(C) The reduction reactions at the cathodes are:$Al^{3+} + 3e^- \to Al$ (requires $3 \ mol$ of electrons for $1 \ mol$ of $Al$)$Cu^{2+} + 2e^- \to Cu$

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$1 \ mol : 1.5 \ mol : 3 \ mol$

(C) The reduction reactions at the cathodes are:$Al^{3+} + 3e^- \to Al$ (requires $3 \ mol$ of electrons for $1 \ mol$ of $Al$)$Cu^{2+} + 2e^- \to Cu$ (requires $2 \ mol$ of electrons for $1 \ mol$ of $Cu$)$Na^+ + e^- \to Na$ (requires $1 \ mol$ of electrons for $1 \ mol$ of $Na$)Given $3 \ F$ ($3 \ mol$ of electrons) are passed through each cell:Moles of $Al$ deposited $= \frac{3 \ F}{3 \ F/mol} = 1 \ mol$Moles of $Cu$ deposited $= \frac{3 \ F}{2 \ F/mol} = 1.5 \ mol$Moles of $Na$ deposited $= \frac{3 \ F}{1 \ F/mol} = 3 \ mol$Therefore,the ratio is $1 \ mol : 1.5 \ mol : 3 \ mol$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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Three faradays of electricity are passed through molten $Al_2O_3$,aqueous solution of $CuSO_4$ and molten $NaCl$ taken in different electrolytic cells. The amount of $Al$,$Cu$ and $Na$ deposited at the cathodes will be in the ratio of

A
$1 \ mol : 2 \ mol : 3 \ mol$
B
$3 \ mol : 2 \ mol : 1 \ mol$
C
$1 \ mol : 1.5 \ mol : 3 \ mol$
D
$1.5 \ mol : 2 \ mol : 3 \ mol$

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Electrochemistry

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Faraday’s law of electrolysis

How many grams of chlorine gas will be produced as a product when a current of $2 \ A$ is passed through a concentrated aqueous solution of $NaCl$ for $30 \ \text{minutes}$?

Medium

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Aqueous $CuSO_4$ solution was electrolysed by passing $2 \ A$ of current for $10 \ min$. What is the weight (in $g$) of copper deposited at the cathode? (Given: $Cu = 63 \ u$; $F = 96500 \ C \ mol^{-1}$)

MediumAP EAMCET 2024

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Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

MediumJEE MAIN 2021

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Equal amounts of electricity are passed through two separate electrolytic cells containing nickel nitrate $[Ni(NO_3)_2]$ and chromium nitrate $[Cr(NO_3)_3]$. If $0.3 \ g$ of nickel is deposited in the first cell,how much chromium will be deposited in the second cell? (Atomic mass of $Ni = 59$,Atomic mass of $Cr = 52$)

Easy

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An acidic solution of dichromate is electrolyzed for $8 \ min$ using $2 \ A$ current. As per the following equation: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. The amount of $Cr^{3+}$ obtained was $0.104 \ g$. The efficiency of the process (in $\%$) is (Take: $F = 96000 \ C$,At. mass of chromium $= 52$)

MediumJEE MAIN 2020

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Three faradays of electricity are passed through molten $Al_2O_3$,aqueous solution of $CuSO_4$ and molten $NaCl$ taken in different electrolytic cells. The amount of $Al$,$Cu$ and $Na$ deposited at the cathodes will be in the ratio of

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How many grams of chlorine gas will be produced as a product when a current of $2 \ A$ is passed through a concentrated aqueous solution of $NaCl$ for $30 \ \text{minutes}$?

Aqueous $CuSO_4$ solution was electrolysed by passing $2 \ A$ of current for $10 \ min$. What is the weight (in $g$) of copper deposited at the cathode? (Given: $Cu = 63 \ u$; $F = 96500 \ C \ mol^{-1}$)

Consider the following reaction:$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

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Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .