IB SL Chemistry - KMT / Gas Laws

• Changes of state result from adding or removing energy from a substance, altering particle kinetic energy.
• Types of molecular motion include vibrational (solids, liquids, gases), rotational (liquids, gases), and translational (gases).
• Melting weakens intermolecular forces; boiling breaks intermolecular forces.
• Real gases follow KMT at low pressure and high temperature; temperature decrease and pressure increase lead to closer particles.
• Gas laws include Boyle's Law (V1P1 = V2P2), Charles's Law (V1/T1 = V2/T2), and Gay-Lussac’s Law (P1/T1 = P2/T2).
• The Combined Gas Law states that V1P1/T1 = V2P2/T2.
• The Ideal Gas Law states that PV = nRT.
• Avogadro's Law states that n1/V1 = n2/V2.
• Individual particles in a gas have no volume compared to the space between particles.
• Individual particles in a real gas have a very small volume.
• No attractive/repulsive forces exist between the particles in a gas.
• Very small attractive/repulsive forces exist between the particles in a real gas.
• Collisions between gas particles and other particles/container walls are elastic, meaning no loss of kinetic energy.
• Collisions between particles in a real gas are inelastic, resulting in energy loss upon collision.
• The average kinetic energy of a gas is directly related to its temperature; higher temperature = higher kinetic energy.
• Gas particles are composed of small particles with mass, mostly empty space, and have a low density.
• Gas particles are in constant random straight-line motion.