(C) The electrolysis reaction is: $MgCl_{2} \longrightarrow Mg^{2+} + 2Cl^{-}$At the cathode: $Mg^{2+} + 2e^{-} \longrightarrow Mg$Since $2 \ F$ $(2 \

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(C) The electrolysis reaction is: $MgCl_{2} \longrightarrow Mg^{2+} + 2Cl^{-}$At the cathode: $Mg^{2+} + 2e^{-} \longrightarrow Mg$Since $2 \ F$ $(2 \times 96500 \ C)$ of charge deposits $1 \ mol$ of $Mg$,$9.65 \ C$ of charge will deposit $Mg = \frac{1 \times 9.65}{2 \times 96500} \ mol = 5 \times 10^{-5} \ mol$.To prepare a Grignard reagent $(R-Mg-X)$,$1 \ mol$ of $Mg$ is required per mole of reagent.Therefore,$5 \times 10^{-5} \ mol$ of $Mg$ will produce $5 \times 10^{-5} \ mol$ of Grignard reagent.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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$9.65 \ C$ of electric current is passed through fused anhydrous magnesium chloride. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of the Grignard reagent obtained is

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A
$5 \times 10^{-4}$
B
$1 \times 10^{-4}$
C
$5 \times 10^{-5}$
D
$1 \times 10^{-5}$

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Electrochemistry

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Faraday’s law of electrolysis

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How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.

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An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.

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$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

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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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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: $Cu = 63 \ u$; $F = 96500 \ C \ mol^{-1}$)

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$9.65 \ C$ of electric current is passed through fused anhydrous magnesium chloride. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of the Grignard reagent obtained is

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How much charge is required for the following reductions:$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.

An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.

$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

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 $PbSO_4 = 303 \ g \ mol^{-1}$)

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: $Cu = 63 \ u$; $F = 96500 \ C \ mol^{-1}$)

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How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.