Anode cathode reaction cu fe12/23/2023 As electrons flow from left to right through the electrode and wire, nitrate ions (anions) pass through the porous plug on the left into the copper(II) nitrate solution. The salt bridge consists of a concentrated, nonreactive, electrolyte solution such as the sodium nitrate (NaNO 3) solution used in this example. The circuit is closed using a salt bridge, which transmits the current with moving ions. At this point, no current flows-that is, no significant movement of electrons through the wire occurs because the circuit is open. The half-cell on the right side of the figure consists of the silver electrode in a 1 M solution of silver nitrate (AgNO 3). The silver is undergoing reduction the silver electrode is referred to as the cathode. The anode is connected to a voltmeter with a wire and the other terminal of the voltmeter is connected to a silver electrode by a wire. The copper is undergoing oxidation the copper electrode is referred to as the anode. The beaker on the left side of the figure is called a half-cell, and contains a 1 M solution of copper(II) nitrate with a piece of copper metal partially submerged in the solution. Galvanic or voltaic cells involve spontaneous electrochemical reactions in which the half-reactions are separated ( Figure 17.4) so that current can flow through an external wire. (credit: modification of work by Mark Ott) As the reaction proceeds (b), the solution turns blue (c) because of the copper ions present, and silver metal is deposited on the copper strip as the silver ions are removed from solution. Figure 17.3 When a clean piece of copper metal is placed into a clear solution of silver nitrate (a), an oxidation-reduction reaction occurs that results in the exchange of Cu 2+ for Ag + ions in solution.
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