**À propos de ce cours : **This introductory physical chemistry course examines the connections between molecular properties and the behavior of macroscopic chemical systems.

Université du Minnesota

**À propos de ce cours : **This introductory physical chemistry course examines the connections between molecular properties and the behavior of macroscopic chemical systems.

**Enseigné par :**Dr. Christopher J. Cramer, Distinguished McKnight and University Teaching Professor of Chemistry and Chemical Physics

Engagement | 4-6 hours/week |

Langue | English |

Comment réussir | Réussissez tous les devoirs notés pour terminer le cours. |

Notes des utilisateurs |

Programme de cours

SEMAINE 1

Module 1

This module includes philosophical observations on why it's valuable to have a broadly disseminated appreciation of thermodynamics, as well as some drive-by examples of thermodynamics in action, with the intent being to illustrate up front the practical utility of the science, and to provide students with an idea of precisely what they will indeed be able to do themselves upon completion of the course materials (e.g., predictions of pressure changes, temperature changes, and directions of spontaneous reactions). The other primary goal for this week is to summarize the quantized levels available to atoms and molecules in which energy can be stored. For those who have previously taken a course in elementary quantum mechanics, this will be a review. For others, there will be no requirement to follow precisely how the energy levels are derived--simply learning the final results that derive from quantum mechanics will inform our progress moving forward. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

9 vidéos, 6 lectures

**Vidéo:**Video 1.0 - The Thermite Reaction**Reading:**Meet the Course Instructor**Reading:**Grading Policy**Reading:**Read Me First**Reading:**Syllabus**Reading:**Resources**Reading:**Module One**Vidéo:**Video 1.1 - That Thermite Reaction**Vidéo:**Video 1.2 - Benchmarking Thermoliteracy**Vidéo:**Video 1.3 - Quantization of Energy**Vidéo:**Video 1.4 - The Hydrogen Chloride Cannon**Vidéo:**Video 1.5 - Atomic Energy Levels**Vidéo:**Video 1.6 - Diatomic Molecular Energy Levels**Vidéo:**Video 1.7 - Polyatomic Molecular Energy Levels**Vidéo:**Video 1.8 - Review of Module 1

SEMAINE 2

Module 2

This module begins our acquaintance with gases, and especially the concept of an "equation of state," which expresses a mathematical relationship between the pressure, volume, temperature, and number of particles for a given gas. We will consider the ideal, van der Waals, and virial equations of state, as well as others. The use of equations of state to predict liquid-vapor diagrams for real gases will be discussed, as will the commonality of real gas behaviors when subject to corresponding state conditions. We will finish by examining how interparticle interactions in real gases, which are by definition not present in ideal gases, lead to variations in gas properties and behavior. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

8 vidéos, 1 lecture

**Reading:**Module 2**Vidéo:**Video 2.1 - Ideal Gas Equation of State**Vidéo:**Video 2.2 - Non-ideal Gas Equations of State**Vidéo:**Video 2.3 - Gas-Liquid PV Diagrams**Vidéo:**Video 2.4 - Law of Corresponding States**Vidéo:**Video 2.5 - Virial Equation of State**Vidéo:**Video 2.6 - Molecular Interactions**Vidéo:**Video 2.7 - Other Intermolecular Potentials**Vidéo:**Video 2.8 - Review of Module 2

SEMAINE 3

Module 3

This module delves into the concepts of ensembles and the statistical probabilities associated with the occupation of energy levels. The partition function, which is to thermodynamics what the wave function is to quantum mechanics, is introduced and the manner in which the ensemble partition function can be assembled from atomic or molecular partition functions for ideal gases is described. The components that contribute to molecular ideal-gas partition functions are also described. Given specific partition functions, derivation of ensemble thermodynamic properties, like internal energy and constant volume heat capacity, are presented. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

