{"id":7071,"date":"2026-10-20T05:30:04","date_gmt":"2026-10-20T05:30:04","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=7071"},"modified":"2026-10-20T05:30:05","modified_gmt":"2026-10-20T05:30:05","slug":"electrochemistry-neet-pyq-analysis","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/electrochemistry-neet-pyq-analysis\/","title":{"rendered":"Electrochemistry NEET PYQ Analysis: Nernst Equation, Conductance and Faraday&#8217;s Laws"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\"><strong>Quick answer:<\/strong> An electrochemistry NEET PYQ analysis shows that NTA asks about two questions a year from this chapter, and most are short numericals from five areas: E\u00b0cell and the electrochemical series, the Nernst equation (including the hydrogen electrode and the equilibrium constant), the link between \u0394G\u00b0 and E\u00b0cell, conductance with Kohlrausch&#8217;s law, and Faraday&#8217;s laws of electrolysis. A small formula set solves almost every past question.<\/p>\n\n\n\n<figure class=\"wp-block-image size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"432\" src=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell-1024x432.jpg\" alt=\"Electrochemistry NEET PYQ analysis showing a Daniell cell with zinc and copper beakers, a salt bridge and a voltmeter\" class=\"wp-image-7072\" srcset=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell-1024x432.jpg 1024w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell-300x127.jpg 300w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell-768x324.jpg 768w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell-1536x648.jpg 1536w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Electrochemistry-NEET-PYQ-Analysis-Daniell-Cell.jpg 2048w\" sizes=\"auto, (max-width: 1024px) 100vw, 1024px\" \/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">This guide breaks down what NTA repeats, the formulas you must know and solved PYQ-pattern numericals. For the full Physical Chemistry plan, see our <a href=\"https:\/\/ksquareinstitute.in\/blog\/physical-chemistry-for-neet-2027\">NEET 2027 Physical Chemistry guide<\/a>.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Want to test yourself first? <a href=\"https:\/\/ksquareinstitute.com\/questions\/neet-previous-year-questions\/chemistry\/electrochemistry\/questions\/\" target=\"_blank\" rel=\"noopener\">Solve the Electrochemistry PYQs<\/a> for free, then use this guide to fix the gaps.<\/p>\n\n\n\n<div class=\"wp-block-rank-math-toc-block\" id=\"rank-math-toc\"><h2>Table of Contents<\/h2><nav><ul><li><a href=\"#why-electrochemistry-is-worth-mastering\">Why Electrochemistry Is Worth Mastering<\/a><\/li><li><a href=\"#electrochemistry-neet-pyq-analysis-what-nta-repeats\">Electrochemistry NEET PYQ Analysis: What NTA Repeats<\/a><\/li><li><a href=\"#galvanic-cells-and-e-cell\">Galvanic Cells and E\u00b0cell<\/a><\/li><li><a href=\"#the-nernst-equation\">The Nernst Equation<\/a><\/li><li><a href=\"#gibbs-energy-and-cell-potential\">Gibbs Energy and Cell Potential<\/a><\/li><li><a href=\"#conductance-of-electrolytic-solutions\">Conductance of Electrolytic Solutions<\/a><\/li><li><a href=\"#kohlrauschs-law\">Kohlrausch&#8217;s Law<\/a><\/li><li><a href=\"#faradays-laws-and-products-of-electrolysis\">Faraday&#8217;s Laws and Products of Electrolysis<\/a><\/li><li><a href=\"#batteries-fuel-cells-and-corrosion\">Batteries, Fuel Cells and Corrosion<\/a><\/li><li><a href=\"#worked-pyq-pattern-questions\">Worked PYQ-Pattern Questions<\/a><\/li><li><a href=\"#common-traps-in-this-chapter\">Common Traps in This Chapter<\/a><\/li><li><a href=\"#practise-every-electrochemistry-pyq\">Practise Every Electrochemistry PYQ<\/a><\/li><li><a href=\"#conclusion\">Conclusion<\/a><\/li><li><a href=\"#\u2753-faq\">FAQ<\/a><\/li><\/ul><\/nav><\/div>\n\n\n\n<h2 id=\"why-electrochemistry-is-worth-mastering\" class=\"wp-block-heading\">Why Electrochemistry Is Worth Mastering<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">The chapter looks heavy, but its questions use the same handful of formulas year after year. Once you can apply E\u00b0cell, E = E\u00b0 \u2212 (0.059\/n) log Q, \u0394G\u00b0 = \u2212nFE\u00b0 and m = ZIt quickly, most questions take under a minute. For chapter notes, use our <a href=\"https:\/\/ksquareinstitute.in\/blog\/electrochemistry-class-12-notes-pdf\">Electrochemistry class 12 notes<\/a>, and to see where it sits among other chapters, check the <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-2027-syllabus-chapter-weightage\">NEET 2027 chapter weightage<\/a>.