PPT-Lecture 5 Electron and Hole concentration at equilibrium

1 Recap In last lecture temperature effect on extrinsic semiconductor was discussed Both d onar and acceptor ionization shows Freeze out region at low temperature A t moderate temperature all . Principles of Chemical Reactivity: . Equilibria. All chemical reactions are reversible, at least in principle.. The concept of equilibrium is fundamental to chemistry. . The general concept of equilibrium was introduced in Chapter 3 to explain the limited dissociation of weak acids.. Equilibria. (. Ch. 19). Suggested HW (. Ch. 19): 4, 10, 14, 18, 26, 36, 46, 52 . Equilibrium. Recap: Gibbs Free Energy and the Criteria for Spontaneity. In the last lecture, we were introduced to Gibbs free energy (. A . reversible reaction . can be approached from either direction. In a . closed system. , no reactants or products can enter or escape. For equilibrium to be achieved, a reaction must be . reversible. Measuring Equilibrium Concentrations. Equilibrium Calculations (ICE Charts). Qualitatively Interpreting the Equilibrium Constant. Meaning of Small Equilibrium Constant. SCH4U – Grade 12 Chemistry, University Preparation. LW3 . Lecture Week . 3-2 (02042016) . Chapter 2 Notes . P-n and n-p junction Review: Forward and Reverse biasing. Energy Band Diagrams. Avalanche and . Zener. Breakdown. Circuit models; Junction and Diffusion Capacitance. Fabio . Landini. . Università . Bocconi. Ugo . Pagano. Università . di Siena and . Central European . University. Second. International . GROE Workshop. Institutions. and . Economic. . Change. Announcements I. Diagnostic Quiz. Should be receiving back in lab. Learn what material to review. SacCT. – will be set up once adding is done. Bring a periodic table to class (I will provide on . on. The Haber process proceeds as follows:. . 2NH. 3 (g). + 92KJ ↔ N. 2 (g). + 3H. 2 (g) . . If the equilibrium concentrations are:. [NH. 3. ] = 3.1x10. -2. M. [N. 2. ] = 8.5x10. -1. M. [H. 2. x and FeSe e MS resulting from longitudinal and transverse transport under a wide range of magnetic eld B up to 50 T shows a physically reasonable and intrinsic interpretation on the electronic states Law of chemical equilibrium. For an equilibrium. a A + b B c C + d D. K = . [C]. c. [D]. d. [A]. a. [B]. b. K is the equilibrium constant for that reaction.. The [ ] mean concentration in molarity. Using Spectrophotometry . and Beer’s Law. Objectives:. . 1.) To determine the . equilibrium constant. for the reaction of iron (III) and thiocyanate to form the thiocyanatoiron(III) complex ion using spectrophotometric data.. . When the rates of the forward and reverse reactions become equal, the concentrations of the reactants and the products remain constant. This is the stage of chemical equilibrium. This equilibrium is . Read Chapter 13 look at the problems. Do . the AP practice test on page AP-13 A-D. (it is in between numbered pages 547-548). 2. AP Test. Historically, the first question on the free response has ALWAYS been an equilibrium question.. indistinguishability of the electrons. ,. electron wave nature. ,. the Pauli exclusion principle. .. (4.6). The function . f. (E). called . the . Fermi-Dirac distribution function. gives the probability that an available energy .