# CW23-Eo1 - If so do not double the E° electrode(e Note...

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CHM 2046/Myers Class Worksheet 23 March 15, 2010 1. Observing E°cell for several Voltaic Cells (on the reverse side) 2. Setting up a Table of Electrode (Half Cell) Potentials. Electrode Reduction Half Reaction 3. Uses of the E° Table: (a)Predict if a redox reaction will go spontaneously. Reaction occurs for a Strong OA and a Strong RA, or Upper Left – Lower Right . (b) Find the E°cell. This is the difference (the gap) between the E° electrodes ’s. (c) Find the signs of the electrodes. Look at the order of the E°s in the table. (d) A source of balanced half reactions ! Note that you reverse the bottom half reaction, that of the Strong RA. To balance the e’s, you may need to double a half-rxn.
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Unformatted text preview: If so, do not double the E° electrode . (e) Note some handy formulas at the bottom. 4. Effect of Concentration on Ecell. Nernst Equation: Ecell = E°cell - n V 0592 . log 10 Q where Q = ] ts tan ac [Re ] oducts [Pr “Ecell” means for any conc., “E ° cell” means “at standard conc.” as 1 M (aq), 1 atm (g), pure (l) & (s). Example: For the cell with reaction as 2 Ag + + Cu 2 Ag + Cu +2 , find the actual cell potential (Ecell) if [Ag + ] = 0.015 M and [Cu +2 ] = 0.20 M. Do these concentrations make the reaction more or less spontaneous than it would be if both were 1M?...
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## This note was uploaded on 09/20/2011 for the course CHM 2051 taught by Professor Staff during the Spring '08 term at University of Florida.

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