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2020/2021

Chemical Equilibrium

Code: 102412 ECTS Credits: 6
Degree Type Year Semester
2500897 Chemical Engineering OB 1 2
The proposed teaching and assessment methodology that appear in the guide may be subject to changes as a result of the restrictions to face-to-face class attendance imposed by the health authorities.

Contact

Name:
Francisco Céspedes Mulero
Email:
Francisco.Cespedes@uab.cat

Use of Languages

Principal working language:
spanish (spa)
Some groups entirely in English:
No
Some groups entirely in Catalan:
No
Some groups entirely in Spanish:
Yes

Prerequisites

Basic knowledge of general chemistry. General knowledge of the elements of the Periodic Table and its reactivities. Formulation and nomenclature of inorganic chemicals.

Objectives and Contextualisation

Context
										
											
										
											The Chemistry Balance course is taught in the Degree in Chemical Engineering as a basic subject within the first academic year. It is an introductory and also finalist course, since it has no continuity in the Curriculum.
										
											
										
											 
										
											
										
											Targets
										
											
										
											Acquire the basic knowledge to understand and solve the problems related to the heterogeneous and homogeneous ion balance in aqueous media. Understand and apply successive approaches to the simplified resolution of systems in balance. Know the acid-base assessments and how to choose an appropriate indicator.

 

 
 
 
 
 

Competences

  • Apply relevant knowledge of the basic sciences, such as mathematics, chemistry, physics and biology, and the principles of economics, biochemistry, statistics and material science, to comprehend, describe and resolve typical chemical engineering problems.
  • Apply scientific method to systems in which chemical, physical or biological transformations are produced both on a microscopic and macroscopic scale.
  • Apply the acquired knowledge and skills to develop a chemical engineering project.
  • Develop personal work habits.
  • Develop thinking habits.

Learning Outcomes

  1. Apply scientific method to the fields of dissolution equilibrium and organic chemistry.
  2. Develop independent learning strategies.
  3. Develop scientific thinking.
  4. Identify the reactions in which changes in oxidation states are produced and understand the principles governing the spontaneity of these reactions as well as the main applications and consequences of electrochemical processes.
  5. Recognise the different processes for acid-base evaluation by means of their curves and be able to choose the suitable indicator.
  6. Recognise the main utensils of the chemical laboratory and use them adequately to carry out basic laboratory operations.
  7. Understand the importance of regulatory dissolutions and apply them to the generation of controlled acidic mediums.
  8. Understand the nature of acid-based equilibriums and analyse them by means of balances of matter and load, both in the case of monoprotic and polyprotic species.
  9. Understand the principles governing the processes of extraction and precipitation and apply them to the interpretation of heterogeneous phase equilibriums.
  10. Use the knowledge acquired in the design of analyses and processes.

Content

 

 
Theoretical content
 
I.- Introduction
Lesson 1: Free energy: criterion of spontaneity. Relationship between DGo and the state of equilibrium. Balance constant of a reaction. Dependence of the equilibrium constant with the temperature. Expressions of the equilibrium constant. Principle of Le Chatelier
Lesson 2: Introduction to the study of ionic balance. Electrolytes Theory of Arrhenius. Characteristics of water as a solvent
 
II. Acid-base equilibrium
Lesson 3: Acids and bases. Historical theories and definitions. Self-ionization of water. Definition of pH. Relative force of an acid-base pair, pKa
Lesson 4: Balance of matter in strong and weak electrolytes. Rule of electronauthenticity. Electric balance. Rigorous pH calculation of an aqueous solution of a base acid pair. General formula
Lesson 5: Calculation of the pH of a dissolution of an acid or a base. Calculation of pH in mixtures of acids and conjugated bases. Regulatory dissolutions of the pH: preparation and properties. Calculation of the pH of mixtures of acid-base pairs. Polypropic acids
Lesson 6: Acid-base volumes. Amortising solution Amortizing capacity Neutralization curves Strong and weak protoples, monoprotic and polyprotics. Acidimetry and alkalimetry. Valuable solutions. Primary types Acid-base indicators
 
