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Physical Chemistry I

Informacje ogólne

Kod przedmiotu: 310-ERS-CHF1E
Kod Erasmus / ISCED: (brak danych) / (brak danych)
Nazwa przedmiotu: Physical Chemistry I
Jednostka: Wydział Chemii
Grupy: erazmus 2024
Program ERASMUS - Chemia
Punkty ECTS i inne: 7.00 Podstawowe informacje o zasadach przyporządkowania punktów ECTS:
  • roczny wymiar godzinowy nakładu pracy studenta konieczny do osiągnięcia zakładanych efektów uczenia się dla danego etapu studiów wynosi 1500-1800 h, co odpowiada 60 ECTS;
  • tygodniowy wymiar godzinowy nakładu pracy studenta wynosi 45 h;
  • 1 punkt ECTS odpowiada 25-30 godzinom pracy studenta potrzebnej do osiągnięcia zakładanych efektów uczenia się;
  • tygodniowy nakład pracy studenta konieczny do osiągnięcia zakładanych efektów uczenia się pozwala uzyskać 1,5 ECTS;
  • nakład pracy potrzebny do zaliczenia przedmiotu, któremu przypisano 3 ECTS, stanowi 10% semestralnego obciążenia studenta.
zobacz reguły punktacji
Język prowadzenia: angielski
Rodzaj przedmiotu:

obowiązkowe
Skrócony opis:

The lecture includes content related to basic definitions and rights thermodynamics, physical states, phase equilibria, and the structure and interaction of molecules. The laboratory consists of 8 exercises performed by students. The seminar includes content related to thermodynamics and thermochemistry, states of aggregation and phase equilibria.
Pełny opis:

LECTURE:

1. Subject and meaning of thermodynamics. The first law of thermodynami,cs. Internal energy of the system. Status functions. Isobaric, isochoric, adiabatic processes. Enthalpy. Reversible and irreversible processes. Hess's law. Calorimetry. Dependence of heat of reaction on temperature. The second law of thermodynamics. Entropy. Thermodynamic potentials. Activity, activity coefficient.

2. Gas condition. Equation of perfect gas state. Ideal gas equation.

3. Liquid state. Liquid structure. Liquid viscosity. Theories of viscosity. Viscosity measurements. Surface energy.

4. Solid state, characteristics. Molar heat of solids. Born-Haber cycle.

5. Gibbs phase rule, Raoult's law. Henry's law. Azeotropes. Ebulliometry. Cryometry. Ternary systems. Gibbs triangle.

6. Refractometry. Construction, principle of operation and use of a refractometer. Refractive index. Refraction.

7. Polarimetry. Torsion of the polarization plane. Obtaining and properties of polarized light. Optically active substances.

8. A chemical bond. Ionic, atomic bond. Polar bond polarization. Intermolecular bonds. Van der Waals interactions. Hydrogen bond.

9. Spectrophotometry. Lambert law, Beer law. Lambert-Beer law. Deviations from Lambert-Beer law.

SEMINAR:

1. Thermodynamics and thermochemistry

2. States of matter aggregation

3. Phase equilibria

LABORATORY:

1. Determination of molar heat of neutralization of a strong acid with a strong base.

2. Incompleted miscibility liquids. Solubility isotherm for ternary system.

3. Liquid state characteristic. Study of viscosity.

4. Liquid - gas equilibrium. Determination of the isobar boiling point of two mutually soluble liquids. Azeotrops.

5. Determination of the molar refraction and study its additive properties

6. Polarimetry - identification and determination of optically active compounds concentration

7. Determination of the dissociation constant of a weak acid using a spectrophotometric method.

8. Nernst’s distribution law.

Complementary classes

Final classes
Literatura:

1. Atkins P. Physical Chemistry Oxford University Press 2017

2. Atkins P., De Paula J. Elements of Physical Chemistry. Oxford University Press 2016

3. Smith B.E. Basic Chemical Thermodynamics, Imperial College Press 2013

4. Hofmann A. Physical Chemistry, Essentials Springer International Publishing AG 2018

and materials provided by the teatcher.
Efekty uczenia się:

