Using a table of standard reduction potentials, determine the best answer to the following...
Question:
Using a table of standard reduction potentials, determine the best answer to the following questions.
a. Which of the following reagents would oxidize Zn to Zn{eq}^{2+} {/eq}, but not Sn to Sn{eq}^{2+} {/eq}?
A. Ca{eq}^{2+} {/eq}
B. Ca
C. Co
D. Br{eq}_2 {/eq}
E. Br{eq}^- {/eq}
F. Co{eq}^{2+} {/eq}
b. Which of the following reagents would oxidize Ag to Ag{eq}^+ {/eq}, but not Au to Au{eq}^{3+} {/eq}?
A. Ca{eq}^{2+} {/eq}
B. Ca
C. Co
D. Br{eq}_2 {/eq}
E. Br{eq}^- {/eq}
F. Co{eq}^{2+} {/eq}
Standard Cell Potential:
The standard cell potential is the potential difference between the cathode half-cell and the anode half-cell at standard conditions. The cathode half-cell is where reduction occurs, this is the half-reaction that involves gain of electrons. The anode half-cell is where oxidation occurs, this is the half-reaction that involves loss of electrons. The standard cell potential is obtained by adding the standard reduction potential of the cathode and the standard oxidation potential of the anode.
Answer and Explanation: 1
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For a reaction to occur, the sum of the {eq}E^{\circ}_{anode} {/eq} (for oxidation half-reaction) and {eq}E^{\circ}_{cathode} {/eq} (for reduction...
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