Identifying Data

2020/21

Subject (*)

Physical Chemistry 3

Code

610G01018

Study programme

Grao en Química

Descriptors

Cycle

Period

Year

Type

Credits

Graduate

1st four-month period

Third

Obligatory

Language

Spanish

English

Teaching method

Hybrid

Prerequisites

Department

Química

Coordinador

Herrero Rodriguez, Roberto

E-mail

r.herrero@udc.es

Lecturers

Barriada Pereira, José Luis

Herrero Rodriguez, Roberto

E-mail

jose.barriada@udc.es

r.herrero@udc.es

Web

http://campusvirtual.udc.es/moodle

General description

A Química Física é o estudo dos principios físicos fundamentais que gobernan as propiedades e o comportamento dos sistemas químicos. Un sistema químico pode estudarse dende un punto de vista microscópico ou macroscópico. Neste curso de Química Física introdúcese a metodoloxía do estudo macroscópico de equilibrio (Termodinámica Química)
Os contidos que se imparten nesta asignatura constituen os fundamentos teóricos imprescindibles para as seguintes asignaturas de Química Física e un marco de referencia para todas as demáis ramas da Química que, necesariamente, aplican boa parte dos conceptos estudiados nesta asignatura no desenvolvemento dos seus programas específicos.

Contingency plan

1. Modificacións nos contidos, Ninguha

2. Metodoloxías
*Metodoloxías docentes que se manteñen

*Metodoloxías docentes que se modifican. As metodoloxías docentes se modificarán para pasar a realizarse en modalidade online

3. Mecanismos de atención personalizada ao alumnado
Correo electrónico, Plataforma Moodle, y Microsoft Teams

4. Modificacións na avaliación

*Observacións de avaliación: Mantense a mesma avaliación pero terá que facerse online.

5. Modificacións da bibliografía ou webgrafía

Study programme competencies

Code	Study programme competences
A1	Ability to use chemistry terminology, nomenclature, conventions and units
A3	Knowledge of characteristics of the different states of matter and theories used to describe them
A5	Understanding of principles of thermodynamics and its applications in chemistry
A14	Ability to demonstrate knowledge and understanding of concepts, principles and theories in chemistry
A15	Ability to recognise and analyse new problems and develop solution strategies
A16	Ability to source, assess and apply technical bibliographical information and data relating to chemistry
A21	Understanding of qualitative and quantitative aspects of chemical problems
B2	Effective problem solving
B3	Application of logical, critical, creative thinking
C3	Ability to use basic information and communications technology (ICT) tools for professional purposes and learning throughout life

Learning aims

Learning outcomes	Study programme competences
To know the principles of thermodynamics and their applications in chemistry	A1 A3 A5 A14 A15 A16 A21	B2 B3	C3
To solve complex problems through the use of spreadsheets.	A1 A14 A15 A16 A21	B2 B3	C3
To adquire skills in literature search of real and research applications about the subject contents of the course	A14 A15 A16 A21	B3	C3

Contents

Topic	Sub-topic
1. Introduction to Chemical Thermodynamics.	Previous concepts and mathematical properties
2. The principles of Thermodynamics.	First law: internal energy, enthalpy, heat capacities. Second law: entropy, calculating the entropy change in simple systems.
3. Thermodynamic potentials and evolution of systems	Equilibrium conditions in closed systems: the Gibbs and Helmholtz functions. Thermodynamic relationships for a closed system. Applications: thermodynamic equations of state, the difference between the heat capacities, the Joule-Thomson coefficient.
4. Thermodynamics standard reaction functions	Standard enthalpy: Kirchhoff's and Hess's law. Standard Entropy: the third law of thermodynamics, conventional entropy determination. Standard Gibbs energy. Using thermodynamic tables.
5. Thermodynamics of systems of variable composition	The chemical potential. Partial molar properties. Material equilibrium conditions: phase equilibrium and chemical equilibrium.
6. Gas state thermodynamics	The ideal gas: chemical potential and properties, ideal gas mixture. Real gases: equation of state and fugacity, fugacity calculation.
7.Phase equilibria in systems of one component	The phase rule. Phase diagram for one-component systems. Clapeyron and Clausius-Clapeyron equations. Classification of phase transitions.
8. Solutions	Ideal solution: Raoult's Law. Ideally dilute solution: Henry's Law. Mixing functions. Nonideal solutions of nonelectrolytes: activity and activity coefficients, the Gibbs-Duhem equation, excess functions. Solutions of electrolytes: the activity coefficient of ionic species.
9. Phase equilibria in multicomponent systems	Liquid-vapor equilibrium: ideal solution at constant T and P constant, fractional distillation, azeotropic mixtures. Liquid-liquid equilibrium: miscibility. Solid-liquid equilibrium: temperature-composition diagrams, simple eutectic, compound formation with congruent and incongruent melting, thermal analysis. Solution-crystalline solid equilibrium. Colligative properties: freezing point depression, boiling point elevation, osmotic pressure, vapor-pressure lowering. Nernst's distribution law.
10. Chemical equilibrium	Chemical equilibrium in gas mixtures: the equilibrium constant, changes in chemical equilibrium-Le Chatelier's principle. Chemical equilibrium in solution. Chemical equilibrium with pure solids and liquids.
11. Surface thermodynamics	The interface: surface tension. Curved interfaces: capillary rise. Adsorption on solid: physisorption and chemisorption, adsorption isotherms.
12. Electrochemical equilibrium	Electrochemical systems. Thermodynamics of electrochemical systems: the electrochemical potential. Galvanic and electrolytic cells. Nernst equation and standard electrode potentials. Types of reversible electrodes. Liquid junction potentials. Determination of thermodynamic parameters.

