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  4. 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 = 63.5 u, NA = Avogadro's constant) :

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Q. 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 $= 63.5\, u, N_A =$ Avogadro's constant) :

JEE MainJEE Main 2014Electrochemistry

Solution:

$ W =\frac{ E }{96500} \times Q $

$ \Rightarrow 6.35 =\frac{63.5}{2 \times 96500} \times Q $

$ \Rightarrow Q =2 \times 9650$ coulomb

$ \Rightarrow 1 F =$ charge of $1$ mol of $ e ^{-}=96500 $

$ \therefore $ No. of $ e ^{-} =\frac{ N _{ A }}{10} \times 2$

$=\frac{ N _{ A }}{5} $