Objectives

General expected learning outcomes
The course aims to provide students the information necessary for a critical knowledge of the principles and applications of physical chemistry ranging from classical thermodynamics to kinetics, electrochemistry and, in particular, to the thermodynamics of irreversible processes. I this way students will acquire the basis to understand some of the topics covered in the courses in the next years of biochemical, chemical pharmaceutical and pharmacological character, with particular regard to transport processes.

Specific expected learning outcomes
KNOWLEDGE AND UNDERSTANDING:
• to know the principles underlying physical chemistry about the thermodynamic, kinetic and thermodynamic treatment of irreversible processes;
• to be able to understand its potential and its use for the study of real systems, about the biological ones.


APPLYING KNOWLEDGE AND UNDERSTANDING:
• to understand the different theoretical-experimental approaches for the resolution of problems in the biochemical and pharmacological fields.

MAKING JUDGMENTS:
• to be able to develop their critical sense following stimuli coming from the teacher:
• to be able to link the topics studied thanks also to the multidisciplinary of the course by integrating the physical chemistry with the knowledge already acquired or to be acquired of the chemical type (inorganic, organic, biochemical chemistry) and biological (pharmacology and toxicology).

LEARNING SKILLS:
• To be able to describe scientific topics related to real systems using in a critical way the methodologies and techniques covered in the course.

COMMUNICATION SKILLS:
• To be able to discuss scientific topics related to physical chemistry and apply them to biological, pharmaceutical and pharmacological processes.

Channels

A - L

FRANCO MAZZEI FRANCO MAZZEI   Teacher profile

Programme

Classical Thermodynamics.
Introduction. Definition of system, environment, variables or thermodynamic functions. States of equilibrium and thermodynamic transformations. Heat and Work. Calorimetry.
The first principle. Internal energy. Thermal capacity and specific heat. Application of the first principle to perfect gases.
Enthalpy. Enthalpy of reactions in the gaseous phase. Enthalpy of physical, atomic and molecular transformations. Thermochemistry. Law of Hess. Enthalpy training standard. Variation of enthalpy with temperature: Kirchhoff's law. Joule-Thomson effect.
6 hours frontal lecture

The second principle. Utterances. Spontaneous transformations. Reversibility and irreversibility.
Entropy. Definition of thermodynamics. Clausius inequality. Reversible and irreversible isothermal expansion of a perfect gas. Adiabatic transformations. Thermodynamic cycles. Theorem and Carnot cycle. Variation of entropy with temperature.
Third principle. Nernst's theorem. Boltzmann report.
5 hours of frontal lecture

Helmholtz energy and Gibbs energy. Maximum work function. Free reaction energy. The fundamental equation of thermodynamics. Maxwell reports. Thermodynamic state equation. Variation of Gibbs energy with pressure and temperature. Gibbs-Helmholtz equation. Fugacity and activity. Partial molar quantities. Chemical potential. Thermodynamic equilibrium criterion. Reaction quotient and equilibrium constant. The Boltzmann equilibrium constant and distribution. Le Chatelier's principle. Van't Hoff equation.
6 hours of frontal lecture

The physical transformations of pure substances. State diagrams: critical point, boiling point and melting point, triple point. The water status diagram. Clapeyron equation. The properties of simple blends. Thermodynamic description of the mixtures. Partial molar quantities. The molar partial volume. Partial molar Gibbs energy. The Gibbs-Duhem equation. Thermodynamic mixing quantities. The chemical potential of liquids. The ideal solutions. Raoult's law. The ideal diluted solutions. Henry's law. Colligative properties: elevated ebullioscope, cryoscopic and osmotic pressure. Solvent activity. The activity of the solute. Ideal diluted solutions. Real solutions.
6 hours of frontal lecture

Phase equilibria: Mix state diagrams. Two-component systems and temperature-composition diagrams. Liquid-liquid status diagrams for partially miscible two-component systems. Liquid-vapor state diagrams for volatile liquid mixtures: characteristic vapor pressure curves; pressure-composition and temperature-composition diagrams; simple and fractional distillation; azeotropes.
4 hours of frontal lecture

Properties of electrolyte solutions: activity; Debye-Hückel theory; electrolytic conductivity: conductivity and resistivity; conductivity measurement; independent ion migration law; mobility and transport numbers. Dissemination. Fick's first law, Einstein-Smoluchowski equation, Gauss's theorem of divergence, Fick's second law. Mobility. Einstein equation, Stokes-Einstein equation, Nernst-Einstein equation. Debye-Hückel-Onsager equation.
6 hours of frontal lecture

