Electrochemistry - Class 12 Chemistry | NCERT for Boards & CUET

Apni Kaksha Official・2 minutes read

The importance of maintaining electricity at home to prevent acid consumption and the significance of a single chemistry chapter worth nine marks are highlighted, with detailed explanations on galvanic cells, non-restriction, and oxidation/reduction processes within electrochemical cells. The text emphasizes the use of elements like zinc and magnesium to prevent rusting, the significance of balancing reactions in cells, and the process of rusting in iron objects, along with the importance of galvanizing iron with zinc for protection.

Insights

  • Understanding the division of the chemistry chapter into three parts, focusing on the galvanic cell setup, non-restriction, and electrolyte cell sections, is crucial for mastering the material and scoring well on exams.
  • Highlighting the significance of balancing reactions in cells, utilizing elements like zinc and magnesium to prevent rusting, and the protective effect of galvanizing iron with zinc underscores the practical applications of electrochemistry in everyday life, from preventing corrosion to maintaining electricity during power outages.

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Recent questions

  • What is the importance of maintaining electricity at home?

    Maintaining electricity at home is crucial to prevent acid consumption, as discussed in the text. Without electricity, lead-acid accumulators in storage batteries may fail, leading to imbalances and potential hazards. Additionally, electricity is essential for non-spontaneous reactions like electrolysis, which require a power source to drive the process.

  • How is the chemistry chapter divided?

    The chemistry chapter discussed in the text is divided into three main parts: galvanic cell, applications, and electrolyte cell sections. Each part focuses on different aspects of electrochemical cells, such as the setup of galvanic cells, the functions of anode and cathode, and the process of oxidation and reduction within the cells.

  • What is the significance of Faraday's rule in electrolysis?

    Faraday's rule is crucial in electrolysis as it is used to calculate the quantity of deposit formed during the process. By utilizing the formula based on the current passing through the electrolyte and the time elapsed, one can determine the amount of substance deposited, making it a fundamental concept in understanding electrolytic reactions.

  • How do fuel cells work?

    Fuel cells, like those used in NASA rockets, operate by producing water as a byproduct, which prevents pollution. These cells generate electricity through chemical reactions between a fuel source and an oxidizing agent, offering a clean and efficient energy alternative. The text emphasizes the importance of fuel cells in sustainable energy solutions and their role in reducing environmental impact.

  • Why is balancing reactions important in cells?

    Balancing reactions in cells, such as galvanizing iron with zinc, is crucial to prevent rusting and protect materials from corrosion. By using elements like zinc and magnesium, one can create a protective layer that shields the underlying material from oxidation. This process is essential in maintaining the integrity and longevity of various objects, highlighting the significance of balanced reactions in electrochemical applications.

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Summary

00:00

"Chemistry: Electricity, Cells, and Standard Potential"

  • The text discusses the importance of maintaining electricity at home to prevent acid consumption.
  • It mentions the significance of a single chemistry chapter worth nine marks.
  • The text introduces Sumit as Mr. T and talks about a one-shot class 12th chemistry video.
  • It emphasizes the importance of understanding the syllabus and the division of the chapter into three parts.
  • The first part of the chapter focuses on the galvanic cell and its setup.
  • The second part highlights non-restriction, a crucial aspect of the chapter.
  • The chapter is divided into galvanic cell, applications, and electrolyte cell sections.
  • The text explains the process of oxidation and reduction within electrochemical cells.
  • It details the functions of anode and cathode within the cell setup.
  • The text concludes with a discussion on standard electrode potential and the representation of cells in IUPAC format.

33:35

Electrochemical Cell Setup and Reactions Explained

  • Sir Wink had a cell of wink and copper on A road, with copper on the cathode.
  • Zinc solid iron presentation is represented in this setup.
  • Single poles are used for the bridge side and the cathode side.
  • Zinc +2 ions are always around the bridge, while Zinc +2 is present.
  • Solid and aqua represent the physical state and phase change, respectively.
  • Reduction always occurs at the cathode, producing h2 gas.
  • Deposits start by going to the cathode, with a gram of electrons involved.
  • The solution will eat electrons with sticks to reduce and form h2 gas.
  • The reference electrode is standard, with the hydrogen electrode breaking its reaction.
  • The SRP determines the likelihood of oxidation or reduction, guiding the direction of the reaction.

01:20:18

"Electrolyte Conductivity: Formulas and Concepts Explained"

  • The first formula involves the beat equal to G multiplied by G star, with the date to remember being G * G*k.
  • The formula for length by area date is mentioned, with non-aaj well constant from cell.
  • Conductors will be placed and removed, along with connectivity being a crucial aspect.
  • Additive chemistry is discussed, emphasizing the importance of units and finding out D continuity.
  • Energy can be referred to as frequency, with conductance and continuity being interchangeable terms.
  • The reciprocal of resistance is highlighted as G date being Ohm Inverse or Simon.
  • The significance of connectivity and its impact on volume and ions is explained.
  • Molar conductance is introduced, focusing on the concentration of the solution and the formula for molarity.
  • The impact of dilution on strong and weak electrolytes is discussed, with the concept of alpha and concentration being crucial.
  • The increase in the number of ions due to dilution and its effect on conductivity is explained, emphasizing the importance of Lambda and the graph representation.

01:57:35

"Electrolysis: Calculating Deposits with Faraday's Rule"

  • Graphical lambda increases for stone and week
  • Beta graph shows sharp increase for the week and gradual increase for the stone
  • Graph allows calculation of lambda and infinity for strong electrolyte and per week electrolyte
  • Strong electrolyte data on stone available for extraction
  • Graphical extraction of lambda and infinity values for strong electrolyte and week electrolyte
  • Data from main lambda and infinity used to calculate dilutions
  • Extraction of substance for electrolyte to remove lambda, M, and infinity values
  • Electrolysis process explained, requiring electricity for non-spontaneous reactions
  • Faraday's rule used to calculate deposit quantity in electrolysis
  • Working formula for deposit quantity based on current and time passed

02:40:40

Battery Backup and Rust Prevention Techniques

  • Lead the storage battery if government electricity fails, using a lead acid accumulator with sulfuric acid to maintain balance and recharge when electricity returns.
  • Discuss the use of fuel cells, like those in NASA rockets, which produce water as a byproduct, preventing pollution, and explaining the process of rusting in iron objects.
  • Emphasize the importance of balancing reactions in cells, using elements like zinc and magnesium to prevent rusting, and the significance of galvanizing iron with zinc to protect it.
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