Ch 3 covers electrochemistry — electrochemical cells, EMF, Nernst equation, conductivity, Kohlrausch's law, electrolysis, Faraday's laws, batteries, fuel cells, and corrosion.
Galvanic (spontaneous, produces electricity): Zn|Zn²⁺||Cu²⁺|Cu. E°cell = E°cathode − E°anode. Nernst equation: E = E° − (RT/nF)ln Q = E° − (0.0592/n)log Q at 298K. ΔG° = −nFE°. Positive E°cell → spontaneous.
Conductance (G = 1/R), specific conductance (κ), molar conductivity (Λm = κ × 1000/c). Kohlrausch: Λ°m = sum of ionic conductivities. Electrolysis: Faraday's 1st law — mass deposited ∝ charge (m = ZIt). 2nd law — masses ∝ equivalent weights. 1 Faraday = 96485 C.
Download: https://ncert.nic.in/textbook/pdf/lech103.pdf | Part I: https://ncert.nic.in/textbook/pdf/lech1ps.zip
Galvanic cells convert chemical energy to electrical energy (spontaneous, ΔG < 0). Electrolytic cells convert electrical energy to chemical energy (non-spontaneous, need external voltage). In galvanic cells, anode is −ve; in electrolytic cells, anode is +ve.
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