1. Student defines the basic concepts of physical chemistry, thermodynamics, phase equilibria and describes how they are related to other fields of science K_W08

2. Selects the appropriate IT tools for the statistical evaluation of the experiment results, calculations and preparation of the presentation K_W11

3. Explains the basics of the construction and principles of operation of measuring equipment K_W12

4. Interprets the results of the conducted experiments, critically evaluates the results, estimates measurement errors, prepares reports K_U04

5. Is responsible for the safety of their own work and that of others K_K05

6. Interested in basic processes related to physical chemistry and their role in everyday life K_K02

7. Learns selected issues independently K_U08
Metody i kryteria oceniania:

In order to pass the laboratory, student must complete all laboratory exercices, pass the reports on the exercises perfomed and obtain a positive grade from the written tests. Exam from the lecture.

Zajęcia w cyklu "Rok akademicki 2024/25" (zakończony)

Okres: 2024-10-01 - 2025-06-30
Wybrany podział planu:
Przejdź do planu
Typ zajęć:
Konwersatorium, 30 godzin więcej informacji
Laboratorium, 45 godzin więcej informacji
Wykład, 45 godzin więcej informacji
Koordynatorzy: Diana Bobrowska, Joanna Breczko, Urszula Klekotka
Prowadzący grup: Anna Basa, Diana Bobrowska, Joanna Breczko, Urszula Klekotka, Joanna Kotyńska
Lista studentów: (nie masz dostępu)
Zaliczenie: Przedmiot - Egzamin
Konwersatorium - Zaliczenie na ocenę
Laboratorium - Zaliczenie na ocenę
Rodzaj przedmiotu:

obowiązkowe
Tryb prowadzenia przedmiotu:

w sali
Skrócony opis:

The lecture includes content related to basic definitions and rights thermodynamics, physical states, phase equilibria, and the structure and interaction of molecules. The laboratory consists of 8 exercises performed by students. The seminar includes content related to thermodynamics and thermochemistry, states of aggregation and phase equilibria.
Pełny opis:

LECTURE:

1. Subject and meaning of thermodynamics. The first law of thermodynami,cs. Internal energy of the system. Status functions. Isobaric, isochoric, adiabatic processes. Enthalpy. Reversible and irreversible processes. Hess's law. Calorimetry. Dependence of heat of reaction on temperature. The second law of thermodynamics. Entropy. Thermodynamic potentials. Activity, activity coefficient.

2. Gas condition. Equation of perfect gas state. Ideal gas equation.

3. Liquid state. Liquid structure. Liquid viscosity. Theories of viscosity. Viscosity measurements. Surface energy.

4. Solid state, characteristics. Molar heat of solids. Born-Haber cycle.

5. Gibbs phase rule, Raoult's law. Henry's law. Azeotropes. Ebulliometry. Cryometry. Ternary systems. Gibbs triangle.

6. Refractometry. Construction, principle of operation and use of a refractometer. Refractive index. Refraction.

7. Polarimetry. Torsion of the polarization plane. Obtaining and properties of polarized light. Optically active substances.

8. A chemical bond. Ionic, atomic bond. Polar bond polarization. Intermolecular bonds. Van der Waals interactions. Hydrogen bond.

9. Spectrophotometry. Lambert law, Beer law. Lambert-Beer law. Deviations from Lambert-Beer law.

SEMINAR:

1. Thermodynamics and thermochemistry

2. States of matter aggregation

3. Phase equilibria

LABORATORY:

1. Determination of molar heat of neutralization of a strong acid with a strong base.

2. Incompleted miscibility liquids. Solubility isotherm for ternary system.

3. Liquid state characteristic. Study of viscosity.

4. Liquid - gas equilibrium. Determination of the isobar boiling point of two mutually soluble liquids. Azeotrops.

5. Determination of the molar refraction and study its additive properties

6. Polarimetry - identification and determination of optically active compounds concentration

7. Determination of the dissociation constant of a weak acid using a spectrophotometric method.

8. Nernst’s distribution law.

Complementary classes

Final classes
Literatura:

1. Atkins P. Physical Chemistry Oxford University Press 2017

2. Atkins P., De Paula J. Elements of Physical Chemistry. Oxford University Press 2016

3. Smith B.E. Basic Chemical Thermodynamics, Imperial College Press 2013

4. Hofmann A. Physical Chemistry, Essentials Springer International Publishing AG 2018

and materials provided by the teatcher.

