PHYSICAL CHEMISTRY I AND LABORATORY
Learning outcomes of the course unit
The educational objectives of the PHYSICAL CHEMISTRY I AND LAB Course agree with those foreseen by the Degree Course Council:
Knowledge and ability to understand
- possesses basic knowledge of the characteristics of the different states of matter and theories used to describe them;
- possesses basic knowledge of the principles of thermodynamics, electrochemistry, kinetic gas theory and chemical kinetics and their applications in chemistry;
-It has basic knowledge of chemical transformations, including catalysis, and the mechanistic interpretation of reactions
Ability to apply knowledge and understanding
- is able to perform elementary energy balance calculations, determinations of equilibrium constants, kinetic constants and reaction orders;
- is able to collect scientific data through laboratory observations and measurements, to elaborate and interpret them;
- is able to use chemical-physical techniques and methodologies to derive molecular properties and for structural recognition;
- possesses basic IT skills related to operating systems, word processing, spreadsheets, use of databases;
Autonomy of judgment
The student :
- is able to collect and critically evaluate, present and discuss the experimental results acquired in collaborative activities;
- is capable of planning and conducting an experiment, also planning time and modalities;
- is able to find and analyze sources of information in literature and in chemical databases;
-is able to handle substances in safe conditions, to classify waste substances, processing residues and dispose of them correctly;
is able to correlate the data and results acquired experimentally with theoretical models;
- is able to communicate, both in oral and written form in the context of professional activities and relationships, with a strict respect for the chemical language;
- is capable of interacting, communicating with properties of language and method and collaborating profitably even in a purposeful way with other people;
- is capable of processing and presenting experimental data even with the aid of multimedia systems;
- is able to interact with other staff on the implementation of procedures and the necessary safety measures in the chemical field.
The student :
- is able to undertake higher level academic studies with a sufficient degree of autonomy or to continue his professional training;
- is able to work by objectives, in groups or independently;
- is able to adapt to different working environments and themes;
-is able to interpret, in an autonomous way, data of scientific technical literature, especially in the practical-applicative field.
Basic notions of general chemistry, of general physics, and of calculus.
Course contents summary
1. The zero law of thermodynamics and the gas properties. 2. The First law of Thermodynamics. 3. The second law of Thermodynamics. 4. The Gibbs energy and the chemical potentials. 5. Physical transformations of pure substances. 6. The solutions. 7. Phase diagrams. 8. Chemical equilibrium. 9. Chemical kinetics.
1. The zero law of thermodynamics and the gas properties. Primitive concepts: system, environment. Thermodynamic state functions. The temperature and the zero Law of thermodynamics. The state equation of the ideal gas. Real gases. Van der Waals equation. The principle of corresponding states.
2. The First law of Thermodynamics. Work, heat and internal energy. The first law of thermodynamics. Expansion work. Heat capacity. The properties of the internal energy. The enthalpy and the transformations at constant pressure. Transformations of the ideal gas. Thermochemistry. Variations of enthalpy in chemical reactions and phases transformations. Standard state of elements and compounds. The standard enthalpies of formation and the reaction enthalpies. The Hess law. The temperature dependence of reaction enthalpies.
3. The second law of Thermodynamics. The Kelvin and Clausius formulations of the second law. The entropy. The Carnot cycle. The Clausius inequality and the irreversible transformations. Variations of entropy in elementary transformations. The third law of Thermodynamics. The molecular interpretation of the entropy. Criterion for spontaneity for isolated systems. The Helmoltz energy and the spontaneous transformations at constant volume and temperature . The Gibbs free energy and the spontaneous transformations at constant pressure and temperature.
4. The Gibbs energy and the chemical potentials. The fundamental equation of thermodynamics. The Maxwell relations. The effects of the pressure and temperature on the Gibbs energy. The chemical potential of pure substances. The chemical potential of real gases.
5. Physical transformations of pure substances. Phases diagrams. The stability of phases. Phases boundaries. The triple point and the critical point. The thermodynamic criterion of the phases equilibrium. The Clapeyron equation and the phase boundaries. The Ehrenfest classification of the phase transitions.
6. The solutions. Partial molar quantities. Chemical potentials. The Gibbs-Duhem equation. The thermodynamics of mixing. Chemical potentials in ideal solutions. The Raoult law. The Henry law. The properties of solutions. Excess functions. Colligative properties. The thermodynamic activities. The solvent activity. The solute activity. The regular solutions.
7. Phase diagrams. Phases, components and degrees of freedom. The Gibbs phases rule. Two components systems. Vapor-liquid phases diagrams. Liquid-liquid phases diagrams. Liquid-solid phases diagrams.
8. Chemical equilibrium. The Gibbs free energy of reaction and the spontaneity of chemical reactions. The standard free energy of reaction, the reaction quotient and the equilibrium constant. Reactions between ideal gases. Reactions in solution. The effect of temperature and pressure on the chemical equilibrium.
9. Chemical kinetics. The reaction rate: definition and measurements. The kinetic laws and the order of reaction. Integrated forms of the zero, first and second order kinetic laws. The effect of the temperature on the reaction rates. Catalysis.
Peter W. Atkins,Julio De Paula, Chimica Fisica, 5a Ed., Zanichelli, 2012.
The teaching activities consist of Lectures, including tutoring seminars, and of Laboratory practice sessions. The slides used during the Lectures will be weekly uploaded on the Elly platform. The slides will be part of the teaching material along with the reference text book.
Assessment methods and criteria
The final verifications will consist of:
- a critical discussion on the written reports of the experiences performed during the laboratory practice, with evaluation scale 0-30 and weight 0.25
- a written examination (2h) with open answers, and with evaluation scale 0-30 and weight 0.25
- an oral examination, with evaluation scale 0-30 and weight 0.50.