6.2 Exercises

Unit 6 Electrochemistry

OpenStax

For each reaction listed, determine whether the reaction is spontaneous at standard conditions.
(a) [latex]\text{Mg}(s)\;+\;\text{Ni}^{2+}(aq)\;{\longrightarrow}\;\text{Mg}^{2+}(aq)\;+\;\text{Ni}(s)[/latex]

(b) [latex]2\text{Ag}^{+}(aq)\;+\;\text{Cu}(s)\;{\longrightarrow}\;\text{Cu}^{2+}(aq)\;+\;2\text{Ag}(s)[/latex]

(c) [latex]\text{Mn}(s)\;+\;\text{Sn(NO}_3)_2(aq)\;{\longrightarrow}\;\text{Mn(NO}_3)_2(aq)\;+\;\text{Sn}(s)[/latex]

(d) [latex]3\text{Fe(NO}_3)_2(aq)\;+\;\text{Au(NO}_3)_3(aq)\;{\longrightarrow}\;3\text{Fe(NO}_3)_3(aq)\;+\;\text{Au}(s)[/latex]
When a solution of 1 M Cu²⁺ is mixed with a solution of 1 M Au³⁺, Cu(s), and Au(s), what spontaneous reaction will happen?
Determine the overall reaction for the reaction in which cadmium metal is oxidized to 1 M cadmium(II) ion and aluminum ions in a 1 M aluminum nitrate solution are reduced to aluminum. Is the reaction spontaneous at standard conditions?

(a) spontaneous; (b) spontaneous; (c) spontaneous; (d) spontaneous
[latex]3\text{Cu}(s)\;+\;2\text{Au}^{3+}(aq)\;{\longrightarrow}\;3\text{Cu}^{2+}(aq)\;+\;2\text{Au}(s)[/latex]
[latex]3\text{Cd}(s)\;+\;2\text{Al}^{3+}(aq)\;{\longrightarrow}\;3\text{Cd}^{2+}(aq)\;+\;2\text{Al}(s)[/latex]; nonspontaneous

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