8 vidéos, 1 lecture

**Reading:**Module 3**Vidéo:**Video 3.1 - Boltzmann Probability**Vidéo:**Video 3.2 - Boltzmann Population**Vidéo:**Video 3.3 - Ideal Gas Internal Energy**Vidéo:**Video 3.4 - Ideal Gas Equation of State Redux**Vidéo:**Video 3.5 - van der Waals Equation of State Redux**Vidéo:**Video 3.6 - The Ensemble Partition Function**Vidéo:**Video 3.7 - The Molecular Partition Function**Vidéo:**Video 3.8 - Review of Module 3

SEMAINE 4

Module 4

This module connects specific molecular properties to associated molecular partition functions. In particular, we will derive partition functions for atomic, diatomic, and polyatomic ideal gases, exploring how their quantized energy levels, which depend on their masses, moments of inertia, vibrational frequencies, and electronic states, affect the partition function's value for given choices of temperature, volume, and number of gas particles. We will examine specific examples in order to see how individual molecular properties influence associated partition functions and, through that influence, thermodynamic properties. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

9 vidéos, 1 lecture

**Reading:**Module 4**Vidéo:**Video 4.1 - Ideal Monatomic Gas: qtrans**Vidéo:**Video 4.2 - Ideal Monatomic Gas: Q**Vidéo:**Video 4.3 - Ideal Monatomic Gas: Properties**Vidéo:**Video 4.4 - Ideal Diatomic Gas: Part 1**Vidéo:**Video 4.5 - Ideal Diatomic Gas: Part 2**Vidéo:**Video 4.6 - Ideal Diatomic Gas: Q**Vidéo:**Video 4.7 - Ideal Polyatomic Gases: Part 1**Vidéo:**Video 4.8 - Ideal Polyatomic Gases: Part 2**Vidéo:**Video 4.9 - Review of Module 4

SEMAINE 5

Module 5

This module is the most extensive in the course, so you may want to set aside a little extra time this week to address all of the material. We will encounter the First Law of Thermodynamics and discuss the nature of internal energy, heat, and work. Especially, we will focus on internal energy as a state function and heat and work as path functions. We will examine how gases can do (or have done on them) pressure-volume (PV) work and how the nature of gas expansion (or compression) affects that work as well as possible heat transfer between the gas and its surroundings. We will examine the molecular level details of pressure that permit its derivation from the partition function. Finally, we will consider another state function, enthalpy, its associated constant pressure heat capacity, and their utilities in the context of making predictions of standard thermochemistries of reaction or phase change. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

11 vidéos, 1 lecture

**Reading:**Module 5**Vidéo:**Video 5.1 - First Law of Thermodynamics**Vidéo:**Video 5.2 - Paths of PV Work**Vidéo:**Video 5.3 - Differentials and State Functions**Vidéo:**Video 5.4 - Characteristic Ideal Gas Expansion Paths**Vidéo:**Video 5.5 - Adiabatic Processes**Vidéo:**Video 5.6 - Microscopic Origin of Pressure**Vidéo:**Video 5.7 - Enthalpy**Vidéo:**Video 5.8 - Heat Capacities**Vidéo:**Video 5.9 - Thermochemistry**Vidéo:**Video 5.10 - Standard Enthalpy**Vidéo:**Video 5.11 - Review of Module 5

SEMAINE 6

Module 6

This module introduces a new state function, entropy, that is in many respects more conceptually challenging than energy. The relationship of entropy to extent of disorder is established, and its governance by the Second Law of Thermodynamics is described. The role of entropy in dictating spontaneity in isolated systems is explored. The statistical underpinnings of entropy are established, including equations relating it to disorder, degeneracy, and probability. We derive the relationship between entropy and the partition function and establish the nature of the constant β in Boltzmann's famous equation for entropy. Finally, we consider the role of entropy in dictating the maximum efficiency that can be achieved by a heat engine based on consideration of the Carnot cycle. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

