(B) According to Faraday's law of electrolysis,the mass deposited is $m = ZIt$,where $Z$ is the electrochemical equivalent of the substance.Since the

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(B) According to Faraday's law of electrolysis,the mass deposited is $m = ZIt$,where $Z$ is the electrochemical equivalent of the substance.Since the substance is silver in both cases,$Z$ is constant.For the first case: $m_1 = m = Z \times 4 \times (2 \times 60) = 480 \ Z$.For the second case: $m_2 = Z \times 6 \times 40 = 240 \ Z$.Taking the ratio: $\frac{m_2}{m_1} = \frac{240 \ Z}{480 \ Z} = \frac{1}{2}$.Therefore,$m_2 = \frac{m_1}{2} = \frac{m}{2}$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be

A
$4 \ m$
B
$\frac{m}{2}$
C
$\frac{4 \ m}{3}$
D
$3 \ m$

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Electrochemistry

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Faraday’s law of electrolysis

When a current of $2 \ A$ is passed for $2 \ hours$ through a copper voltameter,$W \ g$ of copper is deposited. If a current of $1 \ A$ is passed for $4 \ hours$ through the same voltameter,how much copper will be deposited?

Medium

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The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

DifficultMHT CET 2007

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The current flowing in a copper voltameter is $3.2 \ A$. The number of copper ions $(Cu^{2+})$ deposited at the cathode per minute is

Easy

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Clarify the stoichiometry of the reactions occurring on the electrodes of an electrolytic cell and its relationship with the quantity of electricity.

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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 $........ \ C$.

MediumNEET 2014

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In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be

Similar Questions

When a current of $2 \ A$ is passed for $2 \ hours$ through a copper voltameter,$W \ g$ of copper is deposited. If a current of $1 \ A$ is passed for $4 \ hours$ through the same voltameter,how much copper will be deposited?

The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

The current flowing in a copper voltameter is $3.2 \ A$. The number of copper ions $(Cu^{2+})$ deposited at the cathode per minute is

Clarify the stoichiometry of the reactions occurring on the electrodes of an electrolytic cell and its relationship with the quantity of electricity.

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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