{"id":6978,"date":"2026-10-16T07:43:54","date_gmt":"2026-10-16T07:43:54","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=6978"},"modified":"2026-10-16T07:43:55","modified_gmt":"2026-10-16T07:43:55","slug":"chemical-kinetics-neet-pyq-analysis","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-neet-pyq-analysis\/","title":{"rendered":"Chemical Kinetics NEET PYQ Analysis: Order, Half-Life and Arrhenius Patterns"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\"><strong>Quick answer:<\/strong> A chemical kinetics NEET PYQ analysis shows that NTA asks about two questions a year from this chapter, and most are short numericals from four areas: the Arrhenius equation and activation energy, first order reaction half-life and time calculations, finding order from units of the rate constant or rate data, and the relation between rates of different species. The same formulas solve 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\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab-1024x432.jpg\" alt=\"Chemical kinetics NEET PYQ analysis showing flasks changing colour over time beside a stopwatch\" class=\"wp-image-6979\" srcset=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab-1024x432.jpg 1024w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab-300x127.jpg 300w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab-768x324.jpg 768w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab-1536x648.jpg 1536w, https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/10\/Chemical-Kinetics-NEET-PYQ-Analysis-Reaction-Rate-Lab.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 and graphs 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\/chemical-kinetics\/questions\/\" target=\"_blank\" rel=\"noopener\"><strong>Solve the Chemical Kinetics PYQs<\/strong><\/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-chemical-kinetics-is-a-high-return-chapter\">Why Chemical Kinetics Is a High-Return Chapter<\/a><\/li><li><a href=\"#chemical-kinetics-neet-pyq-analysis-what-nta-repeats\">Chemical Kinetics NEET PYQ Analysis: What NTA Repeats<\/a><\/li><li><a href=\"#rate-of-reaction-and-rate-expressions\">Rate of Reaction and Rate Expressions<\/a><\/li><li><a href=\"#order-vs-molecularity\">Order vs Molecularity<\/a><\/li><li><a href=\"#units-of-the-rate-constant\">Units of the Rate Constant<\/a><\/li><li><a href=\"#zero-and-first-order-the-formula-table\">Zero and First Order: The Formula Table<\/a><\/li><li><a href=\"#the-arrhenius-equation\">The Arrhenius Equation<\/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-chemical-kinetics-pyq\">Practise Every Chemical Kinetics PYQ<\/a><\/li><li><a href=\"#conclusion\">Conclusion<\/a><\/li><li><a href=\"#faq\">FAQ<\/a><\/li><\/ul><\/nav><\/div>\n\n\n\n<h2 id=\"why-chemical-kinetics-is-a-high-return-chapter\" class=\"wp-block-heading\">Why Chemical Kinetics Is a High-Return Chapter<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">The chapter has a small formula set and fixed question types, so a few hours of practice can secure its marks. If you want the concepts explained from scratch first, read our <a href=\"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-for-neet-2027\">Chemical Kinetics study guide<\/a> and our <a href=\"https:\/\/ksquareinstitute.in\/blog\/chemical-kinetics-class-12-notes-pdf\">Chemical Kinetics class 12 notes<\/a>. 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\">Students often confuse kinetics with equilibrium: kinetics tells you how fast a reaction goes, equilibrium tells you how far. Our <a href=\"https:\/\/ksquareinstitute.in\/blog\/equilibrium-neet-pyq-analysis\">Equilibrium PYQ analysis<\/a> covers the other half.<\/p>\n\n\n\n<h2 id=\"chemical-kinetics-neet-pyq-analysis-what-nta-repeats\" class=\"wp-block-heading\">Chemical Kinetics 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>Frequency<\/th><th>What it tests<\/th><\/tr><\/thead><tbody><tr><td>Arrhenius equation and activation energy<\/td><td>Most frequent<\/td><td>Two-temperature calculations, ln k vs 1\/T graph, effect of catalyst<\/td><\/tr><tr><td>First order reaction<\/td><td>Very frequent<\/td><td>Half-life, time for a given fraction, integrated rate law<\/td><\/tr><tr><td>Order from units or rate data<\/td><td>Very frequent<\/td><td>Units of the rate constant, method of initial rates<\/td><\/tr><tr><td>Zero order reaction<\/td><td>Regular<\/td><td>Integrated law, half-life, graphs<\/td><\/tr><tr><td>Rate expressions and molecularity<\/td><td>Regular<\/td><td>Relating rates of reactants and products, order vs molecularity<\/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-chemical-kinetics-questions\">five quick chemical kinetics questions<\/a>.