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Buniyaad NCERT Line by Electrochemistry | Boards | NEET #neet #cbse #cbseboard #neet2024

Vora Classes NEET & Boards・2 minutes read

By studying electrochemistry, students can gain a comprehensive understanding of topics like oxidation, reduction, and electron flow, crucial for various competitive exams and academic assessments. Practical applications like calculating electromotive force and understanding Faraday's laws play a significant role in grasping the concepts of electrochemistry for board exams and NEET preparation.

Insights

Electro Chemistry chapter discussed for CBSE, NEET, and JE Mains prep, engaging and easier to memorize with prior knowledge.
Practical aspects include using agar agar powder to create a Salt Bridge essential for completing electrochemical circuits.
Understanding Electrochemical Cells' setup, like Galvanic Cells, is crucial for competitive exams and board questions.
External voltage application to a Galvanic Cell demonstrates practical applications with a 1.1 volts EMF.
Concepts like Faraday's constant, Nernst equation, and equilibrium constants are fundamental for electrochemistry understanding.

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Recent questions

What is the purpose of a Salt Bridge in electrochemical cells?
The Salt Bridge completes the circuit in cells.
How does an Electrochemical Cell function?
Anode is negatively charged, cathode is positively charged.
What is the significance of EMF in Galvanic Cells?
EMF demonstrates practical application of concepts.
How are reduction potentials utilized in determining EMF?
Reduction potentials aid in calculating cell EMF.
What is the role of Faraday's constant in electrochemistry?
Faraday's constant is crucial for charge calculations.

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Summary

00:00

Electro Chemistry: Essential Concepts for Exams

The chapter being discussed is Electro Chemistry, particularly beneficial for CBSE board, NEET, and JE Mains preparation.
The chapter is engaging for children due to its intriguing nature, making it easier to memorize with some prior knowledge.
The session is focused on covering the chapter line by line, with a total of 61 pages to be completed.
Practical aspects of the chapter include the use of agar agar powder to create a Salt Bridge for completing the circuit.
The Salt Bridge is crucial for the completion of the circuit in electrochemical cells.
The overall cell reaction involves zinc being oxidized to copper, generating electricity in a spontaneous redox reaction.
The type of cell discussed is known as an Electrochemical Cell or Galvanic Cell, exemplified by the Daniel Cell.
In a Galvanic Cell, the anode is negatively charged, while the cathode is positively charged, aiding in the understanding of oxidation and reduction processes.
The details provided are essential for understanding the setup and functioning of electrochemical cells, crucial for competitive exams and board questions.
Applying an external voltage to a Galvanic Cell can result in an EMF of 1.1 volts, demonstrating the practical application of the concepts discussed.

15:54

"Understanding Electrochemical Cells and EMF Calculation"

The voltage of the system is 1.1 volts, with electrons flowing from zinc to copper and current flowing in the opposite direction.
If an external voltage lower than 1.1 volts is applied, the same electron and current flow pattern continues, resulting in zinc dissolution and copper deposition.
When the external voltage matches the system's voltage of 1.1 volts, no electron or current flow occurs, maintaining equilibrium.
Applying a voltage higher than 1.1 volts forces electrons to move in the opposite direction, causing a reversal in the electron and current flow.
The process involves reactions between zinc and copper ions, leading to the formation of copper and zinc compounds.
The system is divided into anodic and cathodic compartments, with reduction and oxidation reactions occurring at each electrode.
The reduction potential is crucial in determining the direction of electron flow, with the anode always placed on the left and the cathode on the right.
To calculate the cell's electromotive force (EMF), subtract the reduction potentials of the cathode and anode.
The EMF represents the potential difference between the two half-cells when no current is drawn from the system.
Following conventions and understanding reduction potentials are essential in accurately determining the EMF of the cell for practical applications.

