(B) According to Faraday's first law of electrolysis,the mass deposited $W$ is directly proportional to the charge $Q$ $(W = ZIt)$.Therefore,$\frac{W_

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(B) According to Faraday's first law of electrolysis,the mass deposited $W$ is directly proportional to the charge $Q$ $(W = ZIt)$.Therefore,$\frac{W_1}{W_2} = \frac{I_1 \times t_1}{I_2 \times t_2}$.Given: $W_1 = m$,$I_1 = 4 \ A$,$t_1 = 2 \ \text{minutes} = 120 \ \text{seconds}$.Given: $I_2 = 6 \ A$,$t_2 = 40 \ \text{seconds}$.Substituting the values: $\frac{m}{W_2} = \frac{4 \times 120}{6 \times 40}$.$\frac{m}{W_2} = \frac{480}{240} = 2$.$W_2 = \frac{m}{2} \ g$.

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 $2 \ \text{minutes}$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ \text{seconds}$ will be:

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

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Class 12 Questions

Class 12

Chemistry Questions

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Electrochemistry

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Faraday’s law of electrolysis

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?

Medium

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In two separate experiments,the same quantity of electricity was passed through silver and gold solutions. The amounts of $Ag$ and $Au$ deposited are $2.15 \ g$ and $1.31 \ g$,respectively. The valency of gold is [Atomic mass of $Ag = 107.9$; $Au = 197$].

MediumTS EAMCET 2022

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How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

Easy

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If nearly $10^5 \ C$ liberate $1 \ gm$ equivalent of aluminium,then the amount of aluminium (equivalent weight $9$) deposited through electrolysis in $20 \ minutes$ by a current of $50 \ A$ will be .............. $gm$.

MediumAIPMT 1998

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When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

Easy

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

Similar Questions

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?

In two separate experiments,the same quantity of electricity was passed through silver and gold solutions. The amounts of $Ag$ and $Au$ deposited are $2.15 \ g$ and $1.31 \ g$,respectively. The valency of gold is [Atomic mass of $Ag = 107.9$; $Au = 197$].

How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

If nearly $10^5 \ C$ liberate $1 \ gm$ equivalent of aluminium,then the amount of aluminium (equivalent weight $9$) deposited through electrolysis in $20 \ minutes$ by a current of $50 \ A$ will be .............. $gm$.

When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

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