constant P and n
- Gay-Lussac's Law
- P₁/T₁ = P₂/T₂; pressure and absolute temperature are directly proportional at constant V and n
- Avogadro's Law
- Equal volumes of gases at the same T and P contain equal numbers of moles: V₁/n₁ = V₂/n₂
- Combined Gas Law
- P₁V₁/T₁ = P₂V₂/T₂; merges Boyle's, Charles's, and Gay-Lussac's Laws for a fixed amount of gas
- Ideal Gas Law
- PV = nRT; P in atm, V in liters, n in moles, T in Kelvin, R = 0.08206 L·atm/mol·K
- STP conditions
- Standard Temperature and Pressure: 273.15 K (0°C) and 1.000 atm; molar volume = 22.4 L/mol
- Kelvin conversion
- K = °C + 273.15; always convert Celsius to Kelvin before using gas laws
- Dalton's Law of Partial Pressures
- P_total = P₁ + P₂ + P₃ ...; total pressure is the sum of all individual partial pressures in a mixture
- Partial pressure
- Pressure exerted by a single gas in a mixture; P_gas = X_gas × P_total (X = mole fraction)
- Kinetic Molecular Theory
- Gas particles are in constant random motion; average kinetic energy is proportional to absolute temperature
- Ideal gas assumptions
- Negligible particle volume, no intermolecular forces, perfectly elastic collisions, random motion
- Absolute zero
- 0 K = -273.15°C; theoretical lowest temperature where molecular motion ceases
- Real gas deviation
- Real gases deviate from ideal behavior at high pressures (volume matters) and low temperatures (attractions matter)
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