30:43

Studying Electro Kinetics and Cell Reactions

Chemistry chapters remaining to be studied, focusing on Electro Kinetics and D&F Coordination.
Four to five days allocated for studying chemistry to sort out concepts.
Discussion on oxidation occurring on the anode, specifically related to copper oxidation.
Explanation of the process of oxidation and electron transfer on the anode and cathode.
Troubleshooting a voice lag issue during the discussion.
Detailed explanation of the Standard Hydrogen Electrode setup for measuring potential.
Step-by-step process of setting up an experiment to determine the EMF of a cell.
Instructions on writing cell reactions and representations for academic purposes.
Importance of understanding and applying values of EMF in academic assessments.
Introduction to Gas Ion Half Cell setup using bromine gas and platinum electrode.

44:24

"Chemical Reactions and Reduction Potentials Simplified"

A positive wants to undergo self-reduction to act as an oxidant and cause oxidation in others.
B positive desires to be converted to B to act as an oxidant and undergo reduction.
Fluorine, with a reduction potential of 2.87, aims to be reduced and act as a strong oxidant.
Lithium, acting as a reducing agent, seeks to undergo self-oxidation and cause reduction in others.
The strongest reducing agent is VK, while VK acts as an oxidant.
Focus on NCERT for better understanding and direct questions in exams.
To improve scores from 60-70 to 150-160, focus on NCERT concepts first.
Faraday's constant is 96500 coulombs per mole, not 965.
The Nernst equation involves balancing chemical equations and calculating E cell based on reduction potentials.
Concentration of pure solids or liquids is constant and ignored in the Nernst equation.

59:06

Electrochemical Reactions: Equilibrium, Energy, and Potential

The reaction involves representing a cell with magnesium and silver ions to form magnesium ions and silver.
The anode is made of magnesium, and the reduction process involves converting silver ions to silver.
The cell is represented as Mg2P | Mg2PS, with a concentration of APS.
The formula for calculating the cost of the product is 0.130 divided by the concentration of the reactant.
The temperature must be 298 Kelvin to use the formula 0.059 after n.
The equilibrium constant from the Nernst equation is crucial for understanding the reaction.
The equilibrium constant is calculated using the formula E cell = 2.303 RT/nF log Q.
The free energy concept in electrochemical cells is explained, emphasizing useful work done by the system.
The work done in an electrochemical cell is equal to the electrical potential multiplied by the charge.
The standard electrode potential and the calculation of the potential of a hydrogen electrode in a solution with pH 10 are essential practical applications.

01:14:50

"Hydrogen Electrode E Value Calculation Study"

Making a hydrogen electrode involves determining its E value in a pH 10 solution.
The equation for this process involves 2H+ plus 2 electrons forming hydrogen.
The value of E from H+ to H2 is calculated using the formula E cell = E n cell - 0.059 Ba n log concentration of the product.
To find the pressure for hydrogen gas product, the pressure for H+ square is considered.
The number of electrons involved affects the equation, with halving the electrons halving the result.
Calculating the value of H+ from H2 involves a specific formula, resulting in a value of -0.059.
Managing study time for both board exams and JE preparation involves allocating specific hours for each.
Effective study time is emphasized, with a focus on studying for 10 hours daily for optimal results.
The importance of understanding concepts like conductance and resistivity in electrochemistry is highlighted.
Superconductors and semiconductors are explained, with a mention of materials exhibiting zero resistivity at low temperatures.

01:28:15

"Metal and Ionic Conductivity: Factors and Calculations"

Electronic conductance is due to the movement of electrons in metals, which have valence shell electrons.
The conductivity of metals depends on the number of valence electrons and the structure of the metal.
Temperature affects electrical conductivity, with an increase in temperature leading to a decrease in electrical conductivity in metals.
Ionic conductance depends on the electrolyte used, with solvation varying based on the solvent employed.
The concentration of the electrolyte, measured in molarity, affects ionic conductance, increasing with higher concentrations.
A Wheatstone Bridge is used to calculate resistance, involving resistors and a variable register.
To measure resistance in a conductivity cell, platinum electrodes are placed on a sharpener-like cell with a solution.
Molar conductance is defined in electrolytic cells by adding electrolytes to measure conductance based on molarity.
Formulas for molar conductance calculations involve the relationship between conductivity, resistance, and molarity.
Practical examples involve calculating conductivity and molar conductivity based on given resistances, lengths, and concentrations.

