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Chapter 17: Q39E (page 961)
Why do batteries go dead, but fuel cells do not?
Fuel cells do not go dead because they use chemical energy to produce electrical energy.
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What is the cell potential for the following reaction at room temperature?
\({\bf{Al(s)}}\left| {{\bf{A}}{{\bf{l}}^{{\bf{3 + }}}}{\bf{(aq,0}}{\bf{.15M)}} | | {\bf{C}}{{\bf{u}}^{{\bf{2 + }}}}{\bf{(aq,0}}{\bf{.025M)}}} \right|{\bf{Cu(s)}}\)
What are the values of \(n\) and \(Q\) for the overall reaction? Is the reaction spontaneous under these conditions?
What mass of each product is produced in each of the electrolytic cells of the previous problem if a total charge of \({\bf{3}}.{\bf{33}} \times {\bf{1}}{{\bf{0}}^5}{\rm{ }}{\bf{C}}\) passes through each cell? Assume the voltage is sufficient to perform the reduction
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at \({\bf{298}}{\bf{.15\;K}}\).
(a) \({\bf{Hg(l) + }}{{\bf{S}}^{{\bf{2 - }}}}{\bf{(aq,0}}{\bf{.10M) + 2A}}{{\bf{g}}^{\bf{ + }}}{\bf{(aq,0}}{\bf{.25M)}} \to {\bf{2Ag(s) + HgS(s)}}\)
(b) The galvanic cell is made from a half-cell consisting of an aluminium electrode in 0.015M aluminium nitrate solution and a half-cell consisting of a nickel electrode in \({\bf{0}}{\bf{.25M}}\) nickel(II) nitrate solution.
(c) The cell is made of a half-cell in which \({\bf{1}}{\bf{.0M}}\) aqueous bromide is oxidized to \({\bf{0}}{\bf{.11M}}\) bromine ion and a half-cell in which aluminium ion at \({\bf{0}}{\bf{.023M}}\) is reduced to aluminium metal. Assume the standard reduction potential for \({\bf{B}}{{\bf{r}}_{\bf{2}}}{\bf{(l)}}\) is the same as that of \({\bf{B}}{{\bf{r}}_{\bf{2}}}{\bf{(aq)}}\).
Determine the overall reaction and its standard cell potential at 25 °C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half-cell consisting of an aluminum electrode
in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?
An active (metal) electrode was found to gain mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
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