1. Knowledge and understanding: at the end of the course the student must demonstrate sound knowledge of the fundamental principles and results of classical thermodynamics and chemical kinetics.

2. Applying knowledge and understanding: at the end of the course the student must know how to apply the
principles and results of classical thermodynamics and chemical kinetics to solve simple problems and exercises.

3. Making judgments: the student will recognize situations in which an approach
based on the principles treated can be applied to the solution of problems of interest in
the chemical and related sciences

4. Communication skills: at the end of the course the student will be able to express the concepts and principles of the discipline
using accurate scientific language

5. Ability to learn: at the end of the course the student will be able to explore, with a high degree of autonomy,
advanced concepts of classical thermodynamics and kinetics as required in higher education courses.

Knowledge of general chemistry and mathematics I (General and Inorganic Chemistry and Mathematics I courses)

PHYSICAL CHEMISTRY I

Principles of thermodynamics
1. Introduction and main results
2. Thermodynamic systems and variables
3. Zeroth principle and definition of temperature

Properties of gases
1. The ideal gas and the ideal gas thermometer
2. Kinetic-molecular theory of the ideal gas
3. Molecular collisions and mean free path
4. Maxwell distribution of molecular speeds
5. Real gases
6. Equations of state and the principle of corresponding states

Functions of several variables (outline)
1. Graphical representations
2. Partial derivatives
3. The total differential
4. Differential properties
5. Exact differentials and line integrals

First law of thermodynamics
1. Internal energy and the first law
2. States of equilibrium and reversibility
3. Work and heat
4. Thermochemistry and calorimetry
5. Applications of the first law

Second and third law of thermodynamics
1. Second law: Clausius and Kelvin-Planck postulates
2. Carnot cycle and heat engines
3. Thermodynamic temperature
4. Properties of cyclic processes and entropy
5. Calculation of entropy changes
6. Nernst's heat theorem and third law
7. Auxiliary state functions

Physical transformations of pure substances
1. Phase diagram for a pure substance
2. Thermodynamic aspects
3. Classification of phase transitions
4. Liquid-vapor interface: surface tension and capillary action

Simple binary mixtures
1. Ideal solutions
2. Partial molar quantities and Gibbs-Duhem equation
3. The chemical potential
4. Thermodynamics of the mixing process
5. Non-ideal solutions: activity, activity coefficient and standard states

Colligative properties
1. Lowering of the freezing point
2. Elevation of the boiling point
3. Osmotic pressure

Phase equilibria for multi-component systems
1. The phase rule
2. Binary systems involving vapor
3. Distillation of liquid mixtures and azeotropes
4. Binary systems in condensed phase and thermal analysis
5. Phase diagrams of aqueous salts solutions
6. Formation of intermediate compounds in complex diagrams

Chemical equilibrium
1. Reaction potential, reaction quotient and thermodynamic equilibrium constant
2. Relationships between thermodynamic constant and practical equilibrium constants
3. Dependence of the equilibrium composition on the pressure
4. Dependence of the equilibrium constant on the temperature
5. Equilibria in liquid solutions

Thermodynamic properties of electrolyte solutions
1. Thermodynamics of ion formation
2. Ionic activities
3. Conductivity of electrolyte solutions and ionic mobility
4. Electrochemical cells: cell potential and Nernst equation
5. Standard potentials and their experimental determination
6. Thermodynamic quantities from measurements of EMF
7. pH measurements

Chemical kinetics
1. Reaction rate, kinetic law and rate constant
2. Elementary processes
3. Reactions with simple kinetic form: zeroth order reactions, 1st order, pseudo 1st order and 2nd order reactions
4. Experimental determination of reaction orders
5. Reversible 1st order reactions
6. Relaxation methods
7. Consecutive reactions of the first order
8. The steady-state approximation
9. Unimolecular reactions in gas phase
10. Pre-equilibria
11. The variation of rate constant with temperature

PHYSICAL CHEMISTRY LABORATORY I
1. Determination of heat of combustion
2. Determination of reaction enthalpy by calorimetric method
3. Determination of the liquid/vapor phase diagram for an azeotropic mixture
4. Determination of the dissociation constant of CH3COOH from conductivity measurements
5. Kinetics of the iodination of acetone
6. Kinetics of the hydrolysis of ethyl acetate with the pH-stat technique

1. P. Atkins, J. de Paula, Atkin's Physical Chemistry, 7th Ed. Oxford University Press, Oxford, UK, 2002.
2. R. S. Berry, S. A. Rice, J. Ross, Physical Chemistry, 2nd Ed. Oxford University Press, Oxford, UK, 2000.
3. D. Kondepudi, I. Progogine, Modern Thermodynamics: from heat engines to dissipative structures, John Wiley & Sons Ltd, Chichester, UK, 1998.
4. K. Denbigh, The principles of Chemical Equilibrium with applications in Chemistry and Chemical Engineering, 4th Ed. Cambridge University Press, Cambridge, UK, 1981.
5. J. E. Espenson, Chemical Kinetics and Reaction Mechanisms, McGraw-Hill Series in Advanced Chemistry, McGraw-Hill, Inc. 1981.
6. H. Dewoe, Thermodynamics and Chemistry, available online (http://www.chem.umd.edu/thermobook)

There are Italian editions of books 1 and 4 (although the latter is rather dated). A number of volumes are also available for consultation in the library
of the department.
The dedicated page of the course on the moodle2 platform contains all the teaching material presented during the lectures: presentations in PDF format containing all the derivations illustrated in classroom and a wide selection of solved exercises, example of lab reports, videos of experiments and a large database of quizzes that can be used in preparation for the final written exam.

