In the electrolysis of CuSO4 solution, 6.35 g of copper was deposited in a coulometer. If the same amount of electricity is passed through silver nitrate solution, the mass of Ag deposited at cathode is - Sri Chaitanya Infinity Learn Best Online Courses for NCERT Solutions, CBSE, ICSE, JEE, NEET, Olympiad and Class 6 to 12

A
$1.08 g$
B
$21.6 g$
C
$108.0$
D
$162 g$

Solution:

The reaction is ${Cu}^{2 +} (aq) + 2 e^{-} \to Cu (s)$ , i.e. $1 mol$ of $Cu$ is deposited by 2mol of electrons. For the deposition of $6.35 g Cu (= 0.1 mol Cu), 0.2 mol$ of electrons will be needed. The deposition of $Ag (s)$ involves the reaction . ${Ag}^{+} (aq) + e^{-} \to Ag (s)$ Thus, for $0.2 mol$ of electrons, $0.2 mol$ of $Ag$ will be deposited which is $0.2 X 108 g$ i.e. $21.6 g$

In the electrolysis of ${CuSO}_{4}$ solution, $6.35 g$ of copper was deposited in a coulometer. If the same amount of electricity is passed through silver nitrate solution, the mass of $Ag$ deposited at cathode is

Solution:

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