NCERT/Class 12/Chemistry/Electrochemistry

Electrochemistry

Class 12 · Chemistry

50 questions13 easy29 medium8 hard

Sample Questions

Q1.Kohlrausch's law of independent migration of ions states that:

  • AΛ°m = ν₊λ°₊ + ν₋λ°₋ (each ion contributes independently to Λ°m)
  • BConductivity depends only on cations
  • CAll ions have the same molar conductivity
  • DAnions don't contribute to conductivity

Q2.The electrochemical series (activity series) lists elements in order of:

  • ADecreasing standard reduction potential (most positive at top)
  • BIncreasing atomic number
  • CIncreasing reactivity
  • DAlphabetical order

Q3.One Faraday (F) is defined as:

  • AThe charge carried by one mole of electrons (96485 C/mol)
  • BThe charge of one electron (1.6 × 10⁻¹⁹ C)
  • CThe current of 1 ampere for 1 second
  • DThe charge needed to deposit 1 gram of any element

Q4.In electrolysis of aqueous CuSO₄ with copper electrodes, the cathode reaction is:

  • ACu²⁺ + 2e⁻ → Cu (copper is deposited)
  • B2H₂O → O₂ + 4H⁺ + 4e⁻
  • CSO₄²⁻ → SO₄ + 2e⁻
  • D2H⁺ + 2e⁻ → H₂

Q5.Which of the following is correct about standard electrode potential?

  • AMeasured relative to SHE, with 1 M concentration, 1 atm pressure at 25°C
  • BIt is an absolute value measured alone
  • CIt depends on the size of the electrode
  • DIt is always positive

Q6.This is a sample question to preview what you'll get in the full practice test...

  • A. Option one
  • B. Option two
  • C. Option three
  • D. Option four
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Concepts Covered

0.0592/nAC currentCuSO4 electrolysisDaniell cellDaniell cell calculationDebye-Hückel-Onsager equationEMF calculationF2 electrode potentialFaraday's constantFaraday's first lawFaraday's law calculationFaraday's second lawH2 productionKohlrausch's lawKohlrausch's law applicationKohlrausch's law calculationLeclanché dry cellNaCl molar conductivityNernst equationNernst equation at 25°CNernst equation at equilibriumSHE referenceWheatstone bridgeacetic acidammonium chlorideanode and cathodeanode oxidationanode productbattery electrolytebattery typescathode productcathode reactioncathodic depositioncathodic protectioncell EMFcell EMF = 0cell constantcell diagramcell notationcell reactioncharge calculationcharge of electronschemical and electrical energyconcentrationconcentration cellconcentration effectconductance and temperatureconductance measurementconductivityconductivity calculationconductivity relationshipcopper depositioncopper refiningcorrosioncorrosion inhibitorscorrosion preventiondegree of ionizationdirect electricity generationdischarge reactionelectrical neutralityelectrochemical processelectrochemical serieselectrochemistry definitionelectrode potentialelectrode reactionselectrolysiselectrolysis applicationelectrolysis of molten NaClelectrolytic solutionselectroplatingenergy conversionequilibrium constantequilibrium in cellsequivalent weightfuel cellgalvanic cellgalvanic cellsgalvanic vs electrolytic cellhydrogen electrode potentialhydrogen fuel cellindirect calculationinfinite dilutionion mobilityionic circuitionic conductivitieslead storage batterylimiting ionic conductivitiesmass calculationmass depositionmercury cellmolar conductivitymolar conductivity and dilutionnon-rechargeableoxidation reductionoxidizing agentoxidizing agentspH effectprimary batteryprimary vs secondary batteryprotective layerreaction quotientrechargeabilityreference electroderesistanceresistivityrusting mechanismsacrificial anodesalt bridgesilver depositionsimplified formspecific resistancespontaneityspontaneous vs non-spontaneousstandard EMFstandard conditionsstandard electrode potentialstandard hydrogen electrodestandard reduction potentialstrong electrolyte conductivitystrong electrolytesstrongest oxidizing agentviscositywater electrolysisweak electrolyte conductivityweak electrolytesΔG° and E° relationshipΔG°-K-E° relationshipΛm/Λ°mΛ°m calculation√c dependence

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