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Electrochemistry builds on oxidation numbers and electrode reactions, so our <a href=\"https:\/\/ksquareinstitute.in\/blog\/redox-reactions-neet-pyq-analysis\">Redox Reactions PYQ analysis<\/a> is the right warm-up. Rate and equilibrium ideas also overlap with our <a href=\"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-neet-pyq-analysis\">Chemical Kinetics PYQ analysis<\/a>.<\/p>\n\n\n\n<h2 id=\"electrochemistry-neet-pyq-analysis-what-nta-repeats\" class=\"wp-block-heading\">Electrochemistry NEET PYQ Analysis: What NTA Repeats<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">When you sort the past NEET chemistry PYQs from this chapter, five question types cover nearly everything.<\/p>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Question type<\/th><th class=\"has-text-align-center\" data-align=\"center\">Frequency<\/th><th>What it tests<\/th><\/tr><\/thead><tbody><tr><td>E\u00b0cell and electrochemical series<\/td><td class=\"has-text-align-center\" data-align=\"center\">Most frequent<\/td><td>Cell potential, strongest oxidising or reducing agent, feasibility<\/td><\/tr><tr><td>Nernst calculations<\/td><td class=\"has-text-align-center\" data-align=\"center\">Very frequent<\/td><td>Electrode and cell potential at given concentrations, pH of a hydrogen electrode, log K<\/td><\/tr><tr><td>\u0394G\u00b0 and E\u00b0cell<\/td><td class=\"has-text-align-center\" data-align=\"center\">Very frequent<\/td><td>\u0394G\u00b0 = \u2212nFE\u00b0cell, spontaneity<\/td><\/tr><tr><td>Conductance and \u039b\u00b0m<\/td><td class=\"has-text-align-center\" data-align=\"center\">Very frequent<\/td><td>Cell constant, molar conductivity, \u039b\u00b0m of weak electrolytes, degree of dissociation<\/td><\/tr><tr><td>Electrolysis calculations<\/td><td class=\"has-text-align-center\" data-align=\"center\">Regular<\/td><td>Mass deposited, charge needed, products at each electrode<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">For a quick warm-up, try these <a href=\"https:\/\/ksquareinstitute.in\/blog\/top-5-electrochemistry-questions\">five quick electrochemistry questions<\/a>.<\/p>\n\n\n\n<h2 id=\"galvanic-cells-and-e-cell\" class=\"wp-block-heading\">Galvanic Cells and E\u00b0cell<\/h2>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Feature<\/th><th>Galvanic (electrochemical) cell<\/th><th>Electrolytic cell<\/th><\/tr><\/thead><tbody><tr><td>Energy change<\/td><td>Chemical \u2192 electrical<\/td><td>Electrical \u2192 chemical<\/td><\/tr><tr><td>Reaction<\/td><td>Spontaneous<\/td><td>Non-spontaneous<\/td><\/tr><tr><td>Anode<\/td><td>Oxidation, negative<\/td><td>Oxidation, positive<\/td><\/tr><tr><td>Cathode<\/td><td>Reduction, positive<\/td><td>Reduction, negative<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>E\u00b0cell = E\u00b0cathode \u2212 E\u00b0anode<\/strong> (both as standard reduction potentials)<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>Daniell cell<\/strong>, Zn | Zn\u00b2\u207a || Cu\u00b2\u207a | Cu, has E\u00b0cell = 0.34 \u2212 (\u22120.76) = <strong>1.10 V<\/strong>.<\/li>\n\n\n\n<li>The standard hydrogen electrode (SHE) is assigned <strong>0.00 V<\/strong>.<\/li>\n\n\n\n<li>A <strong>higher reduction potential<\/strong> means a stronger oxidising agent. <strong>F\u2082<\/strong> is the strongest oxidising agent (E\u00b0 = +2.87 V), and <strong>Li<\/strong> is the strongest reducing agent (E\u00b0 = \u22123.05 V).<\/li>\n\n\n\n<li>A reaction is feasible when E\u00b0cell is positive.