(B) According to Faraday's second law of electrolysis,for cells connected in series,the mass of substance deposited is proportional to its equivalent

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(B) According to Faraday's second law of electrolysis,for cells connected in series,the mass of substance deposited is proportional to its equivalent weight: $\frac{m_{Cu}}{m_{Ag}} = \frac{E_{Cu}}{E_{Ag}}$.Equivalent weight $E = \frac{\text{Atomic weight}}{\text{Valency}}$.For $Cu$ $(Cu^{2+})$: $E_{Cu} = \frac{63.57}{2} = 31.785$.For $Ag$ $(Ag^+)$: $E_{Ag} = \frac{107.88}{1} = 107.88$.Given $m_{Cu} = 1 \, mg$,we have $\frac{1}{m_{Ag}} = \frac{31.785}{107.88}$.$m_{Ag} = \frac{107.88}{31.785} \approx 3.394 \, mg \approx 3.4 \, mg$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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Two electrolytic cells containing $CuSO_4$ and $AgNO_3$ respectively are connected in series and a current is passed through them until $1 \, mg$ of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately ......... $mg$ [Atomic weights of copper and silver are respectively $63.57$ and $107.88$]

A
$1.7$
B
$3.4$
C
$5.1$
D
$6.8$

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Electrochemistry

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Faraday’s law of electrolysis

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

Medium

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How many faraday of electricity is required to produce $10 \ g$ of calcium metal (molar mass $= 40 \ g \ mol^{-1}$) from calcium ions (in $F$)?

MediumMHT CET 2021

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Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2 \ F$ electricity through an aqueous solution of potassium succinate,the total volume of gases (at both cathode and anode) at $STP$ ($1 \ atm$ and $273 \ K$) is .............. $L$

DifficultJEE MAIN 2016

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When a current of $0.5 \ A$ is passed for $2 \ hours$ through a molten metal salt,$3.88 \ g$ of the metal was deposited. If the atomic mass of the metal is $208 \ units$,the oxidation state of the metal in the salt is:

MediumAP EAMCET 2020

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$A$ constant current $(0.5 \, A)$ is passed for $1 \, hour$ through $(i)$ aqueous $AgNO_3$,$(ii)$ aqueous $CuSO_4$ and $(iii)$ molten $AlF_3$,separately. The ratio of the mass of the metals deposited on the cathode is $[M_{Ag}, M_{Cu}, M_{Al}$ are molar masses of the respective metals.]

MediumKVPY 2017

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Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

How many faraday of electricity is required to produce $10 \ g$ of calcium metal (molar mass $= 40 \ g \ mol^{-1}$) from calcium ions (in $F$)?

Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2 \ F$ electricity through an aqueous solution of potassium succinate,the total volume of gases (at both cathode and anode) at $STP$ ($1 \ atm$ and $273 \ K$) is .............. $L$

When a current of $0.5 \ A$ is passed for $2 \ hours$ through a molten metal salt,$3.88 \ g$ of the metal was deposited. If the atomic mass of the metal is $208 \ units$,the oxidation state of the metal in the salt is:

$A$ constant current $(0.5 \, A)$ is passed for $1 \, hour$ through $(i)$ aqueous $AgNO_3$,$(ii)$ aqueous $CuSO_4$ and $(iii)$ molten $AlF_3$,separately. The ratio of the mass of the metals deposited on the cathode is $[M_{Ag}, M_{Cu}, M_{Al}$ are molar masses of the respective metals.]

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