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Chapter 17: Q20E (page 959)
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.
The active electrode that gains mass is the part of cathode.
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For each reaction listed, determine its standard cell potential at \({25\circ }{\rm{C}}\) and whether the reaction is spontaneous at standard conditions.
(a)\({\mathop{\rm Mn}\nolimits} (s) + {\rm{N}}{{\rm{i}}^{2 + }}(aq) \to {{\mathop{\rm Mn}\nolimits} ^{2 + }}(aq) + {\rm{Ni}}(s)\)
(b)\(3{\rm{C}}{{\rm{u}}^{2 + }}(aq) + 2{\rm{Al}}(s) \to 2{\rm{A}}{{\rm{l}}^{3 + }}(aq) + 3{\rm{Cu}}(s)\)
(c)\({\rm{Na}}(s) + {\rm{LiN}}{{\rm{O}}_3}(aq) \to {\rm{NaN}}{{\rm{O}}_3}(aq) + {\rm{Li}}(s)\)
(d) \({\rm{Ca}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Ba}}(s) \to {\rm{Ba}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Ca}}(s)\)
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) \({\bf{NO}}_{\bf{3}}^{\bf{ - }} \to {\bf{NO}}\)
For the cell notations in the previous problem, write the corresponding balanced reactions. Given the following cell notations, determine the species oxidized, species reduced, and the oxidizing agent and reducing agent, without writing the balanced reactions.
a. \({\rm{Mg}}(s)\left| {{\rm{M}}{{\rm{g}}^{2 + }}(aq)|| {\rm{C}}{{\rm{u}}^{2 + }}(aq)} \right|{\rm{Cu}}(s)\)
b.\({\rm{Ni}}(s)\left| {{\rm{N}}{{\rm{i}}^{2 + }}(aq) || {\rm{A}}{{\rm{g}}^ + }(aq)} \right|{\rm{Ag}}(s)\)
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) \({\bf{NO}}_{\bf{3}}^{\bf{ - }} \to {\bf{NO}}\)
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 \({\bf{B}}{{\bf{r}}_{\bf{2}}}{\bf{(aq)}}\).
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