Lesson_24 - Cu 2+ Cu 2+ e-A B Anode Lower [Cu 2+ ] Cathode...

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Lesson 24 The Nernst equation The Nernst equation quantifies the dependency of cell voltage on the concentration of chemical species and temperature in a galvanic cell: Q nF RT E E cell cell ln 0 - =
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Lesson 24 A voltaic cell with nonstandard conditions
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Lesson 24 Other forms of the Nernst equation Q nF RT E E cell cell log 3026 . 2 0 - = Q n E E cell cell log 0592 . 0 0 - = Change from ln to log :
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Lesson 24 Example 1 A cell is assembled by placing a silver metal
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Lesson 24 Concentration cells
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Lesson 24 Concentration cells Apply the Nerst equation to a cell which operates with the same half-reactions ( E 0 cell = 0 ) at different concentrations ( Q ≠ 1 ) 0 ln - = Q nF RT E cell pH 0592 . 0 log 0592 . 0 1 log 2 0592 . 0 2 2 × = - = - = x x E cell x H log ] log[ pH - = - = +
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Lesson 24 Concentration cells
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Unformatted text preview: Cu 2+ Cu 2+ e-A B Anode Lower [Cu 2+ ] Cathode Higher [Cu 2+ ] B: Cu + 2 e Cu E = 0.34 V B A cell Cu Cu n E ] [ ] [ log 059 . 2 2 10 + +-= 1 ] [ ] [ ] [ ] [ log 2 2 2 2 10 < < + + + + B A B A cell Cu Cu Cu Cu if E Lesson 24 Example 2 Two hydrogen-hydrogen ion half-cells are connected to make a single galvanic cell. In one of the half-cells the pH is 1.0, but the pH in the other half-cell is not known. The measured voltage delivered by the combination is 0.16 V, and the electrode in the half-cell of known concentration is positive. + o Lesson 24 Suggested readings...
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This note was uploaded on 04/13/2009 for the course CHEMISTRY 102 taught by Professor Soares during the Spring '09 term at Waterloo.

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Lesson_24 - Cu 2+ Cu 2+ e-A B Anode Lower [Cu 2+ ] Cathode...

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