{"id":852,"date":"2024-07-18T05:39:22","date_gmt":"2024-07-18T05:39:22","guid":{"rendered":"https:\/\/www.meniit.com\/study-material\/?p=852"},"modified":"2024-08-02T10:24:56","modified_gmt":"2024-08-02T10:24:56","slug":"some-basic-concepts-of-chemistry","status":"publish","type":"post","link":"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry","title":{"rendered":"Some Basic Concepts of Chemistry"},"content":{"rendered":"<h2 style=\"text-align: justify;\">SECTION 1 : LAWS OF CHEMICAL COMBINATION<\/h2>\n<h4 style=\"text-align: justify;\">1.1 THE LAW OF CONSERVATION OF MASS (LAVOISER, 1744) :<\/h4>\n<p style=\"text-align: justify;\">This law states \u201c<strong>matter can neither be nor be destroyed<\/strong> or in a chemical reaction, the mass of the reactants is equal to the mass of the products\u201d. The exception to this law is nuclear reactions where Einstein equation is applicable.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-854 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/einstein-equation-1.png\" alt=\"einstein-equation\" width=\"606\" height=\"154\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/einstein-equation-1.png 606w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/einstein-equation-1-300x76.png 300w\" sizes=\"auto, (max-width: 606px) 100vw, 606px\" \/><\/p>\n<p style=\"text-align: justify;\">For a complete irreversible reaction total mass of reactants before reaction in equal to the total mass of products after reaction.<\/p>\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_69_1 counter-hierarchy ez-toc-counter ez-toc-light-blue ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title\" style=\"cursor:inherit\">Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" aria-label=\"Toggle Table of Content\"><span class=\"ez-toc-js-icon-con\"><span class=\"\"><span class=\"eztoc-hide\" style=\"display:none;\">Toggle<\/span><span class=\"ez-toc-icon-toggle-span\"><svg style=\"fill: #999;color:#999\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #999;color:#999\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/span><\/span><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\/#12-THE-LAW-OF-CONSTANT-COMPOSITION-OR-DEFINITE-PROPORTION-PROUST-1799\" title=\"1.2 THE LAW OF CONSTANT COMPOSITION OR DEFINITE PROPORTION (PROUST, 1799)\">1.2 THE LAW OF CONSTANT COMPOSITION OR DEFINITE PROPORTION (PROUST, 1799)<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\/#SECTION-2-ATOMIC-MASS-AND-MOLECULAR-MASS\" title=\"SECTION 2 : ATOMIC MASS AND MOLECULAR MASS\">SECTION 2 : ATOMIC MASS AND MOLECULAR MASS<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\/#SECTION-4-MOLE-CONCEPT\" title=\"SECTION 4 : MOLE CONCEPT\">SECTION 4 : MOLE CONCEPT<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\/#SECTION-5-MOLE-CONCEPT-AND-GASES\" title=\"SECTION 5 : MOLE CONCEPT AND GASES\">SECTION 5 : MOLE CONCEPT AND GASES<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\/#SECTION-7-CONCEPT-OF-LIMITING-REACTANT\" title=\"SECTION 7 : CONCEPT OF LIMITING REACTANT\">SECTION 7 : CONCEPT OF LIMITING REACTANT<\/a><\/li><\/ul><\/nav><\/div>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"12-THE-LAW-OF-CONSTANT-COMPOSITION-OR-DEFINITE-PROPORTION-PROUST-1799\"><\/span>1.2 THE LAW OF CONSTANT COMPOSITION OR DEFINITE PROPORTION (PROUST, 1799)<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p style=\"text-align: justify;\">This law states that <strong>\u201cAll pure sample of the same chemical compound contain the same elements combined in the same proportion by mass irrespective of the method of preparation\u201d.<\/strong><\/p>\n<p style=\"text-align: justify;\"><strong>Example<\/strong>: Example: Differ Example: ent samples of carbon dioxide contain carbon and oxygen in the ratio of 3 : 8 by mass.<\/p>\n<p style=\"text-align: justify;\">Similarly in water ratio of weight of hydrogen to oxygen is 1 : 8.<\/p>\n<h4 style=\"text-align: justify;\">1.3 LAW OF MULTIPLE PROPORTION (DALTON, 1803)<\/h4>\n<p style=\"text-align: justify;\">\u201cWhen the two elements combine to form two or more chemical compounds, then the weight of one of the elements which combines with a fixed weight of the other, bear a simple whole number ratio to one another. This is called the law of multiple proportions.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-855 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/carbon-forms-two-oxides-1.png\" alt=\"carbon-forms-two-oxides\" width=\"906\" height=\"258\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/carbon-forms-two-oxides-1.png 906w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/carbon-forms-two-oxides-1-300x85.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/carbon-forms-two-oxides-1-768x219.png 768w\" sizes=\"auto, (max-width: 906px) 100vw, 906px\" \/><\/p>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"SECTION-2-ATOMIC-MASS-AND-MOLECULAR-MASS\"><\/span>SECTION 2 : ATOMIC MASS AND MOLECULAR MASS<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<h4 style=\"text-align: justify;\">2.1 ATOMIC MASS<\/h4>\n<p style=\"text-align: justify;\">As atoms are very tiny particles, their absolute masses are difficult to measure. However it is possible to determine the relative masses of different atoms if small unit of mass is taken as standard (previously, this standard was mass of one atom of hydrogen and taken as unity). Later on, 1\/16<sup>th<\/sup> mass of oxygen atom and now it is 1\/12<sup>th<\/sup> mass of C-12 atom.