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JEE Main & Advanced AIEEE Solved Paper-2003

  • question_answer
    For the redox reaction, \[Zn(s)+C{{u}^{2+}}(0.1M)\xrightarrow{{}}Z{{n}^{2+}}(1M)+Cu(s)\]taking place in a cell, \[E_{cell}^{o}\] is \[1.10\] volt. \[{{E}_{cell}}\] for the cell will be \[\left( 2.303\frac{RT}{F}=0.0591 \right)\]     AIEEE  Solved  Paper-2003

    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 V


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