Physical Chemistry I
A.Y. 2025/2026
Learning objectives
Understanding of the theoretical and practical aspects of Chemical Thermodynamics, which aims to interpret chemical phenomena through laws of general validity. Study of energy exchanges between the study system and the environment in conditions where the system is in equilibrium or in which the system tends to evolve spontaneously.
Expected learning outcomes
At the end of the course, the student will be able to apply the principles of Thermodynamics to chemical systems under equilibrium conditions. He/she will be able to use classical Chemical Thermodynamics in the study of phase equilibrium in single-- and multi-component systems and in chemical equilibrium. He/she will understand the physical principles at the basis of chemical phenomena and will be able to apply them to simple practical problems.
Lesson period: First semester
Assessment methods: Esame
Assessment result: voto verbalizzato in trentesimi
Single course
This course can be attended as a single course.
Course syllabus and organization
Single session
Responsible
Lesson period
First semester
Course syllabus
Properties of gases: ideal gases and ideal gas mixtures, real gases, equations of state.
The First, Second, and Third Laws of Thermodynamics: work, internal energy, heat, enthalpy, entropy, Helmholtz and Gibbs energies, the fundamental equation, chemical potential.
Phase equilibria: phase rule, phase diagrams, phase equilibria in single-component systems, Clausius-Clapeyron equation.
Vapor pressure of pure components and solutions, phase diagrams of binary systems. Colligative properties. Raoult's law and Henry's law. Properties of ideal, ideally dilute, and real liquid solutions. Activity coefficients and their determination.
Thermochemistry: standard enthalpy changes, standard enthalpies of formation and their temperature dependence, calorimetric measurements.
Reaction equilibria: equilibrium constants for reactions in the gas phase and in liquid solution; temperature dependence of the equilibrium constant; heterogeneous phase equilibria; simultaneous and independent equilibrium reactions.
Numerical solution of chemical thermodynamics problems.
The First, Second, and Third Laws of Thermodynamics: work, internal energy, heat, enthalpy, entropy, Helmholtz and Gibbs energies, the fundamental equation, chemical potential.
Phase equilibria: phase rule, phase diagrams, phase equilibria in single-component systems, Clausius-Clapeyron equation.
Vapor pressure of pure components and solutions, phase diagrams of binary systems. Colligative properties. Raoult's law and Henry's law. Properties of ideal, ideally dilute, and real liquid solutions. Activity coefficients and their determination.
Thermochemistry: standard enthalpy changes, standard enthalpies of formation and their temperature dependence, calorimetric measurements.
Reaction equilibria: equilibrium constants for reactions in the gas phase and in liquid solution; temperature dependence of the equilibrium constant; heterogeneous phase equilibria; simultaneous and independent equilibrium reactions.
Numerical solution of chemical thermodynamics problems.
Prerequisites for admission
To successfully approach and understand the topics covered in this course, it is necessary to have a solid knowledge and good command of differential and integral calculus.
A sound understanding of basic chemistry and the stoichiometry of chemical reactions is also essential.
These prerequisites are typically acquired by passing the first-year exams of the Industrial Chemistry degree program or equivalent courses offered in other scientific degree programs.
A sound understanding of basic chemistry and the stoichiometry of chemical reactions is also essential.
These prerequisites are typically acquired by passing the first-year exams of the Industrial Chemistry degree program or equivalent courses offered in other scientific degree programs.
Teaching methods
Lectures (6 ECTS credits in total), consisting of 44 hours of classroom lectures (5.5 ECTS), divided into two modules, A and B, plus 8 hours of numerical exercises (0.5 ECTS), supported by slide presentations and traditional blackboard explanations, which will be provided upon students' request.
Attendance is strongly recommended.
Attendance is strongly recommended.
Teaching Resources
P.W. Atkins, J. De Paula, Physical Chemistry, Oxford University Press, 9th edition, or other editions for the chapters relevant to the topics covered.
K. Denbigh, The Principles of Chemical Equilibrium, Cambridge University Press.
K. Denbigh, The Principles of Chemical Equilibrium, Cambridge University Press.
Assessment methods and Criteria
The exam consists of a preliminary written test, involving the solution of numerical problems in chemical thermodynamics. The test is graded on a 30-point scale.
Passing the written test grants access to the oral examination with both the teachers responsible for Modules A and B. The oral exam covers all topics discussed during the lectures.
The final grade, also expressed on a 30-point scale, is calculated as the arithmetic average of the scores obtained in the written test and in the oral evaluations for both modules.
At the end of the Modules A and B, students have the opportunity to take two written mid-term tests, each based on numerical exercises covered during the lessons. Successfully passing both mid-term tests (graded on a 30-point scale) allows direct access to the oral exam, without the need to take the final written test.
During the oral examination, students must demonstrate a solid understanding of the fundamentals of chemical thermodynamics, the ability to correctly develop and logically apply thermodynamic equations, and the capacity to critically discuss the results obtained in relation to the different systems studied in the course.
Passing the written test grants access to the oral examination with both the teachers responsible for Modules A and B. The oral exam covers all topics discussed during the lectures.
The final grade, also expressed on a 30-point scale, is calculated as the arithmetic average of the scores obtained in the written test and in the oral evaluations for both modules.
At the end of the Modules A and B, students have the opportunity to take two written mid-term tests, each based on numerical exercises covered during the lessons. Successfully passing both mid-term tests (graded on a 30-point scale) allows direct access to the oral exam, without the need to take the final written test.
During the oral examination, students must demonstrate a solid understanding of the fundamentals of chemical thermodynamics, the ability to correctly develop and logically apply thermodynamic equations, and the capacity to critically discuss the results obtained in relation to the different systems studied in the course.
CHIM/02 - PHYSICAL CHEMISTRY - University credits: 6
Practicals: 8 hours
Lessons: 44 hours
Lessons: 44 hours
Professors:
Chiarello Gian Luca, Gervasini Antonella
Educational website(s)
Professor(s)
Reception:
On request by e-mail
Room R25S, B side of Chemistry Department