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NEET Chemistry Electrochemistry / विद्युत् रसायन Question Bank Self Evaluation Test - Electrochemistry

  • question_answer
    Given that: \[E{{{}^\circ }_{A{{g}^{+}}/Ag}}~=0.80V\] and \[[A{{g}^{+}}]={{10}^{-3}}M;\] \[E{{{}^\circ }_{Hg_{2}^{2+}/Hg}}=0.785V\] and \[[Hg_{2}^{2+}]={{10}^{-1}}M\] which is true for the cell reaction \[2Hg(l)+2A{{g}^{+}}(aq)\to 2Ag(s)+Hg_{2}^{2+}(aq)?\]

    A) The forward reaction is spontaneous

    B) The backward reaction is spontaneous

    C) \[{{E}_{cell}}=0.163\,\nu \]

    D) \[{{E}_{cell}}=1.585\,\nu \]

    Correct Answer: B

    Solution :

    [b] \[{{E}_{cell}}=E_{cell}^{{}^\circ }-\frac{0.0592}{2}\log \frac{[Hg_{2}^{2+}(aq)]}{{{[A{{g}^{+}}(aq)]}^{2}}}\] \[=(0.80-0.785)-\frac{0.0592}{2}log\frac{{{10}^{-1}}}{{{({{10}^{-3}})}^{2}}}=-0.133V\] hence backward reaction is spontaneous.


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