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. \[Z{{n}^{2+}}\xrightarrow{{}}Zn\,;\] \[{{E}^{o}}=-0.75\,\,V\] \[C{{u}^{2+}}\xrightarrow{{}}Cu\,;\] \[{{E}^{o}}=-0.34\,\,V\] Redox reaction is \[Zn\xrightarrow{{}}Z{{n}^{2}}+2{{e}^{-}}\] (oxidation) \[\begin{align} & \underline{C{{u}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Cu} \\ & \underline{Zn+C{{u}^{2+}}\xrightarrow{{}}Z{{n}^{2+}}+Cu} \\ \end{align}\] (reduction) \[{{E}_{cell}}=E_{cathode}^{o}-E_{anode}^{o}\] \[=-0.34-(-0.76)\] \[=+0.42\,\,V\] \[{{E}_{cell}}\] is positive, so above reaction is feasible.
You need to login to perform this action.
You will be redirected in
3 sec
