Chemistry · Class 12 · Chapter 2
Electrochemistry
12 lessons 104 min 2 simulations
Electrochemistry links redox chemistry with electricity in both directions: a spontaneous redox reaction can push electrons through a wire (a galvanic cell), and an outside voltage can drive a reaction that would not go by itself (an electrolytic cell). The chapter measures electrode potentials against the hydrogen electrode, ties cell voltage to concentration (Nernst), to Gibbs energy and to equilibrium constants, then turns to how ionic solutions conduct, how much product a given charge makes (Faraday), and the batteries, fuel cells and corrosion that run on the same ideas.
What the exam asks
NEET asks for E°cell from a table of standard potentials, Nernst-equation numericals, ΔrG° = −nFE° and log K = nE°/0.059, conductivity and molar-conductivity conversions with the cell constant, Kohlrausch's law for Λ°m of weak electrolytes and their degree of dissociation, Faraday's-law mass calculations, which product forms in electrolysis, and the electrode reactions of the dry, mercury, lead storage and fuel cells. Marks go on sign conventions (anode is negative in a galvanic cell), unit slips between S cm² mol⁻¹ and S m² mol⁻¹, forgetting n in Nernst, and multiplying E° when a half-equation is doubled.
Lessons
12 lessons · 104 min
1Galvanic and electrolytic cellsNCERT §2.19 min2Electrode potentials and the SHENCERT §2.2; §2.2.18 min3The Nernst equationNCERT §2.310 min 1 sim4Cell potential, Gibbs energy and KNCERT §2.3.1; §2.3.27 min5Conductivity of solutionsNCERT §2.4; §2.4.17 min6Molar conductivity and dilutionNCERT §2.4.210 min 1 sim7Kohlrausch's lawNCERT §2.4.27 min8Electrolysis and Faraday's lawsNCERT §2.57 min9Products of electrolysisNCERT §2.5.16 min10BatteriesNCERT §2.6; §2.6.1; §2.6.27 min11Fuel cells and corrosionNCERT §2.7; §2.89 min12Chapter reviewMust-know facts, traps and formulas17 min