<\/li>\n<\/ul>\n\n\n\n<h2 id=\"the-nernst-equation\" class=\"wp-block-heading\">The Nernst Equation<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">At 298 K:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>E = E\u00b0 \u2212 (0.059\/n) log Q<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Situation<\/th><th>Form to use<\/th><\/tr><\/thead><tbody><tr><td>Metal electrode, M\u207f\u207a + ne\u207b \u2192 M<\/td><td>E = E\u00b0 \u2212 (0.059\/n) log (1\/[M\u207f\u207a])<\/td><\/tr><tr><td>Hydrogen electrode at 1 bar<\/td><td>E = \u22120.059 pH<\/td><\/tr><tr><td>Daniell cell<\/td><td>E = E\u00b0cell \u2212 (0.059\/2) log ([Zn\u00b2\u207a]\/[Cu\u00b2\u207a])<\/td><\/tr><tr><td>At equilibrium (E = 0)<\/td><td>E\u00b0cell = (0.059\/n) log Kc<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 id=\"gibbs-energy-and-cell-potential\" class=\"wp-block-heading\">Gibbs Energy and Cell Potential<\/h2>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Relation<\/th><th>Meaning<\/th><\/tr><\/thead><tbody><tr><td>\u0394G\u00b0 = \u2212nFE\u00b0cell<\/td><td>Positive E\u00b0cell gives negative \u0394G\u00b0, so the reaction is spontaneous<\/td><\/tr><tr><td>\u0394G\u00b0 = \u22122.303RT log K<\/td><td>Links Gibbs energy to the equilibrium constant<\/td><\/tr><tr><td>F = 96,487 C mol\u207b\u00b9 (\u2248 96,500)<\/td><td>Charge on one mole of electrons<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 id=\"conductance-of-electrolytic-solutions\" class=\"wp-block-heading\">Conductance of Electrolytic Solutions<\/h2>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Quantity<\/th><th class=\"has-text-align-center\" data-align=\"center\">Formula<\/th><th class=\"has-text-align-center\" data-align=\"center\">Unit<\/th><\/tr><\/thead><tbody><tr><td>Cell constant (G*)<\/td><td class=\"has-text-align-center\" data-align=\"center\">l\/A<\/td><td class=\"has-text-align-center\" data-align=\"center\">cm\u207b\u00b9<\/td><\/tr><tr><td>Conductivity (\u03ba)<\/td><td class=\"has-text-align-center\" data-align=\"center\">G \u00d7 G*<\/td><td class=\"has-text-align-center\" data-align=\"center\">S cm\u207b\u00b9<\/td><\/tr><tr><td>Molar conductivity (\u039bm)<\/td><td class=\"has-text-align-center\" data-align=\"center\">(\u03ba \u00d7 1000)\/M<\/td><td class=\"has-text-align-center\" data-align=\"center\">S cm\u00b2 mol\u207b\u00b9<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Facts NTA turns into statements:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>On dilution, <strong>conductivity (\u03ba) decreases<\/strong> because there are fewer ions per unit volume, but <strong>molar conductivity (\u039bm) increases<\/strong>.<\/li>\n\n\n\n<li>For <strong>strong electrolytes<\/strong>, \u039bm = \u039b\u00b0m \u2212 A\u221ac (the Debye\u2013H\u00fcckel\u2013Onsager equation), so a plot of \u039bm vs \u221ac is a straight line.<\/li>\n\n\n\n<li>For <strong>weak electrolytes<\/strong>, \u039bm rises steeply at low concentration, so \u039b\u00b0m cannot be found by extrapolation and must be built from ionic values instead.<\/li>\n<\/ul>\n\n\n\n<h2 id=\"kohlrauschs-law\" class=\"wp-block-heading\">Kohlrausch&#8217;s Law<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>\u039b\u00b0m = \u03bd\u208a\u03bb\u00b0\u208a + \u03bd\u208b\u03bb\u00b0\u208b<\/strong>: the limiting molar conductivity of an electrolyte is the sum of the limiting molar conductivities of its ions.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Uses:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Finding \u039b\u00b0m of a weak electrolyte: \u039b\u00b0m(CH\u2083COOH) = \u039b\u00b0m(CH\u2083COONa) + \u039b\u00b0m(HCl) \u2212 \u039b\u00b0m(NaCl)<\/li>\n\n\n\n<li>Degree of dissociation: <strong>\u03b1 = \u039bm \/ \u039b\u00b0m<\/strong><\/li>\n\n\n\n<li>Dissociation constant: <strong>Ka = c\u03b1\u00b2 \/ (1 \u2212 \u03b1)<\/strong><\/li>\n<\/ul>\n\n\n\n<h2 id=\"faradays-laws-and-products-of-electrolysis\" class=\"wp-block-heading\">Faraday&#8217;s Laws and Products of Electrolysis<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>First law:<\/strong> m = Z \u00d7 I \u00d7 t = (M \/ nF) \u00d7 I \u00d7 t<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Second law:<\/strong> when the same charge passes through different electrolytes, the masses deposited are proportional to their equivalent weights.<\/p>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-white-background-color has-background has-border-color has-black-border-color\" style=\"border-width:2px\"><thead><tr><th>Electrolysis of<\/th><th class=\"has-text-align-center\" data-align=\"center\">At the cathode<\/th><th>At the anode<\/th><\/tr><\/thead><tbody><tr><td>Molten NaCl<\/td><td class=\"has-text-align-center\" data-align=\"center\">Na<\/td><td>Cl\u2082<\/td><\/tr><tr><td>Aqueous NaCl<\/td><td class=\"has-text-align-center\" data-align=\"center\">H\u2082<\/td><td>Cl\u2082 (because of overpotential for O\u2082)<\/td><\/tr><tr><td>Dilute H\u2082SO\u2084<\/td><td class=\"has-text-align-center\" data-align=\"center\">H\u2082<\/td><td>O\u2082<\/td><\/tr><tr><td>Concentrated H\u2082SO\u2084<\/td><td class=\"has-text-align-center\" data-align=\"center\">H\u2082<\/td><td>S\u2082O\u2088\u00b2\u207b (peroxodisulphate)<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 id=\"batteries-fuel-cells-and-corrosion\" class=\"wp-block-heading\">Batteries, Fuel Cells and Corrosion<\/h2>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Dry (Leclanch\u00e9) cell:<\/strong> about 1.5 V.