Chemical kinetics: reaction speed, velocity constants and kinetic laws. Reaction order. Kinetic laws in integrated form. Reactions of order 0, of the I, II and III order. Pseudo-order. Half-life. Molecularity of reactions. Elementary and non-elementary reactions. Kinetics of equilibrium reactions, consecutive and competitive reactions.
The dependency of the reaction speed from the temperature. Arrhenius equation. The origin of the Arrhenius parameters. Collision theory. Theory of the activated complex and of the transition state. Enthalpy and activation entropy.
5 hours of frontal lecture

Catalysis. Homogeneous and heterogeneous catalysts. Micellar catalysis. Enzymes and enzymatic catalysis: the models of Michaelis-Menten and Briggs-Haldane; the biochemical-physical meaning of Michaelis's constant; graphical representations of experimental data. Enzyme inhibitors: competitive, non-competitive and incompetitive inhibition.
4 hours of frontal lecture

Heterogeneous catalysis: Nernst diffusion layer. Surfactants: general characteristics and their classification. Monolayer bi and multilayer. Surfactants and critical micellar concentration. Micellar catalysis. Dispersed systems: properties and characteristics. Surface tension. Surface excess, the Gibbs adsorption isotherm.
5 hours of frontal lecture

Colloids: classification and main characteristics. Stability of colloids. The potential of Lennard Jones. The thermodynamics of formation of micelles. The double electric layer. Double layer overlap. DLVO theory. Flocculation and coagulation. Steria stabilization
5 hours of frontal lecture

Thermodynamics of non-equilibrium. Thermostatics and thermodynamics: from equilibrium to steady state; reversibility and irreversibility. Curie Theorem, Prigogine Theorem, Law of Onsager. The dissipation function; thermodynamic systems, chemical reactions and irreversible processes; relaxation time, reaction speed and dissipation function; theory of absolute reaction speed; partition functions; stability of steady-state systems.
6 hours of frontal lecture

Properties of biological membranes. Passive transport. Facilitate transport: kinetic approach and nonequilibrium thermodynamics approach. Main principles of active transport.
4 hours of frontal lecture

Thermodynamics and sustainable development. Steady state economics. Entropy and economic processes. The law of entropy. Bioeconomy. Indicators of ecological sustainability: Exergy and Emergy.
2 hours of frontal lecture

Adopted texts

Lecture notes of the teacher are available on the e-learning website of the course: http://elearning2.uniroma1.it/mod/folder/view.php?id=10782
Although a specific text is not required, further in-depth studies need to refer to some fundamental books including: 1) P. W. Atkins - CHIMICA FISICA, Zanichelli (IV o V edizione); 2) C. Botrè: "Principi di Bioirreversibilità", Bulzoni Editore, 1976 3) C. Botrè: "Le Basi Chimico-Fisiche della Farmacologia", Editore Grasso, 1984; 4)

Prerequisites

We strongly recommend that you have taken the following first-year exams: Mathematics: for the knowledge of logarithms, properties of vectors and scalars, study of functions, derivatives and integrals; Physics: for fundamental laws, work and energy, energy distribution Inorganic Chemistry: general principles and properties of solutions

Frequency modes

Attendance to the course is optional but recommended.

Exam modes

The assessment methods of the course are characterized by an oral exam call fixed each month of the year, excluding the months of August and December. The exam is open for 15-20 days to give students the opportunity to choose the most appropriate date to take the exam. The vote is expressed in thirtieths, with possible praise. Passing the exam presupposes the conferment of a grade of not less than eighteen / thirty and involves the assignment of the corresponding university credits. In the evaluation of the tests for the purpose of the assignment of the final grade, the following will be taken into account: the level of knowledge of the demonstrated contents (superficial, appropriate, precise and complete, complete and in-depth), the ability to apply the theoretical concepts (errors in applying the concepts, discrete, good, well established), the capacity for analysis, synthesis and interdisciplinary links (sufficient, good, excellent), the capacity for critical sense and the formulation of judgments (sufficient, good, excellent), the mastery of expression (deficient, simple, clear and correct, safe and correct).
In general, we start from very general questions about the main concepts of thermodynamics and / or kinetics, followed by more specific and more detailed questions about the application of the principles studied to describe real phenomena. To pass the exam, the mnemonic study is not recommended, but the understanding of the main concepts is required in a preponderant manner. The ability to connect and compare the topics held in different parts of the Physical Chemistry course and/or in other courses is particularly appreciated. Numerical examples may also be processed during the test. 
A sufficient knowledge of the arguments is required to pass the examination with the minimum mark. To obtain the maximum mark, the student has to show a very good knowledge of all the arguments and to be able to reply to the required questions clearly and with suitable scientific language.

