A) \[2.14\] V
B) \[1.80\] V
C) \[1.07\] V
D) \[0.82\] V
Correct Answer: C
Solution :
(i) Find the value of equilibrium constant for the given redox reaction. (ii) Calculate the \[{{E}_{cell}}\] of the reaction by Nernst equation. \[{{E}_{cell}}=E_{cell}^{o}-\frac{0.0591}{n}\log Q\] \[\underset{0.1\,M}{\mathop{C{{u}^{2+}}}}\,+Zn\xrightarrow{{}}Z\underset{1M}{\mathop{{{n}^{2+}}}}\,+Cu\] \[Q=\frac{[Z{{n}^{2+}}]}{[C{{u}^{2+}}]}=\frac{1}{0.1}=10\] \[{{E}_{cell}}=1.10-\frac{0.0591}{2}\log \,\]10 = 1.10-0.0295 = 1.0705 VYou need to login to perform this action.
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