(A) The reduction reactions are as follows: $Mg^{2+} + 2e^- \rightarrow Mg$ To produce $1 \ mole$ of $Mg$,$2 \ moles$ of electrons are required. Charg

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(A) The reduction reactions are as follows: $Mg^{2+} + 2e^- \rightarrow Mg$ To produce $1 \ mole$ of $Mg$,$2 \ moles$ of electrons are required. Charge required $= 2 \times 96500 \ C = 193000 \ C$. $Al^{3+} + 3e^- \rightarrow Al$ To produce $1 \ mole$ of $Al$,$3 \ moles$ of electrons are required. Charge required $= 3 \times 96500 \ C = 289500 \ C$. Therefore,the required charges are $193000 \ C$ and $289500 \ C$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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To gain $1 \ mole$ $Mg$ from $Mg^{2+}$ and $1 \ mole$ $Al$ from $Al^{3+}$,how many Coulombs of electricity are required respectively?

A
$193000 \ C$ and $289500 \ C$
B
$96500 \ C$ and $193000 \ C$
C
$289500 \ C$ and $193000 \ C$
D
$193000 \ C$ and $96500 \ C$

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Class 12

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Electrochemistry

Subtopic

Faraday’s law of electrolysis

Match the following and select the correct option for the quantity of electricity,in $C \ mol^{-1}$,required to deposit various metals at the cathode:

List-$I$ List-$II$

$a. \ Ag^{+}$ $i. \ 386000 \ C \ mol^{-1}$

$b. \ Mg^{2+}$ $ii. \ 289500 \ C \ mol^{-1}$

$c. \ Al^{3+}$ $iii. \ 96500 \ C \ mol^{-1}$

$d. \ Ti^{4+}$ $iv. \ 193000 \ C \ mol^{-1}$

List-$I$	List-$II$
$a. \ Ag^{+}$	$i. \ 386000 \ C \ mol^{-1}$
$b. \ Mg^{2+}$	$ii. \ 289500 \ C \ mol^{-1}$
$c. \ Al^{3+}$	$iii. \ 96500 \ C \ mol^{-1}$
$d. \ Ti^{4+}$	$iv. \ 193000 \ C \ mol^{-1}$

MediumKCET 2025

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Total charge on $1 \, \text{mole}$ of a monovalent metal ion is equal to

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If $96500 \ C$ of electricity liberates one gram equivalent of any substance,the time taken for a current of $0.15 \ A$ to deposit $20 \ mg$ of copper from a solution of copper sulphate is (Chemical equivalent of copper = $32$).

Easy

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The relation between Faraday constant $(F)$,chemical equivalent $(E)$,and electrochemical equivalent $(Z)$ is

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$96.5$ amperes current is passed through the molten $AlCl_3$ for $100$ seconds. The mass of aluminium deposited at the cathode is (atomic weight of $Al = 27$ $u$). (in $g$)

EasyAP EAMCET 2022

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To gain $1 \ mole$ $Mg$ from $Mg^{2+}$ and $1 \ mole$ $Al$ from $Al^{3+}$,how many Coulombs of electricity are required respectively?

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