Unit · year 1
CU-104 · States of Matter & Gases
Threads energy · structure24 lectures6 results
Gases, liquids and solids, and the kinetic picture that explains gas behaviour.
PREREQUISITES
Lectures
| L01 | The Three States and Phase Changes — |
| L02 | Pressure, Volume, and Temperature — |
| L03 | Boyle's, Charles's, and Gay-Lussac's Laws |
| L04 | The Ideal Gas Law |
| L05 | Gas Density and Molar Mass Determination |
| L06 | Dalton's Law of Partial Pressures |
| L07 | The Kinetic Molecular Model — |
| L08 | Pressure from Molecular Collisions |
| L09 | Temperature and Mean Kinetic Energy |
| L10 | Root-Mean-Square Speed |
| L11 | The Maxwell–Boltzmann Distribution |
| L12 | Effect of Temperature and Mass on the Distribution |
| L13 | Mean Free Path and Collision Frequency |
| L14 | Effusion and Diffusion |
| L15 | Graham's Law |
| L16 | Isotope Separation by Effusion |
| L17 | Real Gases and Deviations from Ideality |
| L18 | The van der Waals Equation |
| L19 | Critical Constants and the Critical Point |
| L20 | The Compression Factor and Corresponding States |
| L21 | Liquids: Viscosity, Surface Tension, Vapour Pressure — |
| L22 | Solids: Crystalline versus Amorphous — |
| L23 | Phase Diagrams — |
| L24 | Synthesis: From Molecular Motion to Bulk Behaviour |
Results in this unit
T-018
The ideal gas law
PV = nRT, assembled from the empirical gas laws.
T-019
Kinetic theory of gases
Pressure as the rate of molecular momentum transfer to the walls.
T-020
The distribution of molecular speeds
Temperature sets the spread of molecular speeds.
T-021
The van der Waals equation
Real gases corrected for molecular size and attraction.
T-022
Graham's law of effusion
Effusion rate varies inversely with the square root of molar mass.
T-181
The Arrhenius equation and activation energy
Collision theory in a Maxwell-Boltzmann gas gives k proportional to root-T times exp(-E0/RT), and the activation energy RT^2 dlnk/dT is E0 + RT/2.