(C) According to Faraday's law of electrolysis,the mass deposited is given by $m = Z i t$,where $Z = \frac{E}{F}$.Substituting $Z$,we get $m = \frac{E

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(C) According to Faraday's law of electrolysis,the mass deposited is given by $m = Z i t$,where $Z = \frac{E}{F}$.Substituting $Z$,we get $m = \frac{E \times i \times t}{F}$,which implies $t = \frac{m \times F}{E \times i}$.Given: $m = 27 \ g$,$E = 108$,$i = 2 \ A$,and $F = 96500 \ C/mol$.$t = \frac{27 \times 96500}{108 \times 2} = 12062.5 \ s$.To convert seconds to hours,divide by $3600$: $t = \frac{12062.5}{3600} \ hr \approx 3.35 \ hr$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

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The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.

A
$8.57$
B
$6.70$
C
$3.35$
D
$12.50$

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Faraday’s law of electrolysis

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The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.

Similar Questions

$A$ current of $2 \ A$ passing for $5 \ hours$ through molten tin salt deposited $22.2 \ g$ of tin. The oxidation state of tin in the salt is . . . . . . . (Atomic mass of $Sn = 119$)

The relation between Faraday constant $F$,electron charge $e$,and Avogadro number $N$ is:

When a current of $9.65 \ A$ is passed for $10 \ \text{minutes}$,$3.0 \ g$ of metal is deposited. What is the equivalent weight of the metal?

What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through a solution of an electrolyte for $10 \text{ minutes}$?

What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \text{ mL}$ of $1 \text{ M AgNO}_3$ solution?

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