(A) The charge of $1$ mole of electrons is defined as $1$ Faraday $(F)$. $1 \ F = N_A \times e^-$,where $N_A$ is Avogadro's number $(6.022 \times

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$1 \ F, 96500 \ C, 6.022 \times 10^{23} \ \text{electrons}$

(A) The charge of $1$ mole of electrons is defined as $1$ Faraday $(F)$. $1 \ F = N_A \times e^-$,where $N_A$ is Avogadro's number $(6.022 \times 10^{23} \ \text{mol}^{-1})$ and $e^-$ is the charge of a single electron $(1.602 \times 10^{-19} \ C)$. Therefore,$1 \ F = 6.022 \times 10^{23} \times 1.602 \times 10^{-19} \ C \approx 96500 \ C$. Thus,$1$ mole of electrons equals $1 \ F$,$96500 \ C$,and $6.022 \times 10^{23}$ electrons.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?

A
$1 \ F, 96500 \ C, 6.022 \times 10^{23} \ \text{electrons}$
B
$1 \ F, 9650 \ C, 6.022 \times 10^{23} \ \text{electrons}$
C
$0.5 \ F, 96500 \ C, 3.011 \times 10^{23} \ \text{electrons}$
D
$1 \ F, 96500 \ C, 1.602 \times 10^{-19} \ \text{electrons}$

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Faraday’s law of electrolysis

Calculate the time required in seconds to deposit $6.35 \ g$ of copper from its salt solution by passing a $5 \ A$ current. [Molar mass of $Cu = 63.5 \ g \ mol^{-1}$]

MediumMHT CET 2023

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$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?

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The amount of copper metal deposited at the cathode on passing an electric current of $500 \, mA$ for $20 \, minutes$ in a cupric chloride solution is ............ $g$.

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To deposit a silver layer of thickness $5 \times 10^{-3} \ cm$ on a surface area of $80 \ cm^2$ (density $= 10.5 \ g \ cm^{-3}$),a current of $3 \ A$ is passed through a silver nitrate solution for ......... $sec$.

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The anodic half-cell of a lead-acid battery is recharged using electricity of $0.05 \ F$. The amount of $PbSO_4$ electrolyzed in $g$ during the process is (Molar mass of $PbSO_4 = 303 \ g \ mol^{-1}$)

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$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?

Similar Questions

Calculate the time required in seconds to deposit $6.35 \ g$ of copper from its salt solution by passing a $5 \ A$ current. [Molar mass of $Cu = 63.5 \ g \ mol^{-1}$]

$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?

The amount of copper metal deposited at the cathode on passing an electric current of $500 \, mA$ for $20 \, minutes$ in a cupric chloride solution is ............ $g$.

To deposit a silver layer of thickness $5 \times 10^{-3} \ cm$ on a surface area of $80 \ cm^2$ (density $= 10.5 \ g \ cm^{-3}$),a current of $3 \ A$ is passed through a silver nitrate solution for ......... $sec$.

The anodic half-cell of a lead-acid battery is recharged using electricity of $0.05 \ F$. The amount of $PbSO_4$ electrolyzed in $g$ during the process is (Molar mass of $PbSO_4 = 303 \ g \ mol^{-1}$)

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