(B) The reaction at the cathode is: $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$For $63 \ g$ of $Cu$,the electricity required is $2 \ F$ $(2 \times 96500 \

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(B) The reaction at the cathode is: $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$For $63 \ g$ of $Cu$,the electricity required is $2 \ F$ $(2 \times 96500 \ C)$.So,for $0.4725 \ g$ of $Cu$,the electricity required $(Q)$ is: $Q = \frac{2 \times 96500 \times 0.4725}{63} = 1447.5 \ C$.Using Faraday's law: $Q = I \times t$,where $t = 15 \times 60 \ s = 900 \ s$.$I = \frac{Q}{t} = \frac{1447.5}{900} = 1.608 \ A$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

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A
$0.804$
B
$1.608$
C
$1.206$
D
$0.402$

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Class 12

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Electrochemistry

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Faraday’s law of electrolysis

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$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

Similar Questions

If $5 \ A$ of current is passed for $193 \ s$ through a solution containing $Cu$ salt,$0.32 \ g$ of copper is deposited. What is the oxidation state of the $Cu$ in the salt?

What current strength in $amp$ will be required to liberate $10 \ g$ of chlorine from $NaCl$ solution in one hour?

In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be

How long a current of $3 \, A$ has to be passed through a solution of $AgNO_3$ to coat a metal surface of $80 \, cm^2$ with $0.005 \, mm$ thick layer? Density of $Ag$ is $10.5 \, g/cm^3$. (Answer in $sec$)

When $X$ amperes of current is passed through molten $AlCl_3$ for $96.5$ $s$,$0.09$ $g$ of aluminium is deposited. What is the value of $X$?

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