<\/p>\n\n\n\n<h2 id=\"rate-of-reaction-and-rate-expressions\" class=\"wp-block-heading\">Rate of Reaction and Rate Expressions<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">For a reaction aA + bB \u2192 cC + dD:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Rate = \u2212(1\/a) d[A]\/dt = \u2212(1\/b) d[B]\/dt = +(1\/c) d[C]\/dt = +(1\/d) d[D]\/dt<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Example: for 2N\u2082O\u2085 \u2192 4NO\u2082 + O\u2082,<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u2212(1\/2) d[N\u2082O\u2085]\/dt = (1\/4) d[NO\u2082]\/dt = d[O\u2082]\/dt<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">NTA often gives one rate and asks for another, so divide each rate by its coefficient.<\/p>\n\n\n\n<h2 id=\"order-vs-molecularity\" class=\"wp-block-heading\">Order vs Molecularity<\/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>Order<\/th><th>Molecularity<\/th><\/tr><\/thead><tbody><tr><td>Defined as<\/td><td>Sum of powers of concentration in the experimental rate law<\/td><td>Number of species colliding in an elementary step<\/td><\/tr><tr><td>Found by<\/td><td>Experiment<\/td><td>Theory (from the mechanism)<\/td><\/tr><tr><td>Can be zero or fractional?<\/td><td>Yes<\/td><td>No, always a whole number (1, 2 or rarely 3)<\/td><\/tr><tr><td>Applies to<\/td><td>Elementary and complex reactions<\/td><td>Elementary reactions only<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">For a complex reaction, the <strong>slowest step is the rate-determining step<\/strong>, and its molecularity decides the order.<\/p>\n\n\n\n<h2 id=\"units-of-the-rate-constant\" class=\"wp-block-heading\">Units of the Rate Constant<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">General formula: <strong>units of k = (mol L\u207b\u00b9)^(1 \u2212 n) s\u207b\u00b9<\/strong>, where n is the order.<\/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>Order<\/th><th>Units of rate constant<\/th><\/tr><\/thead><tbody><tr><td>Zero<\/td><td>mol L\u207b\u00b9 s\u207b\u00b9<\/td><\/tr><tr><td>First<\/td><td>s\u207b\u00b9<\/td><\/tr><tr><td>Second<\/td><td>L mol\u207b\u00b9 s\u207b\u00b9<\/td><\/tr><tr><td>Third<\/td><td>L\u00b2 mol\u207b\u00b2 s\u207b\u00b9<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 id=\"zero-and-first-order-the-formula-table\" class=\"wp-block-heading\">Zero and First Order: The Formula Table<\/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>Zero order<\/th><th>First order<\/th><\/tr><\/thead><tbody><tr><td>Integrated rate law<\/td><td>[R] = [R]\u2080 \u2212 kt<\/td><td>k = (2.303\/t) log([R]\u2080\/[R])<\/td><\/tr><tr><td>Half-life<\/td><td>t\u00bd = [R]\u2080 \/ 2k<\/td><td>t\u00bd = 0.693 \/ k<\/td><\/tr><tr><td>Half-life depends on [R]\u2080?<\/td><td>Yes, directly proportional<\/td><td>No, independent<\/td><\/tr><tr><td>Straight-line graph<\/td><td>[R] vs t, slope = \u2212k<\/td><td>ln[R] vs t, slope = \u2212k<\/td><\/tr><tr><td>Example<\/td><td>Decomposition of NH\u2083 on hot platinum at high pressure<\/td><td>Radioactive decay, decomposition of N\u2082O\u2085<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Time-saving shortcuts for first order kinetics:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Time for <strong>75%<\/strong> completion = <strong>2 \u00d7 t\u00bd<\/strong><\/li>\n\n\n\n<li>Time for <strong>87.5%<\/strong> completion = <strong>3 \u00d7 t\u00bd<\/strong><\/li>\n\n\n\n<li>Time for <strong>99.9%<\/strong> completion \u2248 <strong>10 \u00d7 t\u00bd<\/strong><\/li>\n\n\n\n<li>A plot of log([R]\u2080\/[R]) vs t is a straight line through the origin with slope k\/2.303.<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Pseudo first order reactions<\/strong> are second order reactions that behave as first order because one reactant is in large excess, such as the acid hydrolysis of ethyl acetate and the inversion of cane sugar.