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CHM 3410 Physical Chemistry 1 is a Chemistry course at FIU. 3 elite notetakers have produced 6 study materials for this Chemistry course.
These notes introduce the ideal/perfect gas law, first as several separate laws (Boyle's Law, Charles's Law, etc.), then how they all relate to each other and form the ideal gas equation pV=nRT. Explan
These notes begin to discuss properties of real gases (gases do not obey the ideal gas law perfectly). These deviations can typically be seen at high pressures and low temperatures. This is due to the
These notes begin to cover the concepts of the first law of thermodynamics ("the internal energy of an isolated system is constant"). They talk about the conservation of energy, energy as heat and/or work, a system and its surroundings, energy transfer, internal energy (total energy of a system, expansion work (the work arising from a change in volume) and reversible expansion, and ways to measure
These notes continue to cover the first law of thermodynamics and begin to discuss enthalpy (heat inside of the system) and molar enthalpy, relating enthalpy to internal energy, its variation with temperature, relation between heat capacities, the work of adiabatic change, and heat capacity ratio and adiabats.
These notes talk about thermochemistry, the heat produced or acquired during chemical reactions, and the standard changes in enthalpy that occur during phase transitions (enthalpy of fusion/vaporizatio
These notes discuss state functions and exact differentials. State functions are properties that depend only on the current state of a system and not how it came to be that way. Meanwhile, an exact dif
These problems are used to gauge the understanding of the first two chapters (perfect gas law and first law of thermodynamics). Mostly deals with internal energy (by extension heat and work) and change in enthalpy (of reactions) for various scenarios. There is also change in entropy, which is discussed in the beginning of the third chapter (second law).
These notes primary cover the concept of spontaneous change and how to quantify it. The direction of change is related to the distribution of energy and matter, and spontaneous changes are always accom
These notes begin to cover the Third Law of Thermodynamics ("The entropy of all perfect crystalline substances is zero at T = 0."), which help us understand the properties of matter at very low tempera
Here we bring the First and Second Laws together. First, we discuss the properties of internal energy and how it changes with volume. Then, we talk about the properties of Gibbs energy and how it changes with respect to the entropy of the system, temperature, and pressure. We also introduce a new effective pressure called fugacity.
These notes talk about the physical transformations (solid, liquid, gas) of pure substances. First are the phase diagrams, maps that tell us at which temperature and pressure at which each phase of the
These notes cover the first few sections of simple mixtures. These include a thermodynamic description of mixtures as well as partial molar quantities (partial molar volume/ Gibbs energy). We also div
These notes cover other sections on simple mixtures. They introduce colligative properties, which are properties of solutions that depend upon the concentration of solute molecules or ions, but not upo
Here we begin to describe a systematic way of discussing the physical changes mixtures undergo when they are heated or cooled and when their compositions are changed. We see how to use phase diagrams to judge whether two substances are mutually miscible, whether an equilibrium can exist over a range of conditions, or whether the system must be brought to a definite pressure, temperature, and compos
Here we finish describing a systematic way of discussing the physical changes mixtures undergo when they are heated or cooled and when their compositions are changed. We see how to use phase diagrams t
The questions serve to assess your knowledge of phase diagrams (for pure, binary, and ternary systems as well), phase transitions (their implications), and the properties of mixtures of gases, liquids, and solids (ideal and real).