(B) According to Faraday's law of electrolysis,the mass $m$ deposited is given by $m = \frac{E \times i \times t}{96500}$,where $E$ is the chemical eq

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$6 \ \text{min} \ 42 \ \text{sec}$

(B) According to Faraday's law of electrolysis,the mass $m$ deposited is given by $m = \frac{E \times i \times t}{96500}$,where $E$ is the chemical equivalent.Given: $m = 20 \ mg = 20 \times 10^{-3} \ g$,$i = 0.15 \ A$,$E = 32$.Substituting the values: $20 \times 10^{-3} = \frac{32 \times 0.15 \times t}{96500}$.$t = \frac{20 \times 10^{-3} \times 96500}{32 \times 0.15} = \frac{1930}{4.8} \approx 402.08 \ \text{sec}$.$402 \ \text{sec} = 6 \ \text{min} \ 42 \ \text{sec}$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Easy

If $96500 \ C$ of electricity liberates one gram equivalent of any substance,the time taken for a current of $0.15 \ A$ to deposit $20 \ mg$ of copper from a solution of copper sulphate is (Chemical equivalent of copper = $32$).

A
$5 \ \text{min} \ 20 \ \text{sec}$
B
$6 \ \text{min} \ 42 \ \text{sec}$
C
$4 \ \text{min} \ 40 \ \text{sec}$
D
$5 \ \text{min} \ 50 \ \text{sec}$

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Class 12

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Electrochemistry

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Faraday’s law of electrolysis

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

EasyWBJEE 2018

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Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

DifficultAIEEE 2005

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How many atoms of calcium will be deposited at the cathode when a current of $25 \ mA$ is passed through a $CaCl_2$ solution for $60 \ s$?

Medium

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Match the column :-
Column $I$ (Reduction process) Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$ $(p)$ $193000$ $C$
$(b)$ $1$ mole of $Cr_2O_7^{2-}$ to $Cr^{3+}$ $(q)$ $289500$ $C$
$(c)$ $1$ mole of $Sn^{4+}$ to $Sn^{2+}$ $(r)$ $482500$ $C$
$(d)$ $1$ mole of $Al^{3+}$ to $Al$ $(s)$ $579000$ $C$

Column $I$ (Reduction process)	Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$	$(p)$ $193000$ $C$
$(b)$ $1$ mole of $Cr_2O_7^{2-}$ to $Cr^{3+}$	$(q)$ $289500$ $C$
$(c)$ $1$ mole of $Sn^{4+}$ to $Sn^{2+}$	$(r)$ $482500$ $C$
$(d)$ $1$ mole of $Al^{3+}$ to $Al$	$(s)$ $579000$ $C$

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State Faraday's laws of electrolysis and mention their uses.

Medium

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If $96500 \ C$ of electricity liberates one gram equivalent of any substance,the time taken for a current of $0.15 \ A$ to deposit $20 \ mg$ of copper from a solution of copper sulphate is (Chemical equivalent of copper = $32$).

Similar Questions

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

Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

How many atoms of calcium will be deposited at the cathode when a current of $25 \ mA$ is passed through a $CaCl_2$ solution for $60 \ s$?

State Faraday's laws of electrolysis and mention their uses.

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