Chemistry 4615 Examination Study Guide: Fundamentals of Thermodynamics and Ideal Gases - P, Study notes of Physical Chemistry

Download Chemistry 4615 Examination Study Guide: Fundamentals of Thermodynamics and Ideal Gases - P and more Study notes Physical Chemistry in PDF only on Docsity! Study Guide For Examination #1 CHEM 4615 1) General Definitions and Concepts, Fundamental Equations and Expressions. Primary and Secondary SI Units Number of Significant Figures Notion of System, Surrounding, Universe and Process Concept of Open, Closed and Isolated Systems Concept of Homogeneous vs. Heterogeneous (Single Phase vs. Multiple Phase) Systems Concept of Intensive vs. Extensive Properties Concept of Molar Quantity Concept of State Variables, State Functions and Path Functions Introduction to Gibbs Phase Rule for a Closed Homogeneous System Ideal Gas Equation of State (assumptions in the Kinetic Theory of Gases) Zeroth Law of Thermodynamics. Absolute Temperature Scale Concept of Diathermic Boundary and Adiabatic Process Dalton’s Law of Mixtures for Ideal Gases. Isothermal Compression of Gases, Critical Point, Binodal or Coexistence Curve Concept of Potential Energy Curve for Intermolecular Interactions (Attraction, Repulsion) Compression Factor, Virial Series, Boyle’s Temperature Van der Waals Equation of State, Meaning of a and b Assumptions and Goals for the Kinetic Theory of Gases Concept of Collision Frequency, Binary Collisions and Mean Free Path and what they depend on Equipartition Theorem (Concept of Degree of Freedom (total, translation, rotation, vibration)) Concepts of Work, Heat, Energy Sign Notation for Work and Heat First Law of Thermodynamics (differential form and integrated form) Work of Expansion and Compression Differential Form dw = - Pext dV Work of Expansion / Compression Integrated Form depends on whether reversible or not. Heat capacity at constant volume Enthalpy H = U + PV Heat capacity at constant pressure Comparison of ΔH with ΔU 2) Calculation of work, heat, change in internal energy and change in enthalpy for processes on ideal gases that are either isobaric, isochoric or isothermal. Know how to derive these quantities for reversible isothermal expansion/compression processes (P = Pext) and for expansion/compression processes under constant external pressure. Know how to relate initial to final state variables (P, V, T) for each of these processes. Fundamental Equations You NEED to Know: Molar mass (M) = mass (m) / number of moles (n) Density (d) = mass (m) / volume (V) dU = dw + dq (First Law, ALWAYS TRUE) dw = - Pext dV (Expansion, Compression Work, ALWAYS TRUE) dU = CV dT + πT dV (ALWAYS TRUE) dU = CV dT (ALWAYS TRUE for any process on ideal gases or for isochoric processes). H = U + PV (definition of Enthalpy, ALWAYS TRUE) dH = CP dT + μT dP (ALWAYS TRUE) dH = CP dT (ALWAYS TRUE for any process on ideal gases or for isobaric processes). CP - CV = nR (TRUE FOR IDEAL GASES ONLY) CVm = (3/2) R (TRUE FOR MONOATOMIC GASES) Pext = P (TRUE FOR REVERSIBLE PROCESSES + PROCESSES AT CONSTANT P) dq = 0 (TRUE FOR ADIABATIC PROCESSES dU = dqV (TRUE FOR ANY CONSTANT VOLUME (ISOCHORIC) PROCESS dH = dqP (TRUE FOR ANY CONSTANT PRESSURE (ISOBARIC) PROCESS PV = nRT (TRUE FOR IDEAL GASES ONLY) (P + a/Vm2)(Vm - b) = RT (TRUE FOR VAN DER WAALS GASES ONLY) Z = PVm / RT (DEFINITION OF COMPRESSION FACTOR) Z = 1 + B’(T) P + C’(T) P2 + D’(T) P3 + .... (VIRIAL EQUATION OF STATES) Z = 1 + B(T) / Vm + C(T) / Vm2 + D(T) / Vm3 + ....(VIRIAL EQUATION OF STATES) Mathematical Definition of Critical Point = Inflection Point in P vs. V diagram. Mathematical Definition of Boyle’s Temperature: B(Tb) = B’(Tb) = 0 Heat capacity at constant volume and at constant pressure P P V V T HC T UC ⎟ ⎠ ⎞ ⎜ ⎝ ⎛=⎟ ⎠ ⎞ ⎜ ⎝ ⎛= ∂ ∂ ∂ ∂ If F is a state function of two variables X and Y, then: dF = ∂F ∂X ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ Y dX + ∂F ∂Y ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ X dY You also need to know the relationship between km, dm, cm, mm, nm, μm and m. You will be given all constants if needed (R, kb, Navogadro, etc…) as well as conversion factors (Pa to atm to bar to mmHg, for instance). If “calculation” questions are given with regards to Chapter 3 (Kinetic Theory of Gases), you will be given the relevant equations. However, you would need to know what each of the terms in the equation means!!!