<\/li>\n\n\n\n<li><strong>Mercury cell:<\/strong> about 1.35 V, stays constant over its life because no ions are involved in the overall reaction.<\/li>\n\n\n\n<li><strong>Lead storage battery:<\/strong> on discharge, Pb + PbO\u2082 + 2H\u2082SO\u2084 \u2192 2PbSO\u2084 + 2H\u2082O.<\/li>\n\n\n\n<li><strong>H\u2082\u2013O\u2082 fuel cell:<\/strong> used in the Apollo space programme; the water it produced was used for drinking.<\/li>\n\n\n\n<li><strong>Rusting<\/strong> is electrochemical: iron is oxidised at the anode (Fe \u2192 Fe\u00b2\u207a), oxygen is reduced at the cathode, and the rust is hydrated ferric oxide, Fe\u2082O\u2083\u00b7xH\u2082O.<\/li>\n<\/ul>\n\n\n\n<h2 id=\"worked-pyq-pattern-questions\" class=\"wp-block-heading\">Worked PYQ-Pattern Questions<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q1. E\u00b0 for Cu\u00b2\u207a\/Cu is +0.34 V and for Zn\u00b2\u207a\/Zn is \u22120.76 V. Find E\u00b0cell for the Daniell cell.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">E\u00b0cell = E\u00b0cathode \u2212 E\u00b0anode = 0.34 \u2212 (\u22120.76)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 1.10 V.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q2. What is the potential of a hydrogen electrode in a solution of pH 10 at 298 K?<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">E = \u22120.059 \u00d7 pH = \u22120.059 \u00d7 10<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: \u22120.59 V.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q3. For a cell reaction with n = 2 and E\u00b0cell = 1.10 V, find \u0394G\u00b0 (F = 96,500 C mol\u207b\u00b9).<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u0394G\u00b0 = \u2212nFE\u00b0cell = \u22122 \u00d7 96,500 \u00d7 1.10 = \u2212212,300 J mol\u207b\u00b9<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: About \u2212212.3 kJ mol\u207b\u00b9.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q4. A current of 2 A is passed through CuSO\u2084 solution for 965 seconds. What mass of copper is deposited? (Cu = 63.5 g mol\u207b\u00b9)<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Q = I \u00d7 t = 2 \u00d7 965 = 1930 C = 1930\/96,500 = 0.02 F. Cu\u00b2\u207a needs 2 F per mole, so moles of Cu = 0.01.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 0.635 g.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q5. \u039b\u00b0m values (S cm\u00b2 mol\u207b\u00b9) are CH\u2083COONa = 91.0, HCl = 426.2 and NaCl = 126.5. Find \u039b\u00b0m of acetic acid.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u039b\u00b0m(CH\u2083COOH) = 91.0 + 426.2 \u2212 126.5<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 390.7 S cm\u00b2 mol\u207b\u00b9.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q6. Which of these is the strongest reducing agent?<\/strong> (a) Li (b) Na (c) K (d) Zn<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: (a) Li.<\/strong> It has the most negative standard reduction potential (\u22123.05 V).<\/p>\n\n\n\n<h2 id=\"common-traps-in-this-chapter\" class=\"wp-block-heading\">Common Traps in This Chapter<\/h2>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Using E\u00b0anode + E\u00b0cathode instead of E\u00b0cathode \u2212 E\u00b0anode<\/li>\n\n\n\n<li>Saying conductivity increases on dilution (it is molar conductivity that increases)<\/li>\n\n\n\n<li>Trying to find \u039b\u00b0m of a weak electrolyte by extrapolating the \u039bm vs \u221ac graph<\/li>\n\n\n\n<li>Forgetting n (the number of electrons) in the Nernst expression or in \u0394G\u00b0 = \u2212nFE\u00b0<\/li>\n\n\n\n<li>Writing O\u2082 instead of Cl\u2082 at the anode for aqueous NaCl<\/li>\n\n\n\n<li>Calling the anode positive in a galvanic cell<\/li>\n<\/ul>\n\n\n\n<h2 id=\"practise-every-electrochemistry-pyq\" class=\"wp-block-heading\">Practise Every Electrochemistry PYQ<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">This electrochemistry NEET PYQ analysis shows you where the marks are. Solving real past questions makes the formulas automatic. Every Electrochemistry previous year question is available chapter-wise, free:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\ud83d\udc49 <strong><a href=\"https:\/\/ksquareinstitute.com\/questions\/neet-previous-year-questions\/chemistry\/electrochemistry\/\" target=\"_blank\" rel=\"noopener\">Solve all Electrochemistry NEET PYQs<\/a><\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Keep the formula tables beside you for the first round, then solve the second round without them.