Exam reservation date start Exam reservation date end Exam date
01/09/2021 02/02/2022 03/02/2022
01/09/2021 02/02/2022 03/02/2022
01/02/2022 03/03/2022 04/03/2022
01/02/2022 03/04/2022 04/04/2022
01/02/2022 03/05/2022 04/05/2022
01/02/2022 15/06/2022 16/06/2022
01/02/2022 15/06/2022 16/06/2022
01/02/2022 04/07/2022 05/07/2022
01/02/2022 04/07/2022 05/07/2022
01/02/2022 04/09/2022 05/09/2022
01/02/2022 04/09/2022 05/09/2022
01/09/2022 04/11/2022 07/11/2022
01/09/2022 04/11/2022 07/11/2022
01/09/2022 02/12/2022 05/12/2022
01/09/2022 02/12/2022 05/12/2022
01/02/2022 20/01/2023 23/01/2023
01/02/2022 20/01/2023 23/01/2023

M - Z

FRANCO MAZZEI FRANCO MAZZEI   Teacher profile

Programme

Classical Thermodynamics.
Introduction. Definition of system, environment, variables or thermodynamic functions. States of equilibrium and thermodynamic transformations. Heat and Work. Calorimetry.
The first principle. Internal energy. Thermal capacity and specific heat. Application of the first principle to perfect gases.
Enthalpy. Enthalpy of reactions in the gaseous phase. Enthalpy of physical, atomic and molecular transformations. Thermochemistry. Law of Hess. Enthalpy training standard. Variation of enthalpy with temperature: Kirchhoff's law. Joule-Thomson effect.
6 hours frontal lecture

The second principle. Utterances. Spontaneous transformations. Reversibility and irreversibility.
Entropy. Definition of thermodynamics. Clausius inequality. Reversible and irreversible isothermal expansion of a perfect gas. Adiabatic transformations. Thermodynamic cycles. Theorem and Carnot cycle. Variation of entropy with temperature.
Third principle. Nernst's theorem. Boltzmann report.
5 hours of frontal lecture

Helmholtz energy and Gibbs energy. Maximum work function. Free reaction energy. The fundamental equation of thermodynamics. Maxwell reports. Thermodynamic state equation. Variation of Gibbs energy with pressure and temperature. Gibbs-Helmholtz equation. Fugacity and activity. Partial molar quantities. Chemical potential. Thermodynamic equilibrium criterion. Reaction quotient and equilibrium constant. The Boltzmann equilibrium constant and distribution. Le Chatelier's principle. Van't Hoff equation.
6 hours of frontal lecture

The physical transformations of pure substances. State diagrams: critical point, boiling point and melting point, triple point. The water status diagram. Clapeyron equation. The properties of simple blends. Thermodynamic description of the mixtures. Partial molar quantities. The molar partial volume. Partial molar Gibbs energy. The Gibbs-Duhem equation. Thermodynamic mixing quantities. The chemical potential of liquids. The ideal solutions. Raoult's law. The ideal diluted solutions. Henry's law. Colligative properties: elevated ebullioscope, cryoscopic and osmotic pressure. Solvent activity. The activity of the solute. Ideal diluted solutions. Real solutions.
6 hours of frontal lecture

Phase equilibria: Mix state diagrams. Two-component systems and temperature-composition diagrams. Liquid-liquid status diagrams for partially miscible two-component systems. Liquid-vapor state diagrams for volatile liquid mixtures: characteristic vapor pressure curves; pressure-composition and temperature-composition diagrams; simple and fractional distillation; azeotropes.
4 hours of frontal lecture

Properties of electrolyte solutions: activity; Debye-Hückel theory; electrolytic conductivity: conductivity and resistivity; conductivity measurement; independent ion migration law; mobility and transport numbers. Dissemination. Fick's first law, Einstein-Smoluchowski equation, Gauss's theorem of divergence, Fick's second law. Mobility. Einstein equation, Stokes-Einstein equation, Nernst-Einstein equation. Debye-Hückel-Onsager equation.
6 hours of frontal lecture

Chemical kinetics: reaction speed, velocity constants and kinetic laws. Reaction order. Kinetic laws in integrated form. Reactions of order 0, of the I, II and III order. Pseudo-order. Half-life. Molecularity of reactions. Elementary and non-elementary reactions. Kinetics of equilibrium reactions, consecutive and competitive reactions.
The dependency of the reaction speed from the temperature. Arrhenius equation. The origin of the Arrhenius parameters. Collision theory. Theory of the activated complex and of the transition state. Enthalpy and activation entropy.
5 hours of frontal lecture

Catalysis. Homogeneous and heterogeneous catalysts. Micellar catalysis. Enzymes and enzymatic catalysis: the models of Michaelis-Menten and Briggs-Haldane; the biochemical-physical meaning of Michaelis's constant; graphical representations of experimental data. Enzyme inhibitors: competitive, non-competitive and incompetitive inhibition.
4 hours of frontal lecture

