Introduction to Physical Chemistry
Objectives
The overall objective of Introduction to Physical-Chemistry is to provide the fundamental scientific background and practical training in Chemistry that are the basis for the understanding of the world around us. A key general objective is the development of qualitative and quantitative problem-solving skills. Of comparable importance is to learn proper laboratory practices, execute experiments, interpret experimental results and draw reasonable conclusions. Specific learning objectives for this course include the development of conceptual understanding of: bulk properties and models of gases, liquids and solids; thermodynamic laws and their relation with equilibrium - entropy and free energy concepts; physical and chemical equilibria; acqueous equilibria; electrochemistry and chemical kinetics.
General characterization
Code
10690
Credits
6.0
Responsible teacher
Ana Isabel Nobre Martins Aguiar de Oliveira Ricardo
Hours
Weekly - 4
Total - 62
Teaching language
Português
Prerequisites
Available soon
Bibliography
-“Chemical Principles. The Quest for Insight”, P.Atkins and L. Jones, Freeman 5th ed.(2010).
- Chemical Principles Student Solutions Manual, C. Hoeger, L. Lavelle and Y. Ma 6th ed. (2013), ISBN: 978-1-4641-0707-8.
-Química, R. Chang & K. A. Goldsby, McGraw-Hill 11th ed.
Teaching method
The course is organized into lectures (T 28h), problem-solving sessions (TP, 21h) and lab sessions (P, 15h). Fundamentals are explained during the lectures, using data show and challenging the students to solve and think about new problems. Prior to each TP class, problem-sheets are offered to students to be solved before each TP session, and demonstrated in class. The lab classes follow the method of directed study, students are organized in groups of three and the work done is evaluated at the end of each lab session. It is provided access to a page – moodle - containing all course material and related information.
Evaluation method
Final classification:
1/5 (practical grade) + 1/5 (theoretical-practical grade) + 3/5 (theoretical grade) (requires the completion of theoretical-practical questionnaires (Moodle mini-tests).
Theoretical frequency:
Course attendance is obtained by completing 5 Moodle Mini-Tests and attending 50% of T classes and 50% of TP classes.
Practical frequency:
The practical frequency of the discipline is obtained through the completion of all practical work.
Theoretical-practical grade: Average rating of the 5 Moodle mini-tests.
Theoretical note: The assessment of the subjects will include 3 tests lasting a maximum of 90 minutes. To pass the subject, the final average of the 3 tests must be greater than or equal to 9.5.
Practical note: - evaluation of the results obtained in all practical work.
ATTENTION: The practical grade is only valid in the year in which it is made. After this period of time, practical attendance at the course remains but the grade is lost. The final grade is now calculated based on 4/5 of the theoretical grade and 1/5 of the theoretical-practical grade.
In tests and exams, you can use scientific or graphing calculators as long as they are in exam mode
Subject matter
1.1.Intermolecular forces.
1.1.1.Solids, liquids and gases.
1.1.2.Phase transitions.
1.1.3.Phase diagrams for pure substances
1.1.4.Ideal gases and real gases.
1.1.5.State equations.
1.2.Thermochemistry.
1.2.1.Revision of concepts: sistems, work, energie and heat.
1.2.2.Calorimetry. Specific heat and heat capacity.
1.2.3.1st Law of Thermodynamics.
1.2.4.Energy transfer in chemical reactions.
1.2.5.Enthalpy. Formation Enthalpy and reaction Enthalpy.
1.3.Entropy, Gibbs energy and equilibrium.
1.3.1.Spontaneous processes.
1.3.2.Entropy and the 2nd law of Thermodynamics.
1.3.3.Total entropy chnages.
1.3.4.Gibbs energy.
1.3.5.Gibbs energy and chemical equilibrium.
1.4. Physical equilibrium
1.4.1.Phase transitions and phase diagrams.
1.4.2.Solubility.
1.4.3.Colligative properties.
1.4.4. Binarymixtures. Ideal solutions. Raoult Law.
1.5. Chemical Equilibrium.
1.5.1.The concept of chemical equilibrium. Ways of expressing equilibrium constants.
1.5.2.Factors that affect chemical equilibrium. Le Châtelier Principle.
1.6. Acid-Base Equilibria.
1.6.1.Conjugate acid-base pair. The ion product of water and the pH scale.
1.6.2.pH of solutions.
1.6.3.Buffer solutions
1.7. Solubility.
1.7.1.Solubility equilibria and solubility product.
1.7.2.Common ion effect.
1.7.3.Applications.
1.8. Electrochemistry
1.8.1.Galvanic Cells. Schematic representation of galvanic cells.
1.8.2.Standard electrode potentials.
1.8.3.Nernst equation.
1.8.4.Electrolytic Cell.
1.8.5.Electrolysis.
1.9.Chemical kinetics.
1.9.1.The rate of reactions.
1.9.2.Rate laws. Experimental determination of rate law.
1.9.3.Arrhenius Law and activation energy.
1.9.4. Reaction mechanisms. Elementary steps. Molecularity.
1.9.5.Introduction to the collision theory and activated complex theory.