NCERT Solutions For Class 12 Chemistry Chapter 3: Electrochemistry

Education Journalist | Study Abroad Strategy Lead

NCERT Solutions for class 12 Chemistry Chapter 3 Electrochemistry are provided in this article. It consists of all important formulas, chemical equations, important laws and numericals. Important topics covered in Class 12 Chemistry Chapter 3 Electrochemistry are:

Expected No.of Questions: 2 to 4 questions of 9 marks

Download PDF: NCERT Solutions for Class 12 Chemistry Chapter 3 Electrochemistry PDF

NCERT Solutions for Class 12 Chemistry Chapter 3

NCERT Solutions PDF for Class 12 Chemistry Chapter 3 Electrochemistry is given below.

NCERT Solutions

Class 12 Chemistry Chapter 3: Electrochemistry – Important Topics

Important topics of Class 12 Chemistry Chapter 3 Electrochemistry includes the following.

Electrochemistry deals with the study of electricity in chemistry involving electrodes, electrolysis, solutions and solvents. This mechanism is commonly seen in Electrochemical cells. There are two common types of electrochemical cells.

Galvanic Cell: In this, chemical energy is converted to electrical energy. It is also known as voltaic cell. Here, the anode is negatively charged and cathode is positively charged.

Electrolytic Cell: In this, electrical energy is converted to chemical energy. Here, the cathode is negatively charged and anode is positively charged.

Standard Electrode Potential is the standard EMF of the cell. The potential difference between the electrode and electrolyte is known as the potential of electrode and at unit concentration.

E⁰_Cell = E⁰_{red, Cathode} – E⁰_{red, Anode}

Nernst equation is establishes the relation between the cell potential of an electrochemical cell, the standard cell potential, temperature, and the reaction quotient.

$E_{cell} = E^0 _{cell} - \frac{RT}{nF}ln Q$

Also Read:

Related Articles
Cell Potential	Electrodes	Quantitative aspect of Electrolysis
Product of electrolysis	Molar conductivity variations	Uses of Electroplating
Non electrolytes	Reduction Potential	Daniel Cell

Check-Out:

PCMB Study Guides
NCERT Solutions for Class 12 Physics	Class 12 Physics Notes	Formulas in Physics
Topics for Comparison in Physics	Choice-based questions in physics	Topics in relation to physics
Physics Study Notes	Class 12 Physics Book PDF	Class 12 Physics Practicals
Important Derivations in Physics	SI units in Physics	Important Physics Constants and Units
Class 12 Physics Syllabus	Mendeleev's Periodic Table	NCERT Solutions for Class 12 Biology
NCERT Solutions for Class 12 English	NCERT Solutions for Class 11 Chemistry	Class 12 Chemistry Practicals
Class 12 Chemistry Notes	Important Chemical Reactions	Class 12 Maths Notes
Class 12 PCMB Notes	NCERT Class 12 Biology Book	NCERT Class 12 Maths Book
NCERT Class 12 Textbooks	NCERT Solutions for Class 11 Maths	NCERT Solutions for Class 11 Physics
NCERT Solutions for Class 12 Maths	NCERT Solutions for Class 11 Biology	NCERT Solutions for Class 11 English
NCERT Class 11 Chemistry Book	NCERT Class 11 Physics Book	NCERT Class 11 Biology Book
Class 11 Notes	Important Maths Formulas	Important Chemistry Formulas
Class 11 PCMB Syllabus	Chemistry Study Notes	Biology Study Notes
Periodic Table in Chemistry	Important Chemical Reactions	Comparison topics in Chemistry
Comparison Topics in Maths	Biology MCQs	Important Named Reactions
Maths MCQs	Comparison Topics in Biology	Chemistry MCQs

CBSE CLASS XII Related Questions

1.
A solution is prepared by dissolving 0.025 g of potassium sulphate in 2 L of water at 27$^\circ$C. Assuming potassium sulphate is completely dissociated, determine its osmotic pressure. Given: \[ R=0.082 \, L\,atm\,K^{-1}mol^{-1} \] \[ \text{Molar mass of }K_2SO_4=174\,g\,mol^{-1} \] (ii) What type of azeotrope will be formed by a solution of acetone and chloroform? Give reason.
View Solution
2.
Calculate the freezing point of a solution when 10.5 g of MgBr$_2$ was dissolved in 250 g of water, assuming MgBr$_2$ undergoes complete dissociation. Given: \[ \text{Molar mass of MgBr}_2 = 184 \, g\,mol^{-1} \] \[ K_f \text{ for water} = 1.86 \, K\,kg\,mol^{-1} \] (ii) Write two differences between ideal and non-ideal solutions.
View Solution
3.
How much charge in faraday is required for the reduction of 1 mol of Ag$^+$ to Ag?
View Solution
4.
The following reactions occur at the anode during the electrolysis of aqueous sodium chloride solution: \[ Cl^-_{(aq)} \rightarrow \frac{1}{2}Cl_2(g)+e^- \qquad E^\circ_{\text{cell}}=1.36\,V \] \[ 2H_2O(l) \rightarrow O_2(g)+4H^+(aq)+4e^- \qquad E^\circ_{\text{cell}}=1.23\,V \] Which reaction is feasible at the anode and why?
View Solution
5.
Answer the following: (I) Which isomer of C$_4$H$_9$Br is most reactive towards S$_N$1 reaction? (II) Predict the alkene that would be formed by dehydrohalogenation of 1-Bromo-1-methylcyclohexane. (III) Although chlorine shows strong $-I$ effect, yet it is ortho/para-directing in electrophilic aromatic substitution reactions. Why? (ii) Write the major product in the following reactions: (I)
(II)
View Solution
6.
(I) Why do transition metals show variable oxidation states? (II) Out of Mn$^{2+}$ and Ti$^{2+}$ which will be more paramagnetic and why? Atomic No.: Ti = 22, Mn = 25 (III) Which ion is the strongest oxidising agent in the options given below: \[ Cr^{3+},\ V^{3+},\ Mn^{3+} \] Atomic No.: Cr = 24, V = 23, Mn = 25 (ii) Complete and balance the following equations: (I) \[ 2MnO_2+4KOH+O_2\rightarrow ? \] (II) \[ 5C_2O_4^{2-}+2MnO_4^-+16H^+\rightarrow ? \]
View Solution