<\/p>\n\n\n\n<h2 id=\"conclusion\" class=\"wp-block-heading\">Conclusion<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Electrochemistry rewards practice more than reading. Use this electrochemistry NEET PYQ analysis to master E\u00b0cell and the electrochemical series, the Nernst equation, \u0394G\u00b0 = \u2212nFE\u00b0, conductance with Kohlrausch&#8217;s law and Faraday&#8217;s laws. Then solve the past numericals until each one takes under a minute.<\/p>\n\n\n\n<h2 id=\"\u2753-faq\" class=\"wp-block-heading\">\u2753 FAQ<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: How many questions come from Electrochemistry in NEET?<\/strong> A: Usually about two questions a year, mostly short numericals on cell potential, conductance or electrolysis.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: What is the most important topic in Electrochemistry for NEET?<\/strong> A: E\u00b0cell with the electrochemical series and the Nernst equation are the most tested, followed by conductance and electrolysis.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: Why does molar conductivity increase on dilution?<\/strong> A: Molar conductivity is the conductance of all the ions from one mole of electrolyte. On dilution, the ions move more freely, and weak electrolytes dissociate more, so \u039bm increases even though conductivity (\u03ba) decreases.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: What is the potential of a hydrogen electrode in terms of pH?<\/strong> A: At 298 K and 1 bar, E = \u22120.059 pH.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: How much charge deposits one mole of aluminium from Al\u00b3\u207a?<\/strong> A: Three faradays, about 2,89,500 C, because each Al\u00b3\u207a ion needs three electrons.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: Where can I practise Electrochemistry NEET PYQs for free?<\/strong> A: You can solve every Electrochemistry previous year question chapter-wise for free using the practice links in this article.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Quick answer: An electrochemistry NEET PYQ analysis shows that NTA asks about two questions a year from this chapter, and most are short numericals from five areas: E\u00b0cell and the electrochemical series, the Nernst equation (including the hydrogen electrode and the equilibrium constant), the link between \u0394G\u00b0 and E\u00b0cell, conductance with Kohlrausch&#8217;s law, and Faraday&#8217;s [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":7072,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[8,69,2],"tags":[2820,4293,3539,3543,4294,4292,3541,7,4008,24,2328,3538,2322],"class_list":["post-7071","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-study-tips","category-chemistry","category-neet","tag-class-12-chemistry","tag-electrochemical-series","tag-electrochemistry","tag-faradays-laws","tag-galvanic-cell","tag-kohlrauschs-law","tag-molar-conductivity","tag-neet-2027","tag-neet-chapter-wise-pyq","tag-neet-chemistry","tag-neet-pyq","tag-nernst-equation","tag-physical-chemistry"],"_links":{"self":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/7071","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/comments?post=7071"}],"version-history":[{"count":1,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/7071\/revisions"}],"predecessor-version":[{"id":7073,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/7071\/revisions\/7073"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media\/7072"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=7071"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=7071"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=7071"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}