Zajęcia w cyklu "Rok akademicki 2025/26" (jeszcze nie rozpoczęty)

Okres: 2025-10-01 - 2026-06-30
Wybrany podział planu:
Przejdź do planu
Typ zajęć:
Konwersatorium, 30 godzin więcej informacji
Laboratorium, 45 godzin więcej informacji
Wykład, 45 godzin więcej informacji
Koordynatorzy: Joanna Kotyńska
Prowadzący grup: (brak danych)
Lista studentów: (nie masz dostępu)
Zaliczenie: Przedmiot - Egzamin
Konwersatorium - Zaliczenie na ocenę
Laboratorium - Zaliczenie na ocenę
Rodzaj przedmiotu:

obowiązkowe
Tryb prowadzenia przedmiotu:

w sali
Skrócony opis:

The lecture includes content related to basic definitions and rights thermodynamics, physical states, phase equilibria, and the structure and interaction of molecules. The laboratory consists of 8 exercises performed by students. The seminar includes content related to thermodynamics and thermochemistry, states of aggregation and phase equilibria.
Pełny opis:

LECTURE:

1. Subject and meaning of thermodynamics. The first law of thermodynami,cs. Internal energy of the system. Status functions. Isobaric, isochoric, adiabatic processes. Enthalpy. Reversible and irreversible processes. Hess's law. Calorimetry. Dependence of heat of reaction on temperature. The second law of thermodynamics. Entropy. Thermodynamic potentials. Activity, activity coefficient.

2. Gas condition. Equation of perfect gas state. Ideal gas equation.

3. Liquid state. Liquid structure. Liquid viscosity. Theories of viscosity. Viscosity measurements. Surface energy.

4. Solid state, characteristics. Molar heat of solids. Born-Haber cycle.

5. Gibbs phase rule, Raoult's law. Henry's law. Azeotropes. Ebulliometry. Cryometry. Ternary systems. Gibbs triangle.

6. Refractometry. Construction, principle of operation and use of a refractometer. Refractive index. Refraction.

7. Polarimetry. Torsion of the polarization plane. Obtaining and properties of polarized light. Optically active substances.

8. A chemical bond. Ionic, atomic bond. Polar bond polarization. Intermolecular bonds. Van der Waals interactions. Hydrogen bond.

9. Spectrophotometry. Lambert law, Beer law. Lambert-Beer law. Deviations from Lambert-Beer law.

SEMINAR:

1. Thermodynamics and thermochemistry

2. States of matter aggregation

3. Phase equilibria

LABORATORY:

1. Determination of molar heat of neutralization of a strong acid with a strong base.

2. Incompleted miscibility liquids. Solubility isotherm for ternary system.

3. Liquid state characteristic. Study of viscosity.

4. Liquid - gas equilibrium. Determination of the isobar boiling point of two mutually soluble liquids. Azeotrops.

5. Determination of the molar refraction and study its additive properties

6. Polarimetry - identification and determination of optically active compounds concentration

7. Determination of the dissociation constant of a weak acid using a spectrophotometric method.

8. Nernst’s distribution law.

Complementary classes

Final classes
Literatura:

1. Atkins P. Physical Chemistry Oxford University Press 2017

2. Atkins P., De Paula J. Elements of Physical Chemistry. Oxford University Press 2016

3. Smith B.E. Basic Chemical Thermodynamics, Imperial College Press 2013

4. Hofmann A. Physical Chemistry, Essentials Springer International Publishing AG 2018

and materials provided by the teatcher.
Opisy przedmiotów w USOS i USOSweb są chronione prawem autorskim.
Właścicielem praw autorskich jest Uniwersytet w Białymstoku.
ul. Świerkowa 20B, 15-328 Białystok tel: +48 85 745 70 00 (Centrala) https://uwb.edu.pl kontakt deklaracja dostępności mapa serwisu USOSweb 7.1.2.0-8 (2025-07-09)