Gas Laws Revision Sheet

1. 📌 Essentials

• Ideal Gas Law: PV = nRT; relates pressure, volume, temperature, and moles.
• Combined Gas Law: (P1V1)/T1 (P2V2)/T2; used for changing conditions.
• R constant: 0.0821 (L·atm)/(mol·K).
• Conversions: mm Hg to atm (divide by ); Celsius to Kelvin (add 273.15).
• Molar mass of CO₂: 44.01 g/mol.
• Gas behavior assumptions: No interactions, particles occupy negligible volume.
• Inverse relationship: Pressure and volume at constant T and n.
• Temperature in Kelvin: T(K) = Celsius + 273.15.
• Boyle’s Law: P1V1 = P2V2; at constant n, T.
• Charles’s Law: V ∝ T; at constant P, n.
• Gay-Lussac’s Law: P ∝ T; at constant V, n.

2. 🧩 Key Structures & Components

• Gas particles: Tiny molecules in constant, random motion.
• Container: Defines the volume and pressure environment.
• Pressure sensor: Measures force exerted by gas particles.
• Temperature sensor: Indicates kinetic energy of particles.
• Moles (n): Quantity of gas particles.
• R constant: Universal gas constant for calculations.
• Molar mass: Mass per mole; e.g., CO₂ = 44.01 g/mol.
• Ideal gas assumptions: No particle interactions, negligible volume.

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