Electrochemistry Class 12 One Shot | CBSE NEET JEE | Chapter 3

LearnoHub - Class 11, 12・2 minutes read

The video discusses electrochemistry, focusing on electromechanical and electrolytic aspects, exploring two types of chemical reactions, spontaneous and non-spontaneous, and applications such as batteries and electroplating. It explains the concept of redox reactions, cell potential, and the importance of electrode potential in understanding the generation of electricity from redox reactions.

Insights

  • Spontaneous reactions occur naturally without external influence, while non-spontaneous reactions require external energy to proceed, highlighting the importance of motivation in chemical reactions.
  • The use of a fold bridge in electrochemical cells is crucial for maintaining neutrality, completing the circuit, and allowing continuous current flow, showcasing the significance of this component in ensuring the functionality of the cell.

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Recent questions

  • What is electrochemistry?

    The video discusses the relationship between electricity and chemical reactions, focusing on electromechanical and electrolytic aspects. It explores spontaneous and non-spontaneous reactions, emphasizing the generation of electricity from chemicals and vice versa.

  • What are the applications of electrochemistry?

    Electrochemistry finds applications in batteries, electroplating, and various other uses. It involves converting chemical energy into electrical energy and vice versa, playing a significant role in redox reactions and the generation of electricity.

  • How does a Daniel cell operate?

    The Daniel cell, designed by John Daniels, involves zinc and copper combinations to generate chemical and electrical energy. It operates by accepting and releasing electrons, leading to reduction and oxidation processes, determining electrode potential and cell potential.

  • What factors affect conductivity in electrolytic solutions?

    Conductivity in electrolytic solutions is influenced by the nature of the electrolyte, solvent used, concentration, and dilution. Molar conductivity serves as a measure of conductivity activity, with conductivity decreasing rapidly when diluting a strong electrolyte due to incomplete dissociation.

  • How is molar conductivity calculated?

    Molar conductivity depends on dilution and concentration, with a rapid decrease in molar conductivity with increasing dilution. The Law of Independent Migration of Ions explains the relationship between limiting molar conductivity of electrolytes, involving complex equations and experimental data for calculation.

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Summary

00:00

"Essentials of Electrochemistry: Generating Electricity from Reactions"

  • The video discusses electrochemistry, focusing on electromechanical and electrolytic aspects.
  • Electrochemistry studies the relationship between electricity and chemical reactions.
  • Two types of chemical reactions are explored: electricity generation and chemical reactions with electricity.
  • Spontaneous reactions occur naturally, while non-spontaneous reactions require external energy.
  • Motivation is crucial in chemical reactions, with spontaneous reactions occurring without external influence.
  • Electrochemistry involves generating electricity from chemicals and converting chemical energy into electrical energy.
  • Applications of electrochemistry include batteries, electroplating, and various other uses.
  • Electrolytic processes involve converting electrical energy into chemical energy and vice versa.
  • Redox reactions play a significant role in electrochemistry, with oxidation and reduction always occurring in sequence.
  • Understanding the basics of electrochemistry is essential for grasping the generation of electricity from redox reactions.

21:49

"Charge Accumulation and Fold Bridge in Circuits"

  • Accumulation of positive charge on one side and negative charge on the other side due to the accumulation of SO4.
  • Previous state involved neutrals on both sides and copper on one side, now experiencing a positive charge buildup on one side and a negative charge buildup on the other.
  • The buildup is caused by the flow of electrons being stopped, leading to a halt in current flow.
  • To neutralize the buildup, a bridge called a "fold bridge" is introduced in the circuit, allowing for oxidation and reduction to occur.
  • The fold bridge contains an electrolyte to facilitate the movement of electrons and maintain neutrality on both sides.
  • The bridge ensures the completion of the circuit, allowing for continuous current flow and the functioning of the bulb.
  • The fold bridge plays a crucial role in maintaining neutrality, completing the circuit, and reducing the potential difference between oxidation and reduction.
  • The Daniel cell, designed by John Daniels, involves zinc and copper combinations to generate chemical and electrical energy.
  • The cell operates by accepting and releasing electrons, leading to reduction and oxidation processes.
  • Electrode potential and cell potential are determined by the difference in potential between the electrodes and the electrolyte, with the cell potential representing the overall potential difference in the cell.

