(A) The volume of $Cu$ deposited is $V = \text{Area} \times \text{thickness} = (20 \times 5) \ cm^2 \times (3.6 \times 10^{-4} \ cm) = 0.036 \ cm^3$.

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(A) The volume of $Cu$ deposited is $V = \text{Area} \times \text{thickness} = (20 \times 5) \ cm^2 \times (3.6 \times 10^{-4} \ cm) = 0.036 \ cm^3$. The mass of $Cu$ deposited is $W = V \times d = 0.036 \ cm^3 \times 8.9 \ g/cm^3 = 0.3204 \ g$. Using Faraday's law,$W = \frac{M \times Q}{n \times F}$,where $M = 63.5 \ g/mol$,$n = 2$,and $F = 96500 \ C/mol$. $Q = \frac{W \times n \times F}{M} = \frac{0.3204 \times 2 \times 96500}{63.5} \approx 973.81 \ C \approx 974 \ C$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

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A
$974$
B
$580$
C
$1080$
D
$365$

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Faraday’s law of electrolysis

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Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

Similar Questions

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 $1 \ C$ of electricity is passed through an electrolytic solution,the mass deposited on the electrode is equal to which of the following?

When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?

To deposit one litre of hydrogen at $22.4 \text{ atmosphere}$ from acidulated water,the quantity of electricity that must pass through is ............. $coulomb$.

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Which is the weight of $Al$ deposited at cathode when $1 \ A$ current is passed through molten $AlCl_3$ for $9650 \ s$ (in $g$)?
(Atomic mass of $Al = 27$)