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Chapter 17: Q17.3 CYL (page 926)
Use cell notation to describe the galvanic cell where copper(II) ions are reduced to copper metal and zinc metal is oxidized to zinc ions.
The cell notation is \({\mathop{\rm Zn}\nolimits} (s)\left| {{\rm{Z}}{{\rm{n}}^{2 + }}(aq) | |{\rm{C}}{{\rm{u}}^{2 + }}(aq)} \right|{\rm{Cu}}(s).\)
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Given the following pairs of balanced half-reactions, determine the balanced reaction for each pair of half reactions in an acidic solution.
(a) \({\bf{Ca}} \to {\bf{C}}{{\bf{a}}^{{\bf{2 + }}}}{\bf{ + 2}}{{\bf{e}}^{\bf{ - }}}{\bf{,}}\quad {{\bf{F}}_{\bf{2}}}{\bf{ + 2}}{{\bf{e}}^{\bf{ - }}} \to {\bf{2\;}}{{\bf{F}}^{\bf{ - }}}\)
(b) \({\bf{Li}} \to {\bf{L}}{{\bf{i}}^{\bf{ + }}}{\bf{ + }}{{\bf{e}}^{\bf{ - }}}{\bf{,}}\quad {\bf{C}}{{\bf{l}}_{\bf{2}}}{\bf{ + 2}}{{\bf{e}}^{\bf{ - }}} \to {\bf{2C}}{{\bf{l}}^{\bf{ - }}}\)
(c) \({\bf{Fe}} \to {\bf{F}}{{\bf{e}}^{{\bf{3 + }}}}{\bf{ + 3}}{{\bf{e}}^{\bf{ - }}}{\bf{,}}\quad {\bf{B}}{{\bf{r}}_{\bf{2}}}{\bf{ + 2}}{{\bf{e}}^{\bf{ - }}} \to {\bf{2B}}{{\bf{r}}^{\bf{ - }}}\)
(d) \({\bf{Ag}} \to {\bf{A}}{{\bf{g}}^{\bf{ + }}}{\bf{ + }}{{\bf{e}}^{\bf{ - }}}{\bf{,}}\quad {\bf{MnO}}_{\bf{4}}^{\bf{ - }}{\bf{ + 4}}{{\bf{H}}^{\bf{ + }}}{\bf{ + 3}}{{\bf{e}}^{\bf{ - }}} \to {\bf{Mn}}{{\bf{O}}_{\bf{2}}}{\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\)
Consider the following metals: Ag, Au, \(Mg, Ni,\)\(and\)\(Zn\). Which of these metals could be used as a sacrificial anode in the cathodic protection of an underground steel storage tank? Steel is mostly iron, so use \( - 0.447\;{\rm{V}}\) as the standard reduction potential for steel.
For each reaction listed, determine its standard cell potential at 25oC and whether the reaction is spontaneous at standard conditions.
(a) \({\rm{Mg}}(s) + {\rm{N}}{{\rm{i}}^{2 + }}(aq) \to {\rm{M}}{{\rm{g}}^{2 + }}(aq) + {\rm{Ni}}(s)\)
(b) \(2{\rm{A}}{{\rm{g}}^ + }(aq) + {\rm{Cu}}(s) \to {\rm{C}}{{\rm{u}}^{2 + }}(aq) + 2{\rm{Ag}}(s)\)
(c) \({\rm{Mn}}(s) + {\rm{Sn}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) \to {\mathop{\rm Mn}\nolimits} {\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\mathop{\rm Sn}\nolimits} (s)\)
(d) \(3{\rm{Fe}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Au}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_3}(aq) \to 3{\rm{Fe}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_3}(aq) + {\rm{Au}}(s)\)
A current of \({\bf{2}}.{\bf{345}}{\rm{ }}{\bf{A}}\)passes through the cell shown in the Figure \({\bf{17}}.{\bf{20}}\) for \({\bf{45}}\) minutes. What is the volume of the hydrogen collected at room temperature if the pressure is exactly \({\bf{1}}\) atm? Assume the voltage is sufficient to perform the reduction. (Hint: Is hydrogen the only gas present above the water?)
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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