III. Balances of complex formation
Lesson 7: Introduction. Agreements. Lewis Acids. Constants of stability and constants of complex formation. Complexes and acids
 
IV.- Precipitation balances
Lesson 8: Solubility and solubility product of a soluble solid in water. Effectof other solutes on the solubility of a substance. Effect of temperature on solubility of a solid
Lesson 9: Solubility and acidity. Solubility and complexation. Fractional precipitation
 
V.- Oxidation-reduction balances
Lesson 10: Degree of oxidation. Definitions Electrochemical batteries Agreements. Measure of the f.e. of a pile Equation of Nernst
Lesson 11: Electrode potential. Normal potential Reduction potential at 25oC. Factors that influence the potential of electrode: acidity of the medium, precipitation of some of the redox pair species. Applications PH measurement Glass and reference electrodes
 
 
Practical sessions
 
Practice 1. Balances. Volumetric material
Theory: Measures of mass. Volumetric measures. Units of concentration. Disputes. Density
Laboratory: Weighing technique. Determination of the density of standard solutions. Calculation of the concentration of a solution of sodium chloride from the determination of its density.
 
Practice 2. Determination of the degree of acidity of a commercial vinegar
Theory: Acid-base volume.
Laboratory: Evaluation of the degree of acidity of a commercial vinegar.
 
Practice 3. Measure the pH. Relative strength of acids and bases
Theory: Acids and bases. PH scale PH-meter.
Laboratory: Relative strength of acids and bases. Hydrolysis of salts. Shock absorbers and non-shock absorbers.
 
Practice 4. Simple extraction
Theory: Concept of simple extraction. Theoretical foundation. Extraction equipment Emulsions
Laboratory: Separation of a mixture of benzoic acid, 1,3-dinitrobenzene and aniline. Extraction with a basic aqueous and acid phase.
 
Practice 5. Separation and purification of solids
Theory: The burner Bunsen. Filtration by gravity and suction.
Laboratory: Separation of the components of a mixture. Filtration and sublimation. Identification of compounds

Methodology


Although the teacher will use the master class to transmit knowledge of the nuclear aspects of each subject, the student must be an active part of the learning process (interactive master class). In this sense, initiatives on inquiry, motivation and the process of knowledge of things will be promoted, having the student to create them and adapt them to their own learning process. The students will carry out laboratory practices with the aim of completing and reinforcing the knowledge acquired in the theoretical classes and seminars. The teacher will carry out orientation, guidance and reinforcement tasks of those aspects that present more difficulty. There will be plenty of bibliographical material available to students, including theoretical contents and also exercises. To encourage critical reasoning, discussion and reflection on the part of the student, work groups will be enabled in the problem classes and in the seminars in order to complete the learning process through group discussion.

Activities

Title Hours ECTS Learning Outcomes
Type: Directed      
Laboratory sessions 20 0.8
Master classes 22 0.88
Problem classes 11 0.44
Seminars 5 0.2
Type: Supervised      
Tutorials scheduled 7 0.28
Type: Autonomous      
Self study 76.5 3.06

Assessment

The assessment will be individual and will be carried out continuously in the different training activities that have been programmed.

Individual written tests: Two partial exams will be done that will include the contents covered in the different lessons, whose weight will be 75% of the final grade.
At the end of the course, it will be possible to perform a recovery test for all students with the subject not passed and have the practices with a mark higher than 5.0. Laboratory reports: 5 practical sessions are programmed. The practices will be done in pairs. At the end of each practice you will have to complete a report (by partner) that will be delivered before the end of each session (45 minute time to complete the report).
The note of each report will be the mark obtained for each member of the pair of students. All practical sessions are mandatory. An unrealized practice (and not justified by the professor's criteria) will be an automatic suspense of the subject.
The professor responsible for the subject will evaluate the cases of faults justified by the student. The note obtained in each practice report will be supplemented by a note from the laboratory's book and attitude.
The total weight of the final mark of practices will be 20% on the final mark of the subject. Delivery of exercises and works: Throughout the course the student will have to deliver exercises that will be proposed by the teacher. There will be exercises that will have to be done in class, and others will have to do the self-study of the student.
In no case will the days scheduled for the exercises be scheduled and there will be no prior notice. All exercises will be mandatory and the weight will be 3% on the final grade. Attitude in the formative activities: Active participation, face-to-faceassistance, as well asthe attitude in the different training activities such as master classes, problems, seminars and practical sessions of laboratory, will have a subjective assessment by the teacher and will have a weight of 2% on the final grade.

