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_rad + 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_rod. 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. Part B In the context of the zinc-copper cell described in Part A, match each of the following descriptions to the anode or cathode. Drag the appropriate items to their respective bins.

Answer 1

Analyzing a Galvanic Cell Correct 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: Part B In the context of the zinc-copper cell described in Part A, match each of the following descriptions to the anode or cathode Drag the appropriate items to their respective bins. By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which Ex has the opposite sign of Ered You can also write the equivalent equation in terms of the reduction potentials, and avoid manipulating standard potentials gains mass loses mass attracts electrons E cell E red (cathode) - E ed(anode) positive electrode negative electrode stronger reducing agent A table of standard reduction potentials gives E red values for common half-reactions Reduction half-reaction E V) Ag+ (aq) + e →Ag(s) | 080 Cu2 (aq) +2eCus0.3 Ni2 (aq) +2e-Ni(s)-0.26 Fe2 (aq) +2e Fe(s) -0.45 Zn2+ (aq) + 2e →Zn(s) | -0.76 Anode Cathode Zn loses mass negative electrode stronger reducing agent pOsitive electrode gain mas:s attracts electrons Please see the answer