Heterogeneous catalysis: Nernst diffusion layer. Surfactants: general characteristics and their classification. Monolayer bi and multilayer. Surfactants and critical micellar concentration. Micellar catalysis. Dispersed systems: properties and characteristics. Surface tension. Surface excess, the Gibbs adsorption isotherm.
5 hours of frontal lecture

Colloids: classification and main characteristics. Stability of colloids. The potential of Lennard Jones. The thermodynamics of formation of micelles. The double electric layer. Double layer overlap. DLVO theory. Flocculation and coagulation. Steria stabilization
5 hours of frontal lecture

Thermodynamics of non-equilibrium. Thermostatics and thermodynamics: from equilibrium to steady state; reversibility and irreversibility. Curie Theorem, Prigogine Theorem, Law of Onsager. The dissipation function; thermodynamic systems, chemical reactions and irreversible processes; relaxation time, reaction speed and dissipation function; theory of absolute reaction speed; partition functions; stability of steady-state systems.
6 hours of frontal lecture

Properties of biological membranes. Passive transport. Facilitate transport: kinetic approach and nonequilibrium thermodynamics approach. Main principles of active transport.
4 hours of frontal lecture

Thermodynamics and sustainable development. Steady state economics. Entropy and economic processes. The law of entropy. Bioeconomy. Indicators of ecological sustainability: Exergy and Emergy.
2 hours of frontal lecture

Adopted texts

Lecture notes of the teacher are available on the e-learning website of the course: http://elearning2.uniroma1.it/mod/folder/view.php?id=10782
Although a specific text is not required, further in-depth studies need to refer to some fundamental books including: 1) P. W. Atkins - CHIMICA FISICA, Zanichelli (IV o V edizione); 2) C. Botrè: "Principi di Bioirreversibilità", Bulzoni Editore, 1976 3) C. Botrè: "Le Basi Chimico-Fisiche della Farmacologia", Editore Grasso, 1984; 4)

Prerequisites

We strongly recommend that you have taken the following first-year exams: Mathematics: for the knowledge of logarithms, properties of vectors and scalars, study of functions, derivatives and integrals; Physics: for fundamental laws, work and energy, energy distribution Inorganic Chemistry: general principles and properties of solutions

Frequency modes

Attendance to the course is optional but recommended.

Exam modes

The assessment methods of the course are characterized by an oral exam call fixed each month of the year, excluding the months of August and December. The exam is open for 15-20 days to give students the opportunity to choose the most appropriate date to take the exam. The vote is expressed in thirtieths, with possible praise. Passing the exam presupposes the conferment of a grade of not less than eighteen / thirty and involves the assignment of the corresponding university credits. In the evaluation of the tests for the purpose of the assignment of the final grade, the following will be taken into account: the level of knowledge of the demonstrated contents (superficial, appropriate, precise and complete, complete and in-depth), the ability to apply the theoretical concepts (errors in applying the concepts, discrete, good, well established), the capacity for analysis, synthesis and interdisciplinary links (sufficient, good, excellent), the capacity for critical sense and the formulation of judgments (sufficient, good, excellent), the mastery of expression (deficient, simple, clear and correct, safe and correct).
In general, we start from very general questions about the main concepts of thermodynamics and / or kinetics, followed by more specific and more detailed questions about the application of the principles studied to describe real phenomena. To pass the exam, the mnemonic study is not recommended, but the understanding of the main concepts is required in a preponderant manner. The ability to connect and compare the topics held in different parts of the Physical Chemistry course and/or in other courses is particularly appreciated. Numerical examples may also be processed during the test.

Exam reservation date start Exam reservation date end Exam date
01/09/2021 02/02/2022 03/02/2022
01/09/2021 02/02/2022 03/02/2022
01/02/2022 03/03/2022 04/03/2022
01/02/2022 03/04/2022 04/04/2022
01/02/2022 03/05/2022 04/05/2022
01/02/2022 15/06/2022 16/06/2022
01/02/2022 15/06/2022 16/06/2022
01/02/2022 04/07/2022 05/07/2022
01/02/2022 04/07/2022 05/07/2022
01/02/2022 04/09/2022 05/09/2022
01/02/2022 04/09/2022 05/09/2022
01/09/2022 04/11/2022 07/11/2022
01/09/2022 04/11/2022 07/11/2022
01/09/2022 02/12/2022 05/12/2022
01/09/2022 02/12/2022 05/12/2022
01/02/2022 20/01/2023 23/01/2023
01/02/2022 20/01/2023 23/01/2023
Course sheet
  • Academic year: 2021/2022
  • Curriculum: Curriculum unico
  • Year: Second year
  • Semester: Second semester
  • SSD: CHIM/02
  • CFU: 8
Activities
  • Attività formative affini ed integrative
  • Ambito disciplinare: Attività formative affini o integrative
  • Lecture (Hours): 64
  • CFU: 8
  • SSD: CHIM/02