It will be considered NOT EVALUABLE as a final grade when any of these cases are met:
- Missing all laboratory practice sessions
- Do not perform individual written tests (partial) and do not do the FINAL exam

To pass the subject, it is necessary to obtain a score equal to or greater than 5.0 on 10 in the FINAL NOTE while satisfying the following conditions:
- Have laboratory practices with a average grade equal to or greater than 5.0 out of 10
- Be attended to all the sessions of laboratory practices (2 theoretical + 5 practices). If there is any lack of assistance, it must be duly justified.
- Have a mark equal to or greater than 4.5 out of 10 in the average mark of the individual written tests (partial).

Right to the recovery exam:
- In the event of not approving the subject with all the requirements mentioned above, the student will be entitled to a RECOVERY EXAMINATION OF ALL THE MATTER.
To pass the subject and do the weighted average of this recovery test with other evaluable activities, it is mandatory to remove a RECEIPT EXAMINATION NOTE equal to or greater than 5.0, but in this case, only the weighted average will be made
with one value of NOTA RECOVERY EXAM equal to 5.0.
- Once the weighted average of all the activities evaluated has been done, to pass the subject, the FINAL NOTE (eg recovery) will have to be ≥ 5.0.  

FINAL NOTE (for partial) = PARTIAL NOTE (≥ 4.5) * 0.75 + PRACTICAL NOTE (≥ 5) * 0.20+ (EXERCISES+ ATTITUDE) * 0.05

FINALNOTE (ex. recovery) = NOTE RECOVERY EXAM (all subject)(5.0 if the NOTE RECOVERY EXAM ≥ 5.0) * 0.75 + PRACTICAL NOTE (≥5) * 0.20 + (EXERCISES + ATTITUDE) * 0, 05

If the PARTIAL NOTE is <4,5 and / or the NOTE RECOVERY EXAM is <5.0, the academic record will be a note of 4.5 (suspended), if the FINAL NOTE is equal to or greater than 5.0 .

COVI-19: Any suspended student who has a laboratory practice grade higher than 6.5 out of 10 in the 2019-2020 course, may keep this note (only if it is not possible to do the practices in person) for the 2020-2021 course and It will not be compulsory to do the laboratory practices again.
If it is possible to carry out the laboratory practices in person, the laboratory sessions will be compulsory obtaining a new evaluation note.


Assessment Activities

Title Weighting Hours ECTS Learning Outcomes
Completion of work and problem solving. Attitude 5% 2 0.08 9, 7, 8, 3, 2, 5
Realization two partial tests 75% 4.5 0.18 9, 7, 8, 4, 5
Realization of laboratory reports 20% 2 0.08 1, 3, 2, 5, 6, 10

Bibliography

J.A. LÓPEZ CANCIO. Problemas de Química. Cuestiones y ejercicios. Prentice Hall, 2000

SALES; VILARRASA. Introducció a la nomenclatura química. Inorgànica i Orgànica. 5 ed. Reverté SA, 2003

QUIÑOÁ; RIGUERA. Nomenclatura y formulació de los compuestos inorgánicos. McGraw Hill, 1997

ATKINS; JONES. Principios de Química. Los caminos del descubrimiento. 3ª ed. Editorial Medica panamericana, 2006

HARRIS. Anàlisi Química Quantitativa (traducció al català de la 6ena edició en españyol). Reverté SA, 2006

MAHAN; MYERS. Química. Curso universitario. 4ª ed. Addison-Wesley Iberoamericana; 1990

CHANG. Química. McGraw Hill, 2010, 10ª ed.

SILVA; BARBOSA. Equilibrios iónicos y sus aplicaciones analíticas. Síntesis, 2002

PETRUCCI, HARWOOD, HERRING. Química General. 8a ed. Prentice Hall, 2007

 

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