Lecture29 - Chem 162, Lecture 29, Spring 2011 Interplay of...

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Interplay of chemical energy ( G) electrical energy (E) Chemical reactions electricity Reduction-oxidation (redox) reactions. Imagine a piece of copper being added to a solution of silver nitrate A redox (reduction-oxidation) reaction will occur. Cu(s) + 2Ag + (aq) 2Ag(s) + Cu 2+ (aq) The change in oxidation numbers tells us it is a redox reaction. Cu(s) gets oxidized (gives off electrons)—it is the reducing agent Ag + (aq) gets reduced (gains electrons)—it is the oxidizing agent We can separate the overall reaction into two half reactions Half reactions: Oxidation: Cu(s) Cu 2+ (aq) + 2e - Reduction: Ag + (aq) + e - Ag(s) Adding these two half-reactions up, first multiplying the reduction reaction by 2 to cancel electrons, we get the overall reaction: Cu(s) + 2Ag + (aq) 2Ag(s) + Cu 2+ (aq) A spontaneous oxidation-reduction reaction such as shown above can be designed as a galvanic, also called voltaic, cell – a way to generate a flow of electrons or electricity. Such a galvanic cell is commonly called a battery. 1
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This note was uploaded on 11/09/2011 for the course CHEM 162 taught by Professor Siegal during the Spring '08 term at Rutgers.

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Lecture29 - Chem 162, Lecture 29, Spring 2011 Interplay of...

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