<\/p>\n\n\n\n<h2 id=\"the-arrhenius-equation\" class=\"wp-block-heading\">The Arrhenius Equation<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>k = A e^(\u2212Ea\/RT)<\/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>Form<\/th><th>Use<\/th><\/tr><\/thead><tbody><tr><td>ln k = ln A \u2212 Ea\/RT<\/td><td>A plot of ln k vs 1\/T is a straight line with slope \u2212Ea\/R<\/td><\/tr><tr><td>log k = log A \u2212 Ea\/(2.303RT)<\/td><td>Slope of log k vs 1\/T = \u2212Ea\/(2.303R)<\/td><\/tr><tr><td>log(k\u2082\/k\u2081) = [Ea\/(2.303R)] \u00d7 [(T\u2082 \u2212 T\u2081)\/(T\u2081T\u2082)]<\/td><td>Two-temperature questions<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Facts that come back again and again:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For many reactions, a <strong>10 \u00b0C rise roughly doubles the rate<\/strong>.<\/li>\n\n\n\n<li>A <strong>catalyst lowers the activation energy<\/strong>, so it speeds up both forward and backward reactions. It does <strong>not<\/strong> change \u0394G or the equilibrium constant.<\/li>\n\n\n\n<li>In collision theory, <strong>rate = P Z_AB e^(\u2212Ea\/RT)<\/strong>, where P is the steric (probability) factor that accounts for proper orientation.<\/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. A first order process has k = 0.0693 min\u207b\u00b9. How long does it take to reach 75% completion?<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">t\u00bd = 0.693\/k = 0.693\/0.0693 = 10 min. For 75% completion, t = 2 \u00d7 t\u00bd.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 20 minutes.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q2. The k of a reaction has units L mol\u207b\u00b9 s\u207b\u00b9. The order of the reaction is:<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Using (mol L\u207b\u00b9)^(1 \u2212 n) s\u207b\u00b9: (mol L\u207b\u00b9)\u207b\u00b9 means 1 \u2212 n = \u22121, so n = 2.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: Second order.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q3. When the concentration of A is doubled, the rate increases four times. The order with respect to A is:<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">2\u207f = 4, so n = 2.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 2.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q4. The rate of a reaction doubles when the temperature rises from 300 K to 310 K. Find Ea (R = 8.314 J K\u207b\u00b9 mol\u207b\u00b9, log 2 = 0.301).<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">log 2 = [Ea\/(2.303 \u00d7 8.314)] \u00d7 [10\/(300 \u00d7 310)]<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Ea = 0.301 \u00d7 2.303 \u00d7 8.314 \u00d7 9300 \u2248 53,600 J mol\u207b\u00b9<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: About 53.6 kJ mol\u207b\u00b9.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q5. For a zero order reaction, the half-life is:<\/strong> (a) Independent of initial concentration (b) Proportional to initial concentration (c) Inversely proportional to initial concentration (d) Proportional to the square of initial concentration<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: (b).<\/strong> t\u00bd = [R]\u2080\/2k, so it is directly proportional to the initial concentration.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q6. In 2N\u2082O\u2085 \u2192 4NO\u2082 + O\u2082, if d[O\u2082]\/dt = 1.0 \u00d7 10\u207b\u2074 mol L\u207b\u00b9 s\u207b\u00b9, what is d[NO\u2082]\/dt?<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">(1\/4) d[NO\u2082]\/dt = d[O\u2082]\/dt, so d[NO\u2082]\/dt = 4 \u00d7 1.0 \u00d7 10\u207b\u2074.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Answer: 4.0 \u00d7 10\u207b\u2074 mol L\u207b\u00b9 s\u207b\u00b9.