In a galvanic cell, a spontaneous redox reaction occurs. However the reactants a

Question

In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can also write the equivalent equation in terms of the reduction potentials, and avoid manipulating standard potentials: E^o cell = E^o red (cathode) - -E^o red (anode) A table of standard reduction potentials gives E^o red values for common half-reactions. Calculate the standard potential for the following galvanic cell: Zn(s) | Zn2 * (aq) 11 Cu2 ' (aq) | Cu(s) which has the overall balanced equation: Calculate the standard potential following galvanic cell: Zn(s) |Zn^2+ (aq)|| Cu^2+ (aq) |Cu(s) Which has the overall balanced equation: Zn(s) + Cu^2+ (aq) right arrow Zn^2+ (aq) + Cu(s) In the context of the zinc-copper cell described in Part A, match each of the following descriptions to the anode or c Drag the appropriate items to their respective bins. r~

Explanation / Answer

E0cell = E0cathode - E0anode

      = 0.34-(-0.76)

      = 1.1 V

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