(C) According to Faraday's law of electrolysis,$W = \frac{M \times I \times t}{n \times F}$.Here,$W = 36 \ g$,$M = 108 \ g/mol$,$n = 1$ (for $Ag^+ + e

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(C) According to Faraday's law of electrolysis,$W = \frac{M \times I \times t}{n \times F}$.Here,$W = 36 \ g$,$M = 108 \ g/mol$,$n = 1$ (for $Ag^+ + e^- \rightarrow Ag$),$t = 7 \times 60 \ s = 420 \ s$,and $F = 96500 \ C/mol$.Substituting the values: $36 = \frac{108 \times I \times 420}{1 \times 96500}$.$I = \frac{36 \times 96500}{108 \times 420}$.$I = \frac{3474000}{45360} \approx 76.58 \ A \approx 76.6 \ A$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Easy

What current strength is required to deposit $36 \ g$ of $Ag$ in $7 \ minute$ from $AgNO_3$ solution by electrolysis (in $A$)? (Atomic mass $Ag = 108$)

MHT CET 2022 All MHT CET

A
$11.44$
B
$5.72$
C
$76.6$
D
$38.3$

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What current strength is required to deposit $36 \ g$ of $Ag$ in $7 \ minute$ from $AgNO_3$ solution by electrolysis (in $A$)? (Atomic mass $Ag = 108$)

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