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Electro Chemistry ONESHOT Marathon | Class 12 | CBSE 2024 | Haritha Ma'am

Vedantu Master Tamil・21 minutes read

Practicing questions builds exam confidence, while understanding oxidation, reduction, and electrochemical reactions is crucial. Faraday's laws dictate the relationship between deposited substance weight and current quantity, with key formulas determining dissociation percentages in electrolytes.

Insights

  • Practice questions are essential for exam preparation as they build confidence in facing exams by solidifying understanding and application of concepts, making the test-taking process smoother and more manageable.
  • Understanding electrochemical reactions involves recognizing the roles of the anode and cathode, defining oxidation and reduction, calculating cell potential, and utilizing equations like the Nernst equation to determine equilibrium constants, highlighting the intricate relationship between standard cell potential, equilibrium constant, and standard Gibbs free energy in electrochemistry.

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Recent questions

  • What is the significance of oxidation and reduction in electrochemical reactions?

    Oxidation involves the loss of electrons, while reduction involves the gain of electrons. These processes are crucial in electrochemical reactions as they determine the flow of electrons between the anode and cathode, leading to the generation of electrical energy.

  • How is cell potential calculated for galvanic cells?

    The cell potential for galvanic cells is calculated by finding the difference between the cathode and anode potentials. This potential difference drives the flow of electrons through the external circuit, generating electrical energy in the process.

  • What is the Nernst equation used for in chemistry?

    The Nernst equation is utilized to calculate the equilibrium constant for a given reaction. By considering the concentrations of reactants and products, this equation provides insights into the spontaneity and direction of chemical reactions.

  • How are standard cell potential and equilibrium constant related?

    Standard cell potential, equilibrium constant, and standard Gibbs free energy are interconnected in electrochemical reactions. These parameters provide information about the feasibility and direction of reactions, shedding light on the thermodynamic aspects of chemical processes.

  • What do Faraday's laws state about electrolysis?

    Faraday's laws establish that the weight of a substance deposited during electrolysis is directly proportional to the quantity of current passed. Additionally, the second law specifies that the number of equivalents deposited corresponds to the number of Faradays passed, elucidating the relationship between electricity and chemical transformations.

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Summary

00:00

"Exam Confidence, Oxidation-Reduction, Nernst Equation Relationship"

  • Understanding the importance of practicing questions for building confidence in facing exams.
  • Recognizing the processes of oxidation and reduction in electrochemical reactions.
  • Identifying the anode as the site of oxidation and the cathode as the site of reduction.
  • Defining oxidation as the loss of electrons and reduction as the gain of electrons.
  • Explaining the significance of oxidation state changes in electrochemical reactions.
  • Describing the conversion of half-cell reactions in standard notation.
  • Calculating the cell potential for galvanic cells using the difference between cathode and anode potentials.
  • Determining the strongest oxidizing agent based on reduction potentials.
  • Utilizing the Nernst equation to calculate the equilibrium constant for a given reaction.
  • Understanding the relationship between standard cell potential, equilibrium constant, and standard Gibbs free energy.

39:42

Calculating Degree of Dissociation in Electrolytes

  • To calculate the percentage of degree of dissociation, use the given data of normality as 0.0n for ammonium hydroxide, M conductance as 9.6, and molar conductance at infinite dilution as 272.
  • The formula to find the percentage of degree of dissociation is alpha = molar conductance by conductivity at infinite dilution into 100, resulting in a value of 0.353 into 100.
  • On dilution, the molar conductivity of a strong electrolyte increases, as seen with the example of CH3CO with a molar conductivity of 48 CM s per 4 Simon cm square per mole and molar conductivity at infinite dilution of 344 Simon cm square per mole.
  • The percentage dissociation of acetic acid can be calculated using the formula alpha = conductivity by conductivity at infinite dilution into 100, yielding a final answer of 13.9%.
  • The molar conductivity at infinite dilution for strong electrolytes can be determined by the conductivity of individual ions, applicable only for strong electrolytes.
  • During electrolysis, sodium chloride forms sodium and chlorine gas, with the positive ion going to the cathode and the negative ion to the anode.
  • Faraday's laws state that the weight of a substance deposited during electrolysis is directly proportional to the quantity of current passed, with the second law specifying that the number of equivalents deposited is the same as the number of Faradays passed.
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