Class 12 Chemistry - ODISHA
Electrochemistry
Electrochemistry is a crucial branch of physical chemistry that explores the relationship between electrical energy and chemical changes. For Class 12 students under the Odisha Board (BSE), this chapter covers essential topics such as electrochemical cells, galvanic cells, Nernst equation, electrolytic conductance, Kohlrausch's law, and commercial batteries like fuel cells. Mastery of this chapter is vital for board exams as it features a mix of conceptual reasoning and numerical problems. Scoring well here depends on a clear understanding of oxidation-reduction reactions, standard electrode potentials, and precise application of mathematical formulas.
Start Learning FreeKey Concepts
Electrochemical Cells
Devices that convert chemical energy into electrical energy (galvanic cells) or electrical energy into chemical energy (electrolytic cells).
Nernst Equation
A mathematical equation used to calculate the electrode potential of a cell at any given concentration and temperature.
Molar Conductivity
The conducting power of all the ions produced by dissolving one mole of an electrolyte in a solution of a given volume.
Kohlrausch's Law of Independent Migration of Ions
States that the limiting molar conductivity of an electrolyte is the sum of the individual contributions of its anions and cations.
Faraday's Laws of Electrolysis
Quantitative laws that relate the amount of chemical change during electrolysis to the quantity of electricity passed through the electrolyte.
Important Formulas
Board Exam Info
In the Odisha (BSE) Class 12 Chemistry board exam, Electrochemistry typically carries around 5 to 7 marks. Questions frequently include numerical problems based on the Nernst equation, Kohlrausch's law, and Faraday's laws, alongside short answer questions on rusting, salt bridge functions, and working principles of primary and secondary cells.
Frequently Asked Questions
What is the function of a salt bridge in a galvanic cell?
A salt bridge completes the electrical circuit and maintains electrical neutrality in the two half-cells by preventing the accumulation of charges.
Why does the molar conductivity of a weak electrolyte increase sharply on dilution?
Dilution increases the degree of dissociation of weak electrolytes, which increases the total number of ions free to carry current in the solution.
Can we store copper sulfate solution in a zinc pot?
No, because zinc is more reactive than copper (has a lower standard reduction potential) and will displace copper from the solution, creating holes in the zinc pot.
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