PPT-Determining An Equilibrium Constant

Using Spectrophotometry and Beers Law Objectives 1 To determine the equilibrium constant for the reaction of iron III and thiocyanate to form the thiocyanatoironIII complex ion using spectrophotometric data. 2.1 Chemical Equilibrium (and Equilibrium Constant). 2.2 Calculations using Kc expressions. 2.3 Effect of changing conditions on equilibria. Chemical Equilibrium. Describe the term chemical equilibrium.. 15.3. Using Equilibrium Constants in Calculations. Bill Vining. SUNY Oneonta. Equilibrium and the Equilibrium Constant. In . this section…. Determining an equilibrium constant. Determining if a system is at equilibrium. Author: Wesley Tung. Technical Things. A chemical equation of a reaction uses mole ratios to describe the production of products from reactants.. In . , hydrogen and oxygen are reactants, and water is a product.. 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. To do list week 1. Read the syllabus. If desired download . powerpoint. slides. . Register for . MasteringChemistry. Complete extra credit chapter 16 pre- assignment . Complete intro to mastering assignment . Measuring Equilibrium Concentrations. Equilibrium Calculations (ICE Charts). Qualitatively Interpreting the Equilibrium Constant. Meaning of Small Equilibrium Constant. SCH4U – Grade 12 Chemistry, University Preparation. Equilibrium. When a reaction is at a state of equilibrium, the rate of the forward reaction __________ the rate of the reverse reaction.. is equal to. is slower than. is faster than. is the reverse of. Honors . Chemistrry. Enloe. High School. Chemical Equilibrium. Condition which the concentrations of all reactants and products in a closed system cease to change with time. Occurs when opposing reactions are proceeding at equal rates. Lecture Presentation. Chapter 14. Chemical Equilibrium. Hemoglobin. Hemoglobin is a protein (Hb), found in red blood cells, that reacts with O. 2. . . It enhances the amount of O. 2. that can be carried through the bloodstream.. James F. Kirby. Quinnipiac University. Hamden, CT. Lecture Presentation. The Concept of Equilibrium. . Chemical equilibrium. occurs when a reaction and its reverse reaction proceed at the same rate. In the figure above, equilibrium is finally reached in the third picture.. The State of Chemical Equilibrium. Chemical Equilibrium. : The state reached when the concentrations of reactants and products remain constant over time.. 2 NO. 2. (. g. ). N. 2. O. 4. (. g. ). Brown. . 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 . The Meaning of K. . K > 1 . . the equilibrium position is far to the right . K < 1 . . the equilibrium position is far to the left . The value of . K. for a system can be calculated from a known set of equilibrium concentrations. . Chemical System: . A system is described in terms of empirical properties such as . temperature, pressure, volume and amount of substance present.. By definition, all chemical systems are fast, quantitative, stoichiometric and spontaneous! However, this assumption is NOT always true..