Complementary Physical Chemistry

Code:

Q3010

Acronym:

Q3010

Level:

300

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2022/2023 - 1S

Active?	No
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	Bachelor in Chemistry

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:Q	0	study plan from 2016/17	3	-	6	56	162

Teaching language

Portuguese

Objectives

Learning outcomes and competences

The principles of Physical Chemistry are a framework for all other areas of Chemistry.

Chemical Engineering uses thermodynamics to predict the equilibrium composition of reaction mixtures, reactor design and eventual temperature control systems. Chemical Kinetics is an important topic because while thermodynamics tells us what spontaneous change is about, it tells us nothing about how quickly processes will occur; chemical kinetics is essential in predicting the speed of obtaining products and in designing new processes, using catalysts, where the physical chemistry of the interface also plays an important role; the thermodynamic principles of phase equilibria are of the utmost relevance in the separation of products. The Physical Chemistry of heterogeneous systems and the interface is of great interest in obtaining new materials in the metallurgical, ceramics, polymers, pharmaceutical, cosmetics or food industries.

It is therefore intended that students acquire and consolidate knowledge that allows them to better integrate Chemistry subjects taught in other curricular units, in order to better face the challenges they will encounter in their professional activity or in future academic courses.

Working method

Presencial

Program

1 Thermodynamics of heterogeneous equilibrium in multi component systems

Temperature-composition phase diagrams for binary ideal or quasi ideal mixtures of volatile liquids : Gibb´s Phase rule and Lever rule

Excess Functions, regular solutions, gaps of miscibility; Liquid–liquid phase diagrams and phase separation 

Solid solutions and gaps of miscibility
Liquid- solid phase diagrams of isomorphous (complete solid solubility) and eutectic  (solid immiscibility) binary systems

Phase Behavior in Ternary Systems: Gibbs phase rule and  Lever rule; triangular phase diagrams (or compositional diagrams at Constant T and P) for some simple systems

2. Interface thermodynamics in heterogeneous systems

Surfaces and interfaces in polyphasic systems.
Surface or interfacial tension and excess Gibbs function.

Curving of liquid surfaces-Laplace and Kelvin equations: their consequences
Adsorption on liquid surfaces and liquid-liquid interfaces: Gibbs adsorption isotherm.
Amphiphilic molecules and interfaces: their effect on surface tension of liquids, formation of insoluble films on liquid surfaces and stabilization of  colloidal dispersions.

Solid surfaces; surface tension and adsorption of gases or solutes of a liquid solution:La ngmuir, Freundlich and Bet adsorption isotherms; modification of properties of solid surfaces

3. Chemical Kinetics

Mechanisms and laws of velocities of complex reactions: reversible reactions-approximation of equilibrium; first-order parallel reactions (kinetic and thermodynamic velocity controls), chain reactions (initiation, propagation, and closing steps) and derivation of kinetic laws using steady-state approximation to intermediate species;
unimolecular reactions and the Lindemann-Hinshelwood mechanism; explosive reactions; photochemical reactions and quantum yield; mechanisms of homogeneous and heterogeneous catalysis.

The kinetic theory of collisions and the specific velocity of bimolecular reactions in the gaseous state.
Theory of transition state or activated complex; the Eyring equation, for the calculation of the specific velocity of a bimolecular process in the gaseous state, using statistical thermodynamic results; thermodynamic parameters of activation.

The theory of collisions, the theory of the activated complex and the experimental law of Arrhenius; theoretical predictive models versus a relation obtained experimentally between specific velocity and temperature.

Effects of the solvent on the reaction rates in solution: diffusion controlled reactions or formation of the activated complex. Effect of the ionic strength on the specific rate of reactions between ions in solution.

Mandatory literature

Atkins P. W.; Physical chemistry. ISBN: 0-19-855284-X
Shaw Duncan J.; Introduction to colloid and surface chemistry. ISBN: 0-408-71049-7
Levine Ira N.; Physical chemistry. ISBN: 0-07-113472-7

Teaching methods and learning activities

Lectures and practical classes of theoretical discussion and problem solving.

Evaluation Type

Distributed evaluation with final exam

Assessment Components

designation	Weight (%)
Teste	50,00
Exame	50,00
Total:	100,00

Amount of time allocated to each course unit

designation	Time (hours)
Estudo autónomo	106,00
Frequência das aulas	56,00
Total:	162,00

Eligibility for exams

Terms of frequency: The students must have no more absences then that 1/4 of the total number of the theorethical and theoretical-practical classes.

Calculation formula of final grade

Type of evaluation: distributed with final exam.

Formula Evaluation for distributed evaluation: The final classification is the weighted average of the grades obtained in the two tests (T1 and T2) one realized during the semester and the second in exam  


At the time of appeal the exam is an overall test

Internship work/project

Special assessment (TE, DA, ...)

Students with special status can opt by final exam

Classification improvement

Exam