PPT-Shifting Equilibrium Applications Involving the Equilibrium Constant

The Meaning of K K gt 1 the equilibrium position is far to the right K lt 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 . . cultivation:. . Activity. . data. . &. . Emission. . Factors. . for. . an. . integrated,. . scalable. . system. Moving. . on. . From. . Experimental. . Approaches. . to. . Advancing. Reactions are reversible. A + B C + D ( forward). C + D A + B (reverse). Initially there is only A and B so only the forward reaction is possible. As C and D build up, the reverse reaction speeds up while the forward reaction slows down.. AP . Chem. Mr. Nelson. The Concept of Equilibrium. The term . reversible reaction . is used to describe reactions that can go in either the forward or the reverse direction. Equilibrium. is used to specify that a reversible reaction has reached an . 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 . 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. At equilibrium, the number of. people riding up the lift and the. number of people skiing down . the slope . are constant.. Learning Goal . Calculate the equilibrium constant for a reversible reaction given the concentrations of reactants and products at equilibrium.. Lecture 8. How do deal with individual ions in aqueous solution?. We can’t simply add Na. . to a solution (positive ions would repel each other).. We can add . NaCl. . How do we partition thermodynamic parameters between Na. 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. 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 . 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..