PHYSICAL CHEMISTRY I Principles of thermodynamics 1. Introduction and main results 2. Thermodynamic systems and variables 3. Zeroth principle and definition of temperature Properties of gases 1. The ideal gas and the ideal gas thermometer 2. Kinetic-molecular theory of the ideal gas 3. Molecular collisions and mean free path 4. Maxwell distribution of molecular speeds 5. Real gases 6. Equations of state and the principle of corresponding states Functions of several variables (outline) 1. Graphical representations 2. Partial derivatives 3. The total differential 4. Differential properties 5. Exact differentials and line integrals First law of thermodynamics 1. Internal energy and the first law 2. States of equilibrium and reversibility 3. Work and heat 4. Thermochemistry and calorimetry 5. Applications of the first law Second and third law of thermodynamics 1. Second law: Clausius and Kelvin-Planck postulates 2. Carnot cycle and heat engines 3. Thermodynamic temperature 4. Properties of cyclic processes and entropy 5. Calculation of entropy changes 6. Nernst's heat theorem and third law 7. Auxiliary state functions Physical transformations of pure substances 1. Phase diagram for a pure substance 2. Thermodynamic aspects 3. Classification of phase transitions 4. Liquid-vapor interface: surface tension and capillary action Simple binary mixtures 1. Ideal solutions 2. Partial molar quantities and Gibbs-Duhem equation 3. The chemical potential 4. Thermodynamics of the mixing process 5. Non-ideal solutions: activity, activity coefficient and standard states Colligative properties 1. Lowering of the freezing point 2. Elevation of the boiling point 3. Osmotic pressure Phase equilibria for multi-component systems 1. The phase rule 2. Binary systems involving vapor 3. Distillation of liquid mixtures and azeotropes 4. Binary systems in condensed phase and thermal analysis 5. Phase diagrams of aqueous salts solutions 6. Formation of intermediate compounds in complex diagrams Chemical equilibrium 1. Reaction potential, reaction quotient and thermodynamic equilibrium constant 2. Relationships between thermodynamic constant and practical equilibrium constants 3. Dependence of the equilibrium composition on the pressure 4. Dependence of the equilibrium constant on the temperature 5. Equilibria in liquid solutions Thermodynamic properties of electrolyte solutions 1. Thermodynamics of ion formation 2. Ionic activities 3. Conductivity of electrolyte solutions and ionic mobility 4. Electrochemical cells: cell potential and Nernst equation 5. Standard potentials and their experimental determination 6. Thermodynamic quantities from measurements of EMF 7. pH measurements Chemical kinetics 1. Reaction rate, kinetic law and rate constant 2. Elementary processes 3. Reactions with simple kinetic form: zeroth order reactions, 1st order, pseudo 1st order and 2nd order reactions 4. Experimental determination of reaction orders 5. Reversible 1st order reactions 6. Relaxation methods 7. Consecutive reactions of the first order 8. The steady-state approximation 9. Unimolecular reactions in gas phase 10. Pre-equilibria 11. The variation of rate constant with temperature PHYSICAL CHEMISTRY LABORATORY I 1. Determination of heat of combustion 2. Determination of reaction enthalpy by calorimetric method 3. Determination of the liquid/vapor phase diagram for an azeotropic mixture 4. Determination of the dissociation constant of CH3COOH from conductivity measurements 5. Kinetics of the iodination of acetone 6. Kinetics of the hydrolysis of ethyl acetate with the pH-stat technique

Lectures with presentations (beamer or powerpoint) Laboratory experiments in which the students (divided into groups of 3-4 people) perform the tasks illustrated during the lectures, under the supervision of the lecturer and the tutor.

For any question you might have, please contact the lecturer by email

The exam consists of a written test and an oral exam, to which the student can have access after passing the written test.

The written test consists of 15 multiple choice exercises (all of equal weight, and generally of a numerical character, 1 correct answer out of 4 possible choices).
The aim is to test the student's ability to apply knowledge and understanding.
The passing grade is greater than or equal to 18/30.

Before attending the oral exam, which serves to test communication skills and theoretical knowledge of the discipline (classical thermodynamics and chemical kinetics), the student must submit the lab reports (just one report per group). The reports will be discussed during the oral examination. The oral exam covers all the topics covered in the course and can include simple derivations of equations / general results discussed during the lectures.

The evaluation grid adopted is as follows:
- Excellent (30 - 30 cum laude): excellent knowledge of the topics, excellent proficiency of the technical language,
excellent analytical ability.
- Very good (27 - 29): good knowledge of the topics, notable fluency in technical language,
good analytical ability.
- Good (24-26): good knowledge of the main topics, fair command of technical language; the
student shows adequate analytical ability.
- Satisfactory (21-23): the student does not show full mastery of the main topics, despite possessing the fundamental knowledge;
language skills are satisfactory and the analytical ability is sufficient.
- Sufficient (18-20): minimal knowledge of the main topics and
technical language, limited analytical ability.
- Insufficient: the student does not have acceptable knowledge of the contents of the
different topics of the program.

Changes to the above guidelines, which could be made to enforce security measures related to the COVID19 emergency, will be notified on the Department's web site.

This course explores topics closely related to one or more goals of the United Nations 2030 Agenda for Sustainable Development (SDGs)