Planning

Methodologies / tests	Competencies	Ordinary class hours	Student’s personal work hours	Total hours
Problem solving	A1 A5 A14 A15 A21 B2 B3	11	33	44
Guest lecture / keynote speech	A1 A3 A5 B3	30	60	90
ICT practicals	A14 B2 B3 C3	0.5	1.5	2
Critical bibliographical	A16 C3	0.5	1.5	2
Mixed objective/subjective test	A1 A3 A5 A14 A21 B2 B3	8	0	8
Mixed objective/subjective test	A1 A3 A5 A14 A15 A21 B2 B3	4	0	4

Personalized attention		0	0	0

(*)The information in the planning table is for guidance only and does not take into account the heterogeneity of the students.

Methodologies

Methodologies	Description
Problem solving	Seminars in small groups where it will be shown the application of the theoretical contents from the lectures into problem solving
Guest lecture / keynote speech	Lectures, where the theoretical concepts will be introduced
ICT practicals	Practical exercises where students will solve complex problems using computer programs
Critical bibliographical	Students will be taught to do bibliographic search. They will be asked to perform searches about topics related with the subject. Reading of papers related with topics from the subject will be also proposed
Mixed objective/subjective test	Students will be asked to solve a collection of problems which combines the theoretical concepts and their application. Two of these tests will be done in the semester.
Mixed objective/subjective test	A final test will be done at the end of the semester. Students will be asked solving problems on their own

Personalized attention

Methodologies

Description

These works are proposed in the class and students must solve them supported by individual tutorials with the teacher.

Part-time students and those with special academic leave permission will have access to the materials of the subject in the moodle application. They could ask for presential or email tutorials when necessary while they prepare for the final test.

Assessment

Methodologies	Competencies	Description	Qualification
Mixed objective/subjective test	A1 A3 A5 A14 A15 A21 B2 B3	Final examination of the contents of the subject based on the autonomous, individual resolution of problems. The final qualification obtained it will be the best of the following results: 20% of the tests done in the semester + 80% of the final test OR 100% of the final test	80
Mixed objective/subjective test	A1 A3 A5 A14 A21 B2 B3	The tests will be done along the semester. It will be assessed the individual contribution to the resolution of all activities. These tests do not eliminate contents to be evaluated in the final test. The qualifications obteined can contribute up to a 20% of the final qualification (10% each test)	20

Assessment comments
The student who engages in any of the two tests will be considered to have attended on the subject at the time of the final mark. The qualifications obtained will correspond to January (first opportunity). Exceptionally, the rating of both opportunities will be made with the final test, scoring 10 out of 10, for those student with special academic leave permission. The rating of the second opportunity will be made only with a final test, scoring 10 out of 10. Honors grade: priority is given in the first opportunity. Honors grade may only be granted in the second opportunity if their number have not be exhausted in the first opportunity final qualifications. Should it be more candidates to honors grade than honors available, allocation will be done through a extraordinary exam.

Sources of information

Basic
	§LEVINE, I.N. (2008). Physical Chemistry. 6th Ed. McGraw-Hill. §ATKINS, P.W and de Paula, J. (2010). Physical Chemistry. 9 Ed. Oxford University Press
Complementary
	§ DENBIGH, K. (1981). The principles of chemical equilibrium. Cambridge University Press § McQUARRIE, D.A., SIMON, J.D. (1997). Physical Chemistry. Univ. Science Books. § KLOTZ, I.M., ROSENBERG, R.M. (2008) Chemical Thermodynamics 7th Ed. Wiley

Recommendations

Subjects that it is recommended to have taken before

Mathematics 1/610G01001

Mathematics 2/610G01002

Physics 1/610G01003

Physics 2/610G01004

General Chemistry 2/610G01008

Subjects that are recommended to be taken simultaneously

Experimental Physical Chemistry/610G01019

Subjects that continue the syllabus

Experimental Physical Chemistry/610G01019

Advanced Physical Chemistry/610G01020

Other comments

(*)The teaching guide is the document in which the URV publishes the information about all its courses. It is a public document and cannot be modified. Only in exceptional cases can it be revised by the competent agent or duly revised so that it is in line with current legislation.