(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

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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:

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

The current flowing in a copper voltameter is $1.6 \ A$. The number of $Cu^{2+}$ ions deposited at the cathode per minute are

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When the same quantity of electricity is passed through solutions of $Ag^{+}$,$Cu^{2+}$,and $Fe^{3+}$ ions,what is the ratio of the number of moles of each metal deposited?

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How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

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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 $60 \ s$?

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On passing $C$ ampere of current for time $t$ seconds through $1 \ L$ of $2 \ M$ $CuSO_4$ solution (atomic weight of $Cu = 63.5$), the amount $m$ of $Cu$ (in grams) deposited on the cathode will be:

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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

The current flowing in a copper voltameter is $1.6 \ A$. The number of $Cu^{2+}$ ions deposited at the cathode per minute are

When the same quantity of electricity is passed through solutions of $Ag^{+}$,$Cu^{2+}$,and $Fe^{3+}$ ions,what is the ratio of the number of moles of each metal deposited?

How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

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 $60 \ s$?

On passing $C$ ampere of current for time $t$ seconds through $1 \ L$ of $2 \ M$ $CuSO_4$ solution (atomic weight of $Cu = 63.5$), the amount $m$ of $Cu$ (in grams) deposited on the cathode will be:

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