(D) The reduction reaction is $Al^{3+} + 3e^{-} \rightarrow Al$. From the stoichiometry,$3 \ mol$ of electrons are required to produce $1 \ mol$ of $A

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(D) The reduction reaction is $Al^{3+} + 3e^{-} \rightarrow Al$. From the stoichiometry,$3 \ mol$ of electrons are required to produce $1 \ mol$ of $Al$. $1 \ mol$ of $Al = 27 \ g$. Charge required for $27 \ g$ of $Al = 3 \times 96500 \ C = 289500 \ C$. Mass of $Al$ to be produced = $5.12 \ kg = 5120 \ g$. Charge required for $5120 \ g$ of $Al = \frac{289500 \ C}{27 \ g} \times 5120 \ g$. Charge $\approx 5.49 \times 10^{7} \ C$.

Class 12 Chemistry Electrochemistry Faraday’s law of electrolysis

Medium

For the reaction $Al^{3+} + 3e^{-} \rightarrow Al$ (atomic mass of $Al = 27 \ g \ mol^{-1}$),calculate the quantity of electricity in coulombs required to produce $5.12 \ kg$ of $Al$.

A
$1.83 \times 10^{6} \ C$
B
$1.83 \times 10^{7} \ C$
C
$5.49 \times 10^{5} \ C$
D
$5.49 \times 10^{7} \ C$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Electrochemistry

Subtopic

Faraday’s law of electrolysis

If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)

Medium

View Solution

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?

Medium

View Solution

$A$ solution of $Fe_{2}(SO_{4})_{3}$ is electrolyzed for '$x$' min with a current of $1.5 \ A$ to deposit $0.3482 \ g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]
Given : $1 \ F = 96500 \ C \ mol^{-1}$
Atomic mass of $Fe = 56 \ g \ mol^{-1}$

EasyJEE MAIN 2022

View Solution

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:

Medium

View Solution

The laws of electrolysis were proposed by

Easy

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

For the reaction $Al^{3+} + 3e^{-} \rightarrow Al$ (atomic mass of $Al = 27 \ g \ mol^{-1}$),calculate the quantity of electricity in coulombs required to produce $5.12 \ kg$ of $Al$.

Similar Questions

If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)

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?

$A$ solution of $Fe_{2}(SO_{4})_{3}$ is electrolyzed for '$x$' min with a current of $1.5 \ A$ to deposit $0.3482 \ g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]Given : $1 \ F = 96500 \ C \ mol^{-1}$Atomic mass of $Fe = 56 \ g \ mol^{-1}$

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:

The laws of electrolysis were proposed by

Vedclass Test Series

Exam Paper Generator

Online Exam Module

$A$ solution of $Fe_{2}(SO_{4})_{3}$ is electrolyzed for '$x$' min with a current of $1.5 \ A$ to deposit $0.3482 \ g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]
Given : $1 \ F = 96500 \ C \ mol^{-1}$
Atomic mass of $Fe = 56 \ g \ mol^{-1}$