Physical Chemistry I: Thermodynamics

Chemical thermodynamics from its foundations to its applications: systems, state functions, standard states and the sign conventions for heat and work; the ideal gas law and kinetic theory, compression factors, the virial and van der Waals equations, critical points and corresponding states; the first law, reversible and irreversible expansion work, internal energy and adiabatic processes; enthalpy, heat capacities, calorimetry, Hess's law, enthalpies of formation, bond enthalpies and Kirchhoff's law; the second law from Carnot and Clausius, entropy changes for expansion, heating, phase changes and mixing, and Boltzmann's formula; the third law, Debye extrapolation, absolute and residual entropies; the Gibbs and Helmholtz energies as criteria of spontaneity and measures of maximum work, crossover temperatures and the graphite–diamond boundary; the fundamental equations, Maxwell relations, chemical potential and fugacity; phase diagrams of water and carbon dioxide, the phase rule and the Clapeyron and Clausius–Clapeyron equations; ideal and real solutions, Raoult's and Henry's laws, azeotropes, freezing-point depression, road salt and osmotic pressure; the equilibrium constant, Le Chatelier's principle, the van 't Hoff equation and the ammonia equilibrium; and a capstone on electrochemical cells, the Nernst equation, batteries, fuel cells, electrolysis and the Haber–Bosch process, with runnable Python programs throughout.

CHEM-271 Year 2 3 credits 12 lessons · 4 h 50 min ▶ Video lessons coming soon

Offered by HSM University · Chemistry

This is the American version of this course. See the Canadian version.

What you'll learn

Explain the scope of chemical thermodynamics as the study of energy, direction and equilibrium, classify systems and properties, distinguish state functions from path functions, and use standard states and the chemistry sign convention for heat and work.
Apply the ideal gas law and kinetic theory, measure non-ideality with the compression factor and virial equation, and use the van der Waals equation to calculate real-gas pressures, critical constants and reduced properties.
Calculate expansion work, heat and internal energy changes for reversible and irreversible, isothermal and adiabatic processes of ideal gases, and explain why reversible processes give limiting values of work.
Relate enthalpy to heat at constant pressure, use heat capacities and calorimetry, calculate reaction enthalpies with Hess's law, enthalpies of formation and bond enthalpies, and correct them for temperature with Kirchhoff's law.
State the second law, define entropy through reversible heat, calculate entropy changes for expansion, heating, phase transitions and mixing, and judge spontaneity from the total entropy change of system and surroundings.
Explain the third law and residual entropy, determine absolute entropies from heat capacities with a Debye extrapolation, and calculate standard reaction entropies from tables.
Define the Gibbs and Helmholtz energies, use them as criteria of spontaneity and measures of maximum work, calculate standard reaction Gibbs energies and crossover temperatures, and predict the effect of temperature and pressure on G.
Derive and use the fundamental equations and Maxwell relations, apply the thermodynamic equation of state, and define chemical potential, partial molar quantities and fugacity as the basis of equilibrium.
Interpret phase diagrams of pure substances with the phase rule, and apply the Clapeyron and Clausius–Clapeyron equations to phase boundaries, vapor pressures and boiling points.
Describe ideal and real solutions with chemical potentials and activities, apply Raoult's and Henry's laws to vapor pressures, distillation and gas solubility, and calculate colligative properties including freezing-point depression and osmotic pressure.
Relate the reaction Gibbs energy to the equilibrium constant, predict the response of equilibria to changes in composition, pressure and temperature, and use the van 't Hoff equation to find reaction enthalpies and equilibrium yields.
Relate cell potentials to Gibbs energies, apply the Nernst equation to galvanic, concentration and fuel cells, and analyze batteries, electrolysis and the Haber–Bosch process as applications of chemical thermodynamics.

Course content

12 lessons · 4 h 50 min total · final exam

1 What physical chemistry is: energy, change and equilibrium 27 min · quiz
2 Gases: ideal behavior, real gases and the van der Waals equation 24 min · quiz
3 The first law: work, heat and internal energy 23 min · quiz
4 Enthalpy, heat capacity and thermochemistry 24 min · quiz
5 Entropy and the second law 23 min · quiz
6 The third law, absolute entropies and spontaneity 25 min · quiz
7 Gibbs and Helmholtz energies 24 min · quiz
8 Fundamental equations, Maxwell relations and chemical potential 25 min · quiz
9 Phase equilibria of pure substances: phase diagrams and the Clapeyron equation 22 min · quiz
10 Mixtures and solutions: Raoult's and Henry's laws, colligative properties 25 min · quiz
11 Chemical equilibrium: the equilibrium constant, temperature and van 't Hoff 23 min · quiz
12 Capstone: electrochemistry and thermodynamics at work 25 min · quiz
E Final exam 20 questions

Requirements

Recommended background. You can start any course at any time.

Description

Part of the Science stream, typically taken in year 2.