Lecture 32 - 3/31/10 5.3.B. Spontaneous Redox reactions...

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3/31/10 1 5.3.B. Spontaneous Redox reactions rxn as written is non-spontaneous Non-standard conditions: consider E cell 15 cell = E o C - E o A = E o reduction + E o oxidation rxn as written is spontaneous cell > 0 : cell < 0 : cell is spontaneous in reverse direction C > E° A Both written as reduction potentials 16 e.g. Show that the following reaction is spontaneous under standard conditions and 298 K: Cu (s) + 2 Ag + (aq) ! Cu 2+ (aq) + 2 Ag (s) Method 1 : Write reactions as reductions & get E° from table Ag + (aq) + e - ! Ag (s) cell is positive, therefore cell reaction is spontaneous = 0.800 ! 0.340 = 0.460 V Cu 2+ (aq) + 2 e - ! Cu (s) Anode: Cathode: E cell o = E C o ! E A o = E Ag + /Ag o ! E Cu 2 + /Cu o E° = 0.340 V E° = 0.800 V Cu(s) ! Cu 2+ (aq) + 2 e - Where oxidation occurs Write as reduction 17 Look at each half-reaction separately (no balancing) Don’t need to flip reactions Don’t need to change signs of E° Don’t need to multiply E° by an integer
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This note was uploaded on 04/22/2010 for the course CHEM 102 taught by Professor Brown during the Winter '10 term at University of Alabama at Birmingham.

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Lecture 32 - 3/31/10 5.3.B. Spontaneous Redox reactions...

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