Question

Standard reduction potentials (E°red) are defined for reduction half-reactions. For a voltaic cell, E°red for the cathode (reduction) must be more positive than E°red for the anode (oxidation). Consider the following two metals and their standard reduction potentials. Co2+(aq) + 2e- -> Co(s) E°red = -0.28 V Ag+(aq) + e- -> Ag(s) E°red = 0.80 V If half-cells for these two metals were combined in a voltaic cell, what reaction would take place at the anode? What reaction would take place at the cathode? Ans: Calculate the cell potential for the overall (spontaneous) reaction under standard conditions. Ans: Write the balanced chemical equation for the overall reaction. Ans: The activity of a metal is defined as its ease of oxidation (an active metal is one that is easily oxidized). Based on their standard reduction potentials, which is the more active metal, cobalt or silver? Ans:

          Standard reduction potentials (E°red) are defined for reduction half-reactions. For a voltaic cell, E°red for the cathode (reduction) must be more positive than E°red for the anode (oxidation). Consider the following two metals and their standard reduction potentials.

Co2+(aq) + 2e- -> Co(s) E°red = -0.28 V
Ag+(aq) + e- -> Ag(s) E°red = 0.80 V

If half-cells for these two metals were combined in a voltaic cell, what reaction would take place at the anode? What reaction would take place at the cathode?

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Calculate the cell potential for the overall (spontaneous) reaction under standard conditions.

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Write the balanced chemical equation for the overall reaction.

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The activity of a metal is defined as its ease of oxidation (an active metal is one that is easily oxidized). Based on their standard reduction potentials, which is the more active metal, cobalt or silver?

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Added by Ian B.

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