This preview shows pages 1–2. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: Determination of Equilibrium Constant Group Participants: Jason Christian , Thomas Cassidy, Brendan Mitchelson, and Samir Kashyap Section Number: 528, Group #8 Meeting Time: 12:30-5:20 March 16, 2007 TA: Brian Roehm Introduction An equilibrium constant, K, is the ratio of products to reactants in a reaction. It corresponds to the extent that a reaction has advanced in one direction or the other. An equilibrium constant is just that, a constant. It changes only with varying temperature. According to Le Chatelier’s Principle, when a system at equilibrium has a change in concentration of either reactants or products, the solution will shift back towards equilibrium. The equilibrium of the system before the change was induced will be the same as the equilibrium concentration calculated after the change in concentration. Another important concept involving equilibrium constants is Beer-Lambert’s law (Beer’s law). The general form of Beer’s law is: A= a x b x c where A is the absorbance, a is the molar absorptivity specific to each element, b is the path length, and c is the concentration of the solution. Fe 3+ (aq) + SCN- (aq) FeSCN 2+ (aq) In this week’s lab, a solution of two colorless solutions, Fe 3+ and SCN- , were added together to create a colored solution. Using a derivation of Beer’s law, the K c of FeSCN 2+ was found using the above chemical equation and following linear equation derivated...
View Full Document
This note was uploaded on 04/07/2008 for the course CHEM 185 taught by Professor Berrie during the Spring '08 term at Kansas.
- Spring '08