9 vidéos, 1 lecture

**Reading:**Module 6**Vidéo:**Video 6.1 - Entropy**Vidéo:**Video 6.2 - Entropy as a State Function**Vidéo:**Video 6.3 - Spontaneity and the Second Law**Vidéo:**Video 6.4 - Statistical Entropy**Vidéo:**Video 6.5 - Computing Entropy**Vidéo:**Video 6.6 - Entropy and the Partition Function**Vidéo:**Video 6.7 - Beta and Boltzmann’s Constant**Vidéo:**Video 6.8 - The Carnot Cycle**Vidéo:**Video 6.9 - Review of Module 6

SEMAINE 7

Module 7

This module is relatively light, so if you've fallen a bit behind, you will possibly have the opportunity to catch up again. We examine the concept of the standard entropy made possible by the Third Law of Thermodynamics. The measurement of Third Law entropies from constant pressure heat capacities is explained and is compared for gases to values computed directly from molecular partition functions. The additivity of standard entropies is exploited to compute entropic changes for general chemical changes. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts.

7 vidéos, 1 lecture

**Reading:**Module 7**Vidéo:**Video 7.1 - Entropy and Other Thermodynamic Functions**Vidéo:**Video 7.2 - Third Law of Thermodynamics**Vidéo:**Video 7.3 - Standard Entropy**Vidéo:**Video 7.4 - Entropy from the Partition Function**Vidéo:**Video 7.5 - Third Law Entropies**Vidéo:**Video 7.6 - Additivity of Entropies**Vidéo:**Video 7.7 - Review of Module 7

SEMAINE 8

Module 8

This last module rounds out the course with the introduction of new state functions, namely, the Helmholtz and Gibbs free energies. The relevance of these state functions for predicting the direction of chemical processes in isothermal-isochoric and isothermal-isobaric ensembles, respectively, is derived. With the various state functions in hand, and with their respective definitions and knowledge of their so-called natural independent variables, Maxwell relations between different thermochemical properties are determined and employed to determine thermochemical quantities not readily subject to direct measurement (such as internal energy). Armed with a full thermochemical toolbox, we will explain the behavior of an elastomer (a rubber band, in this instance) as a function of temperature. Homework problems will provide you the opportunity to demonstrate mastery in the application of the above concepts. The final exam will offer you a chance to demonstrate your mastery of the entirety of the course material.

9 vidéos, 1 lecture

**Reading:**Module 8**Vidéo:**Video 8.1 - Helmholtz Free Energy**Vidéo:**Video 8.2 - Gibbs Free Energy**Vidéo:**Video 8.3 - Maxwell Relations from A**Vidéo:**Video 8.4 - Maxwell Relations from G**Vidéo:**Video 8.5 - Rubber Band Thermodynamics**Vidéo:**Video 8.6 - Natural Independent Variables**Vidéo:**Video 8.7 - P and T Dependence of G**Vidéo:**Video 8.8 - Review of Module 8**Vidéo:**Video 8.9 - Credits

SEMAINE 9

Final Exam

This is the final graded exercise (20 questions) for the course. There is no time limit to take the exam.

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Créateurs

Université du Minnesota

The University of Minnesota is among the largest public research universities in the country, offering undergraduate, graduate, and professional students a multitude of opportunities for study and research. Located at the heart of one of the nation’s most vibrant, diverse metropolitan communities, students on the campuses in Minneapolis and St. Paul benefit from extensive partnerships with world-renowned health centers, international corporations, government agencies, and arts, nonprofit, and public service organizations.

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Notation et examens

Note moyenne 4.9 sur 5 sur 141 notes

sk

The course instructor was excellent. Although I finished only 5 modules, I could learn a lot.

RC

This is the best organized course on any platform, MOOC or live-in-classroom. Lectures, reading material, supporting documentation... everything is perfectly well laid out, sequentially, and in good order. Really, a delight taking this course. Even for students whose math skills are rusty, the concepts are ideally presented. Bravo to the instructor and supporting staff!

MR

" Really informative and interesting, the instructor has a great ability to explain the most complex concepts in a clear and simple way "

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GK

great course