(B) Total mass of $Al$ required = $24 \times 5.0 \ g = 120 \ g$. Using Faraday's law: $w = \frac{M}{n \times F} \times I \times t \times \text{efficie

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(B) Total mass of $Al$ required = $24 \times 5.0 \ g = 120 \ g$. Using Faraday's law: $w = \frac{M}{n \times F} \times I \times t \times \text{efficiency}$. Here,$w = 120 \ g$,$M = 27 \ g/mol$,$n = 3$ (for $Al^{3+} + 3e^- \rightarrow Al$),$F = 96500 \ C/mol$,$I = 9650 \ A$,and efficiency = $0.90$. $120 = \frac{27}{3 \times 96500} \times 9650 \times t \times 0.90$. $120 = \frac{27}{30} \times t \times 0.90$. $120 = 0.9 \times 0.9 \times t$. $120 = 0.81 \times t$. $t = \frac{120}{0.81} \approx 148.14 \ s$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

In the Hall process,aluminium is produced by the electrolysis of molten $Al_2O_3$. How many seconds would it take to produce enough aluminium by the Hall process to make a case of $24$ cans of aluminium soft-drink,if each can uses $5.0 \ g$ of $Al$,a current of $9650 \ A$ is employed,and the current efficiency of the cell is $90.0 \ \%$?

A
$203.2$
B
$148.14$
C
$333.33$
D
$6.17$

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Class 12

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Electrochemistry

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Faraday’s law of electrolysis

When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?

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When the same quantity of electricity is passed through the aqueous solutions of the given electrolytes for the same amount of time,which metal will be deposited in maximum amount on the cathode?

MediumTS EAMCET 2021

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Two Faraday of electricity is passed through a solution of $CuSO_4$. The mass of copper deposited at the cathode is ......... $g$. (at. mass of $Cu = 63.5 \ amu$)

DifficultJEE MAIN 2015

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When electric current is passed through acidified water for $1930 \,s$, $1120 \,mL$ of $H_2$ gas is collected (at $STP$) at the cathode. What is the current passed in amperes?

DifficultTS EAMCET 2008

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The amount of substance deposited when a current of $1 \ A$ is passed for $1 \ s$ is equal to:

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When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?

When the same quantity of electricity is passed through the aqueous solutions of the given electrolytes for the same amount of time,which metal will be deposited in maximum amount on the cathode?

Two Faraday of electricity is passed through a solution of $CuSO_4$. The mass of copper deposited at the cathode is ......... $g$. (at. mass of $Cu = 63.5 \ amu$)

When electric current is passed through acidified water for $1930 \,s$, $1120 \,mL$ of $H_2$ gas is collected (at $STP$) at the cathode. What is the current passed in amperes?

The amount of substance deposited when a current of $1 \ A$ is passed for $1 \ s$ is equal to:

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