44:34

"Vent Two Plus: Electrode Potential Extraction"

  • Vent Two Plus is made of a solution that involves dividing the electrolyte into two parts, with one side having ghee and the other side having sulphate.
  • Zinc is a metal that is part of the solution in Vent Two Plus, and it removes Sulphate Reddy through Sopore.
  • The representation of the cell involves using a vertical line metal and an electrolyte solution.
  • Copper and Silver are metals included in the Vent Two Plus solution.
  • The electrode location and behavior are determined by the representation of the cell, with Copper undergoing oxidation.
  • The reduction potential of metals is crucial, with the sign indicating the operation needed.
  • The electrode potential of metals like Copper and Zinc is determined by their reduced form stability compared to hydrogen.
  • The standard hydrogen electrode setup involves dipping a platinum electrode in a solution and connecting it to a volt meter.
  • The electrode potential of Zinc and Copper is calculated based on the readings from the volt meter, indicating their reduced form stability.
  • The notification OBC explains how to extract electrode potential in different concentrations, with the value varying based on the concentration of the solution.

01:11:12

"Electron Creation and Equilibrium in YouTube"

  • The reaction takes place in YouTube School, focusing on the creation of electrons and the concentration of CO2 acid.
  • Subscribing to the channel is encouraged for more content on reduction potential and minor irrigation potential.
  • The process involves the reduction potential of copper and states, emphasizing the importance of equilibrium.
  • Equilibrium is discussed, highlighting the creation of electrons and the formation of C.U.
  • The equilibrium constant is explored, with a focus on the relationship between Delta G and the equilibrium state.
  • The calculation of cell potential involves the transfer of electrons and the use of log values.
  • The Equilibrium content is detailed, with a focus on the balance between reduction and oxidation.
  • The calculation of electrode potential and the cost of a ₹1 note are explained.
  • The determination of reaction necessity is based on the value of notes and the presence of reduction.
  • The process involves the calculation of electron values and the identification of reduction locations.

01:44:45

"Understanding Conductivity in Electrolytic Solutions"

  • The value of the note is determined by the equation NotesEquals to log33.
  • The equation involves the use of a minus b, resulting in Point 3038 divided by the Law of Cassie.
  • The note's value is linked to the number of subscribers, with a total of 496 subscribers.
  • The text discusses the concept of electrolytic solutions and their conductivity.
  • Conductivity in electrolytic solutions is affected by the nature of the electrolyte and the solvent used.
  • The resistance in electrical circuits is directly proportional to the length of the conductor and inversely proportional to the area.
  • Conductors can be classified into semiconductor conductors with high conductivity and insulators with low conductivity.
  • The text explains metallic conduction and how temperature affects conductivity.
  • Electrolytes conduct electricity, with conductivity influenced by the concentration and nature of the solvent.
  • The molar conductivity is introduced as a measure of conductivity activity in electrolytes, affected by concentration and dilution.

02:12:58

"Electrolyte Conductivity: Dilution and Dissociation"

  • Leo discusses the difference in conductivity between two electrolytes, one increasing and the other decreasing rapidly.
  • Conductivity decreases rapidly when diluting a strong electrolyte due to incomplete dissociation.
  • Dilution of electrolytes leads to an increase in dissociation and conductivity.
  • Molar conductivity decreases rapidly with increasing dilution.
  • Graphically, molar conductivity increases with dilution for strong electrolytes.
  • Molar conductivity depends on dilution and concentration.
  • Limiting molar conductivity occurs when concentration approaches zero.
  • The Law of Independent Migration of Ions explains the relationship between limiting molar conductivity of electrolytes.
  • Calculation of molar conductivity involves complex equations and experimental data.
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