Chemistry · Class 12 · Chapter 2

Electrochemistry

12 lessons107 min3 simulations10 practice questions

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.

Also called: electrochemical cells · Nernst equation · conductance

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Lessons

12 lessons · 107 min

01Galvanic and electrolytic cellsNCERT §2.19 min 02Electrode potentials and the SHENCERT §2.2; §2.2.111 min1 sim 03The Nernst equationNCERT §2.310 min1 sim 04Cell potential, Gibbs energy and KNCERT §2.3.1; §2.3.27 min 05Conductivity of solutionsNCERT §2.4; §2.4.17 min 06Molar conductivity and dilutionNCERT §2.4.210 min1 sim 07Kohlrausch's lawNCERT §2.4.27 min 08Electrolysis and Faraday's lawsNCERT §2.57 min 09Products of electrolysisNCERT §2.5.16 min 10BatteriesNCERT §2.6; §2.6.1; §2.6.27 min 11Fuel cells and corrosionNCERT §2.7; §2.89 min 12Chapter reviewMust-know facts, traps and formulas17 min

Simulations

3 in this chapter

Which electrode is the anode, and what voltage do you get?In: Electrode potentials and the SHE How does concentration change a cell's voltage?In: The Nernst equation Why does molar conductivity rise on dilution?In: Molar conductivity and dilution