A) \[Z{{n}^{2+}}+Cu\xrightarrow{{}}Zn+C{{u}^{2+}}\]
B) \[C{{u}^{2+}}+Zn\xrightarrow{{}}Cu+Z{{n}^{2+}}\]
C) \[Z{{n}^{2+}}+C{{u}^{2+}}\xrightarrow{{}}Zn+Cu\]
D) None of the above
Correct Answer: B
Solution :
Key Idea Electrode potential of cell must be positive for spontaneous reaction. \[Z{{n}^{2+}}\xrightarrow{{}}Zn;\,\,{{E}^{o}}=-0.76\,V\] \[C{{u}^{2+}}\xrightarrow{{}}Cu;\,\,{{E}^{o}}=-0.34\,V\] Redox reaction is \[\begin{align} & \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,Zn\xrightarrow{{}}Z{{n}^{2+}}+2{{e}^{-}}\,\,(oxidation) \\ & \underline{\overline{C{{u}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Cu\,\,\,\,\,\,\,}}\,\,\,\,\,\,\,\,\,\,\,(reduction) \\ & \,\,\,\,\,\,\,\,\,{{E}_{cell}}=E_{cathode}^{o}-E_{anode}^{o} \\ \end{align}\] \[=-0.34-(-0.76)\] \[=+\,0.42\,V\] \[{{E}_{cell}}\]is positive, so above reaction is feasible.
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