01:43:38

"Improvement Exam Center, Conductivity, and Kohla's Law"

Improvement exam must be taken at the same center where the original exam was taken.
Aim for a decent percentage to ensure eligibility for competitive exams.
Completed 33 pages out of 60, with three studies left to finish.
Focus on stopping at the 40th page to complete one section.
Emphasize understanding the Variation of Conductivity and Molar Conductance.
Conductivity is the conductance of a solution enclosed in a 1 cm volume.
Conductivity decreases with dilution due to a reduction in the number of ions.
Molar conductance increases with dilution for strong electrolytes due to increased mobility of ions.
Weak electrolytes show a rapid increase in conductance with dilution.
Kohla's Law of Independent Migration of Ions is the final topic to study.

01:58:37

Ions Behavior in Solutions and Exam Prep

Kolash's Law of Independent Migration of IAS explains the behavior of ions in a solution, emphasizing that they do not interact with each other.
The story narrates a family living in a large house with multiple generations and relatives residing together.
The concept of a "dilute solution" is highlighted, indicating that all ions in the solution move independently.
The Law of Independent Migration of Ions to Colloids is introduced, detailing how ions behave in electrolytes.
Practical instructions are given on calculating the molar conductance of various compounds like CaCl2 and MgSO4.
The process of determining the dissociation constant for weak electrolytes is explained, involving the degree of dissociation and molarity.
Instructions are provided on calculating the degree of dissociation for acetic acid and other compounds.
The importance of not neglecting small values like alpha in calculations is emphasized.
Recommendations are made to study from NCRT and practice previous year questions for exams like JEE and NEET.
The teacher advises on the study plan, covering topics like chemical kinetics, D & F block elements, and coordination compounds for exam preparation.

02:15:54

Electrolyte Dissociation and Faraday's Laws

Differentiating between complete and incomplete dissociation in electrolytes
Determining the value of 'i' based on electrolyte strength and dissociation completeness
Strong electrolytes exhibit complete dissociation, while weak electrolytes show incomplete dissociation
Significance of 'k' value in determining electrolyte strength, with high values indicating strong electrolytes
Transition to the fifth lesson on electrolytic Faraday, cell, and electrolysis in class
Exploring the process of electrolysis to produce electricity from redox reactions
Illustrating the conversion of copper electrodes through electrolysis in a copper sulfate solution
Anode oxidation leading to copper deposition and cathode reduction in electrolysis
Introduction to Faraday's laws, focusing on the relationship between charge passed and substance deposited
Application of Faraday's laws in calculating substance deposition in electrolysis, emphasizing equivalent mass concept

02:30:38

Key Concepts in Electrochemistry and Reactions

The formula for calculating the quantity of electricity is q = n * n factor, where q represents charge in coulombs.
To determine the number of moles needed to reduce a substance, the mole concept is applied, with 1 mole of Cr2 72 mine requiring 6 moles of electrons.
The oxidation state of chromium shifts from +6 to +3 and then +4 during a chemical reaction.
The factor for the quantity of electricity needed is 6 Farad, equivalent to 6 * 96500 coulombs.
Balancing equations is crucial in chemical reactions to ensure accurate results.
Electrolysis processes involve the release of hydrogen gas at the cathode and chlorine gas at the anode.
The standard electrode potential and overpotential play significant roles in determining the products of electrolysis.
Different oxidant reducing species present in an electrolytic cell influence the products of electrolysis.
The electrolysis of sulfuric acid results in the release of oxygen gas during dilution and the formation of h2o - s2 o8 2 - in concentrated solutions.
Understanding the basics of batteries, corrosion, and fuel cells is essential for a comprehensive grasp of electrochemistry.

02:45:49

"Electrochemistry Practice: Predicting Reactions and Products"

The topic covered in today's session was electrochemistry, specifically focusing on practicing questions related to the subject.
Specific questions marked for practice include 2.4, 2.9, 2.11, 2.14, and 2.15, with an emphasis on predicting feasible reactions and products of electrolysis.

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