Silver is the metal electrode in a molar solution of Ag+ ions in a standard cell with a reference electrode.
(a) What reactions occur at the two electrodes?
(b) What voltage is developed in the cell? (c) What is the Gibbs free energy change per silver ion involved in the reaction?
(a) Since the Ag reduction reaction is more electropositive than hydrogen reduction reaction, the Ag will not be oxidized or go into solution. Thus, Ag deposits on the Ag electrode according to the reaction Ag+ + 1e– ? Ag, and at the reference electrode the reaction is H2 ? 2H+ + 2e– or hydrogen ions are produced from hydrogen gas.
(b) The voltage developed is the voltage for the reduction reaction of Ag+ + 1e– ? Ag or+ 0.800 V.
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