Lecture notes for Monday Dec 3 2007 CHEM135 Johnson

Lecture notes for Monday Dec 3 2007 CHEM135 Johnson -...

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Lecture notes for Monday, Dec. 3 for Exam V Dr. Johnson CHEM135 Electrochemistry We have discussed the following redox reaction before in lecture. Refer to figure in book. Cu (s) + 2 Ag + (aq) Cu 2+ (aq) + Ag (s) If we separate the half reactions into two separate beakers, we can construct a galvanic cell (also called a voltaic cell) Electrons produced Electrons consumed Oxidation Reduction Build up of cations Build up of anions As ions are build up in beaker the reaction stops. Therefore a “salt bridge” is constructed to allow ions to pass between the two solutions to keep the solutions ioncially neutral. anion flow cation flow Anode Cathode electron flow Salt Bridge Cu (s) Cu 2+ (aq) + 2e - Ag + (aq) + 1 e - Ag (s) Cu Ag Cu 2+ Ag + E o oxid. = E o reduct. =
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Shorthand notation for the cell: Cu (s) / Cu 2+ (aq, 1M)// Ag + (aq, 1 M)/ Ag (s) Anode always written first (left side) Electrodes on either end (if no solid use Pt as an inert electrode) “/” denotes a phase boundary; “//” denotes a salt bridge Satandard conditions for a standard cell is 1 M for a solution and 1 atm pressure for a gas. a galvanic cell (also called a voltaic cell) is characterized by a spontaneous redox reaction see examples in OWL standard reduction potential (E
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Lecture notes for Monday Dec 3 2007 CHEM135 Johnson -...

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