<\/strong><\/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>Saying the first order half-life depends on initial concentration<\/li>\n\n\n\n<li>Thinking a catalyst changes the equilibrium constant or \u0394G<\/li>\n\n\n\n<li>Giving molecularity as zero or a fraction<\/li>\n\n\n\n<li>Forgetting to divide by stoichiometric coefficients in rate expressions<\/li>\n\n\n\n<li>Using ln and log interchangeably without the 2.303 factor<\/li>\n\n\n\n<li>Writing the slope of ln k vs 1\/T as +Ea\/R instead of \u2212Ea\/R<\/li>\n<\/ul>\n\n\n\n<h2 id=\"practise-every-chemical-kinetics-pyq\" class=\"wp-block-heading\">Practise Every Chemical Kinetics PYQ<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">This chemical kinetics NEET PYQ analysis shows you where the marks are. Solving real past questions makes the formulas automatic. Every Chemical Kinetics 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\/chemical-kinetics\/\" target=\"_blank\" rel=\"noopener\">Solve all Chemical Kinetics NEET PYQs<\/a><\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Keep the formula table beside you for the first round, then solve the second round without it.<\/p>\n\n\n\n<h2 id=\"conclusion\" class=\"wp-block-heading\">Conclusion<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Chemical Kinetics rewards practice more than reading. Use this chemical kinetics NEET PYQ analysis to master the Arrhenius equation, first order half-life shortcuts, units of the rate constant and rate expressions. Then solve the past numericals until each one takes under a minute.<\/p>\n\n\n\n<h2 id=\"faq\" class=\"wp-block-heading\">FAQ<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: How many questions come from Chemical Kinetics in NEET?<\/strong> A: Usually about two questions a year, mostly short numericals.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: What is the most important topic in Chemical Kinetics for NEET?<\/strong> A: The Arrhenius equation and activation energy calculations are the most tested, followed by first order half-life and finding the order of a reaction.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: Does the half-life of a first order reaction depend on initial concentration?<\/strong> A: No. t\u00bd = 0.693\/k, so it is independent of the initial concentration. For a zero order reaction, it is directly proportional to it.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: Does a catalyst change the equilibrium constant?<\/strong> A: No. A catalyst lowers the activation energy and speeds up both forward and backward reactions equally, so the equilibrium constant and \u0394G stay the same.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: How do I find the order of a reaction from the units of k?<\/strong> A: Use units of k = (mol L\u207b\u00b9)^(1 \u2212 n) s\u207b\u00b9. For example, s\u207b\u00b9 means first order and L mol\u207b\u00b9 s\u207b\u00b9 means second order.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Q: Where can I practise Chemical Kinetics NEET PYQs for free?<\/strong> A: You can solve every Chemical Kinetics previous year question chapter-wise for free using the practice links in this article.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Quick answer: A chemical kinetics NEET PYQ analysis shows that NTA asks about two questions a year from this chapter, and most are short numericals from four areas: the Arrhenius equation and activation energy, first order reaction half-life and time calculations, finding order from units of the rate constant or rate data, and the relation [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":6979,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[8,69,2],"tags":[3407,3408,4288,2820,4289,4290,7,4008,24,2328,4291,2322,3406],"class_list":["post-6978","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-study-tips","category-chemistry","category-neet","tag-activation-energy","tag-arrhenius-equation","tag-chemical-kinetics","tag-class-12-chemistry","tag-first-order-reaction","tag-half-life-2","tag-neet-2027","tag-neet-chapter-wise-pyq","tag-neet-chemistry","tag-neet-pyq","tag-order-and-molecularity","tag-physical-chemistry","tag-rate-constant"],"_links":{"self":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/6978","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=6978"}],"version-history":[{"count":1,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/6978\/revisions"}],"predecessor-version":[{"id":6980,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/6978\/revisions\/6980"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media\/6979"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=6978"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=6978"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=6978"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}