Chapter 17: Q17.5CYL (page 935)
What is the standard free energy change and the equilibrium constant for the following reaction at room temperature? Is the reaction spontaneous?
The standard free energy change value is negative thus the reaction is spontaneous
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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 \({\bf{2}}{{\bf{5}}^{\bf{^\circ }}}{\bf{C}}\)
Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agentin each of the reactions of the previous problem.
(a) \({\bf{S}}{{\bf{O}}_{\bf{3}}}^{{\bf{2 - }}}{\bf{(aq) + Cu(OH}}{{\bf{)}}_{\bf{2}}}{\bf{(s)}} \to {\bf{S}}{{\bf{O}}_{\bf{4}}}^{{\bf{2 - }}}{\bf{(aq) + Cu(OH)(s)}}\)
(b) \({{\bf{O}}_{\bf{2}}}{\bf{(g) + Mn(OH}}{{\bf{)}}_{\bf{2}}}{\bf{(s)}} \to {\bf{Mn}}{{\bf{O}}_{\bf{2}}}{\bf{(s)}}\)
(c) \({\bf{N}}{{\bf{O}}_{\bf{3}}}^{\bf{ - }}{\bf{(aq) + }}{{\bf{H}}_{\bf{2}}}{\bf{(g)}} \to {\bf{NO(g)}}\)
(d) \({\bf{Al(s) + Cr}}{{\bf{O}}_{\bf{4}}}^{{\bf{2 - }}}{\bf{(aq)}} \to {\bf{Al(OH}}{{\bf{)}}_{\bf{3}}}{\bf{(s) + Cr(OH}}{{\bf{)}}_{\bf{4}}}^{\bf{ - }}{\bf{(aq)}}\)
Determine the overall reaction and its standard cell potential at \({25\circ }{\rm{C}}\) for these reactions. Is the reaction spontaneous at standard conditions? Assume the standard reduction for \({\rm{B}}{{\rm{r}}_2}(l)\) is the same as for \({\rm{B}}{{\rm{r}}_2}(aq)\).
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?
For each of the following balanced half-reactions, determine whether an oxidation or reduction is occurring.
(a) \({\bf{C}}{{\bf{l}}^{\bf{ - }}}{\bf{ + 3}}{{\bf{e}}^{\bf{ - }}} \to {\bf{C}}{{\bf{l}}_{\bf{2}}}\)
(b) \({\bf{M}}{{\bf{n}}^{{\bf{2 + }}}} \to {\bf{Mn}}{{\bf{O}}_{\bf{2}}}\)
(c) \({{\bf{H}}_{\bf{2}}} \to {{\bf{H}}^{\bf{ + }}}\)
(d) \({\bf{NO}}_{\bf{3}}^{\bf{ - }} \to {\bf{NO}}\)
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