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

  • question_answer
    How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper \[=63.5u,{{N}_{A}}\] = Avogadro's constant):

    A) \[\frac{{{N}_{A}}}{20}\]                                  

    B) \[\frac{{{N}_{A}}}{10}\]

    C) \[\frac{{{N}_{A}}}{5}\]                       

    D) \[\frac{{{N}_{A}}}{2}\]

    Correct Answer: C

    Solution :

    [c] \[Cu\xrightarrow{{}}C{{u}^{++}}+2{{e}^{-}}\] i.e, to deposit 1 mole of Cu at cathode from \[C{{u}^{2+}}SO{{_{4}^{2-}}^{~}}\]solution = 2 moles of electrons are required i.e. To deposit \[6.35g=\frac{6.35}{63.5}\times 2=\frac{2}{10}=\frac{1}{5}moles\] Thus total no. of electrons required \[=\frac{{{N}_{A}}}{5}\]


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