(D) According to Faraday's law of electrolysis,the mass deposited $(m)$ is given by: $m = \frac{M \times Q}{n \times F}$Where $M = 118 \ g/mol$,$Q = 2

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(D) According to Faraday's law of electrolysis,the mass deposited $(m)$ is given by: $m = \frac{M \times Q}{n \times F}$Where $M = 118 \ g/mol$,$Q = 24125 \ C$,$F = 96500 \ C/mol$,and $m = 7.375 \ g$.Substituting the values: $7.375 = \frac{118 \times 24125}{n \times 96500}$$n = \frac{118 \times 24125}{7.375 \times 96500}$$n = \frac{2846750}{711687.5} \approx 4$Therefore,the charge on the tin ion is $+4$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

What is the charge on tin if $7.375 \ g$ of metallic tin is deposited by the passage of $24125 \ C$ through a solution containing the ion? [Atomic weight of $Sn = 118 \ g/mol$]

A
$+1$
B
$+3$
C
$+2$
D
$+4$

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Faraday’s law of electrolysis

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When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

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What is the charge on tin if $7.375 \ g$ of metallic tin is deposited by the passage of $24125 \ C$ through a solution containing the ion? [Atomic weight of $Sn = 118 \ g/mol$]

Similar Questions

How much electricity in terms of Faraday is required to produce:$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?

If solutions of silver nitrate and cupric salt are connected in series and the same current is passed,what will be the weight of copper deposited in $gm$ when $1.08 \ g$ of silver is deposited?

$A$ solution of $CuSO_4$ is electrolysed for $10 \,min$ with a current of $1.5 \,A$. What is the mass of copper deposited at the cathode (in $,g$)?

In the electrolysis of an aqueous $NiI_2$ solution using $Ni$ electrodes,what happens to the mass of the cathode upon passing $1$ equivalent of charge? (Given: atomic mass of $Ni = 59$)

When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

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How much electricity in terms of Faraday is required to produce:
$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?
$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?