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Electrolytic Cells and Electrolysis

Electrochemistry

Chemistry

Class 12

Overview

Describe the components, working and chemistry behind an Electrolytic cell.

Learn

Videos

Introduction to Electrolysis

9 mins

Faraday's First Law of Electrolysis

12 mins

Faradays Second Law of Electrolysis

25 mins

Numerical on Faraday's First Law of Electrolysis

13 mins

Numerical on Faraday's Second Law of Electrolysis

12 mins

Electrolysis of Molten NaCl

14 mins

Study Materials

Electrolysis: Electrolytic cells and Electrolysis, Process, Examples, Videos Fuel Cells: Working, Setup, Role of Electrolyte and Advantages, Examples Conductance of electrolytic solutions: Types of Conductors and Factors affecting Electrolytic Conduction

Quick summary with Stories

Introduction to Electrolysis

3 mins mins read

Faraday Second Law of Electrolysis

3 mins mins read

Revise with Concepts

Electrolytic Cells and Electrolysis

ExampleDefinitionsFormulaes

Faraday's Law

ExampleDefinitionsFormulaes

Products of Electrolysis

ExampleDefinitionsFormulaes

Practice Questions

That are catagorized depending on difficulty level

Easy Medium Hard

A current of 4.0 A is passed for 5 hours through 1L of 2M solution of nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be:

Hard

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Complete the following reaction:
$C r_{2} O_{7}^{2 -} + 2 O H^{-} \to$

Medium

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A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:

Medium

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On electrolysis, water splits into :

Easy

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$96500$ coulombs of electric current liberates from $C u S O_{4}$ solution

Medium

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$(a)$ A current of $1.50 A$ was passed through an electrolytic cell containing $A g N O_{3}$ solution with inertelectrodes. The weight of $A g$ deposited was $1.50 g$ . How long did the current flow?
$(b)$ Write the reactions taking place at the anode and cathode in all the above cell.
$(c)$ Give reactions taking place at the two electrodes if these are made up of $A g$ .

Hard

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If $m$ is the mass of silver deposited at the cathode by $2 A$ current flowing for $25 m i n$ through a silver voltameter, then the mass deposited by $1.5 A$ current flowing for $600 s$ is _________.

Medium

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A layer of chromium metal $0.25 m m$ thick is to be plated on an auto bumper with a total area of $0.32 m^{2}$ from a solution containing $C r O_{4}^{2 -}$ . What current flow is required for this electroplating if the bumper is to be plated in $60 s$ ? The density of chromium metal is $7.20 g / c m^{3}$ .

Hard

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To deposit one gm equivalent of an element at an electrode, the quantity of electricity needed is

Medium

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The compounds which do not decompose on passage of an electric current through them are known as:

Easy

View solution

Electrolytic Cells and Electrolysis

Overview

Learn

Videos

Study Materials

Quick summary with Stories

Introduction to Electrolysis

Faraday Second Law of Electrolysis

Revise with Concepts

Electrolytic Cells and Electrolysis

Faraday's Law

Products of Electrolysis

Related questions

A current of 4.0 A is passed for 5 hours through 1L of 2M solution of nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be:

Complete the following reaction:
$C r_{2} O_{7}^{2 -} + 2 O H^{-} \to$

A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:

On electrolysis, water splits into :

$96500$ coulombs of electric current liberates from $C u S O_{4}$ solution

If $m$ is the mass of silver deposited at the cathode by $2 A$ current flowing for $25 m i n$ through a silver voltameter, then the mass deposited by $1.5 A$ current flowing for $600 s$ is _________.

To deposit one gm equivalent of an element at an electrode, the quantity of electricity needed is

The compounds which do not decompose on passage of an electric current through them are known as:

More topics

Electrolytic Cells and Electrolysis

Overview

Learn

Videos

Study Materials

Quick summary with Stories

Introduction to Electrolysis

Faraday Second Law of Electrolysis

Revise with Concepts

Electrolytic Cells and Electrolysis

Faraday's Law

Products of Electrolysis

Related questions

A current of 4.0 A is passed for 5 hours through 1L of 2M solution of nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be:

Complete the following reaction: Cr2​O72−​+2OH−→

A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:

On electrolysis, water splits into :

96500 coulombs of electric current liberates from CuSO4​ solution

If m is the mass of silver deposited at the cathode by 2A current flowing for 25min through a silver voltameter, then the mass deposited by 1.5A current flowing for 600s is _________.

A layer of chromium metal 0.25 mm thick is to be plated on an auto bumper with a total area of 0.32 m2 from a solution containing CrO42−​. What current flow is required for this electroplating if the bumper is to be plated in 60s? The density of chromium metal is 7.20 g/cm3.

To deposit one gm equivalent of an element at an electrode, the quantity of electricity needed is

The compounds which do not decompose on passage of an electric current through them are known as:

More topics

Complete the following reaction:
$C r_{2} O_{7}^{2 -} + 2 O H^{-} \to$

$96500$ coulombs of electric current liberates from $C u S O_{4}$ solution

If $m$ is the mass of silver deposited at the cathode by $2 A$ current flowing for $25 m i n$ through a silver voltameter, then the mass deposited by $1.5 A$ current flowing for $600 s$ is _________.