(C) According to Faraday's first law of electrolysis,the mass of substance deposited is given by $w = \frac{I \times t \times M_{wt}}{n \times F}$.Her

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(C) According to Faraday's first law of electrolysis,the mass of substance deposited is given by $w = \frac{I \times t \times M_{wt}}{n \times F}$.Here,$I = 0.01 \ A$,$t = 3 \ hours = 3 \times 3600 \ s = 10800 \ s$,$w = 0.072 \ g$,$M_{wt} = 192 \ g/mol$,and $n = x$.Substituting the values: $0.072 = \frac{0.01 \times 10800 \times 192}{x \times 96500}$.$0.072 = \frac{108 \times 192}{x \times 96500}$.$x = \frac{108 \times 192}{0.072 \times 96500}$.$x = \frac{20736}{6948} \approx 2.98$.Thus,the value of $x$ is approximately $3$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

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

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Electrochemistry

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Faraday’s law of electrolysis

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

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When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

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What is the number of moles of electrons passed when a current of $5 \ A$ is passed through a solution of $FeCl_3$ for $20 \ minutes$?

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What amount of electricity can deposit $1 \ mole$ of $Al$ metal at cathode when passed through molten $AlCl_3$?

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Match List $I$ with List $II$.
List $I$ (Conversion) List $II$ (Number of Faraday required)
$A$. $1 \text{ mol of } H_2O \text{ to } O_2$ $I$. $3F$
$B$. $1 \text{ mol of } MnO_4^- \text{ to } Mn^{2+}$ $II$. $2F$
$C$. $1.5 \text{ mol of } Ca \text{ from molten } CaCl_2$ $III$. $1F$
$D$. $1 \text{ mol of } FeO \text{ to } Fe_2O_3$ $IV$. $5F$
Choose the correct answer from the options given below:

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List $I$ (Conversion)	List $II$ (Number of Faraday required)
$A$. $1 \text{ mol of } H_2O \text{ to } O_2$	$I$. $3F$
$B$. $1 \text{ mol of } MnO_4^- \text{ to } Mn^{2+}$	$II$. $2F$
$C$. $1.5 \text{ mol of } Ca \text{ from molten } CaCl_2$	$III$. $1F$
$D$. $1 \text{ mol of } FeO \text{ to } Fe_2O_3$	$IV$. $5F$

$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

Similar Questions

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

When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

What is the number of moles of electrons passed when a current of $5 \ A$ is passed through a solution of $FeCl_3$ for $20 \ minutes$?

What amount of electricity can deposit $1 \ mole$ of $Al$ metal at cathode when passed through molten $AlCl_3$?

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