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 :
In the spontaneous reactions, the electrode potential of cell becomes positive. \[Z{{n}^{2+}}\xrightarrow[{}]{{}}Zn,\] \[E{}^\circ =-0.76V\] \[C{{u}^{2+}}\xrightarrow[{}]{{}}Cu,\] \[E{}^\circ =-0.34V\] In the redox reaction \[Zn\xrightarrow[{}]{{}}Z{{n}^{2+}}+2{{e}^{-}}\] (oxidation) \[C{{u}^{2+}}+2{{e}^{-}}\xrightarrow[{}]{{}}Cu\] (reduction) \[\overline{Zn+C{{u}^{2+}}\xrightarrow[{}]{{}}Z{{n}^{2+}}+Cu}\] \[{{E}_{cell}}=E_{cathode}^{o}-E_{anode}^{o}\] \[=-0.34-(-0.76)\] \[=+0.42V\]
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