Chapter 17: Q17.2E (page 957)
For the scenario in the previous question, how many electrons moved through the circuit.
Number of electrons is \({\rm{3}}{\rm{.28 \times 1}}{{\rm{0}}^{{\rm{22}}}}\)
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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 \({\bf{B}}{{\bf{r}}_{\bf{2}}}{\bf{(aq)}}\).
Why do batteries go dead, but fuel cells do not?
Suppose you have three different metals, \({\rm{A}}\), \(B\), and \({\rm{C}}\). When metals \({\rm{A}}\) and \(B\) come into contact, \(B\) corrodes and \({\rm{A}}\)do not corrode. When metals \({\rm{A}}\)and \({\rm{C}}\) come into contact, \({\rm{A}}\) corrodes and \({\rm{C}}\) do not corrode. Based on this information, which metal corrodes and which metal does not corrode when \(B\) and \({\rm{C}}\) come into contact?
An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
Use the data in Appendix \({\rm{L}}\) to determine the equilibrium constant for the following reactions. Assume 298.15\({\rm{K}}\) if no temperature is given.
(a) \({\bf{AgCl(s)}}\rightleftharpoons {\bf{A}}{{\bf{g}}^{\bf{ + }}}{\bf{(aq) + C}}{{\bf{l}}^{\bf{ - }}}{\bf{(aq)}}\)
(b) \({\bf{CdS(s)}}\rightleftharpoons {\bf{C}}{{\bf{d}}^{{\bf{2 + }}}}{\bf{(aq) + }}{{\bf{S}}^{{\bf{2 - }}}}{\bf{(aq)}}\) at \({\bf{377\;K}}\)
(c) \({\bf{H}}{{\bf{g}}^{{\bf{2 + }}}}{\bf{(aq) + 4B}}{{\bf{r}}^{\bf{ - }}}{\bf{(aq)}}\rightleftharpoons {\left[ {{\bf{HgB}}{{\bf{r}}_{\bf{4}}}} \right]^{{\bf{2 - }}}}{\bf{(aq)}}\)
(d) \({{\bf{H}}_{\bf{2}}}{\bf{O(l)}}\rightleftharpoons {{\bf{H}}^{\bf{ + }}}{\bf{(aq) + O}}{{\bf{H}}^{\bf{ - }}}{\bf{(aq)}}\) at \({\bf{2}}{{\bf{5}}^{\bf{^\circ }}}{\bf{C}}\)
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