<\/p>\n<p style=\"text-align: justify;\">The atomic mass of an element can be defined as the number which indicates how many times the mass of one atom of the element is heavier in comparison to 1\/12<sup>th<\/sup> mass of an atom of C-12.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-856 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-unit-1.png\" alt=\"atomic-mass-unit\" width=\"709\" height=\"232\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-unit-1.png 709w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-unit-1-300x98.png 300w\" sizes=\"auto, (max-width: 709px) 100vw, 709px\" \/><\/p>\n<h4 style=\"text-align: justify;\">2.2 ATOMIC MASS UNIT<\/h4>\n<p style=\"text-align: justify;\">The quantity 1\/12<sup>th<\/sup> mass of an atom of carbon-12 is known as<strong> atomic mass unit<\/strong> and is abbreviated as amu. The actual mass of one atom of carbon-12 is 1.9924 \u00d7 10<sup>\u201323<\/sup> g or 1.9924 \u00d710<sup>\u201326<\/sup> kg<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-857 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-1.png\" alt=\"atomic-mass\" width=\"820\" height=\"202\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-1.png 820w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-1-300x74.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/atomic-mass-1-768x189.png 768w\" sizes=\"auto, (max-width: 820px) 100vw, 820px\" \/><\/p>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"SECTION-4-MOLE-CONCEPT\"><\/span>SECTION 4 : MOLE CONCEPT<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p style=\"text-align: justify;\">Mole is a collection of 6.023 \u00d7 10<sup>23<\/sup> particles (atoms or molecules or ions). It is the SI unit for amount of a substance also. For instance, one mole CaO molecules refer to 6.023 \u00d7 10<sup>23<\/sup> molecules of CaO.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-858 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/mole-concepts-1.png\" alt=\"mole-concepts\" width=\"942\" height=\"514\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/mole-concepts-1.png 942w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/mole-concepts-1-300x164.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/mole-concepts-1-768x419.png 768w\" sizes=\"auto, (max-width: 942px) 100vw, 942px\" \/><\/p>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"SECTION-5-MOLE-CONCEPT-AND-GASES\"><\/span>SECTION 5 : MOLE CONCEPT AND GASES<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p style=\"text-align: justify;\">It is imperative to know that gases can be quantified similar to solids and liquids. Many of the earlier developments related moles to gases and their volumes. To understand this clearly, we must learn that we presume all gases present in the universe to be <strong>ideal\u00a0<\/strong>and for all ideal gases the <strong>Ideal Gas Equation<\/strong> holds true. This is given as: <strong>P \u00d7 V = nRT.<\/strong> Here, P is the pressure of the gas, V is the volume of the gas (which is taken T to be the volume of the vessel in which it is contained), n are the number of moles of the gas and T is temeprature of the gas (in Kelvin). Here, R is the universal gas constant and its value can be taken to be 0.0821 l.atm\/mol.K or 8.314 J\/mol.K.<\/p>\n<p style=\"text-align: justify;\">Some of the developments are listed here for your knowledge:<\/p>\n<h4 style=\"text-align: justify;\">5.4 VAPOUR DENSITY<\/h4>\n<p style=\"text-align: justify;\">t is defined as a number which indicates how dense a gas is with respect to density of H<sub>2<\/sub> gas at STP. Learn, that vapour density is just a number and hence dimensionless.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-859 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/vapour-density-1.png\" alt=\"vapour-density\" width=\"916\" height=\"154\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/vapour-density-1.png 916w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/vapour-density-1-300x50.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/vapour-density-1-768x129.png 768w\" sizes=\"auto, (max-width: 916px) 100vw, 916px\" \/><\/p>\n<h4 style=\"text-align: justify;\">5.5 MOLAR VOLUME OF AN IDEAL GAS AT STP<\/h4>\n<p style=\"text-align: justify;\">We know from our earlier discussion that Standard Pressure for ideal gases is taken to be 1 atm and Standard Temperature is taken to be 273.15 K or 0\u00b0C. Under these conditions the volume of one mole of a ideal gas also called Molar Volume will be calculated as<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-860 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/molar-volume-1.png\" alt=\"molar-volume\" width=\"856\" height=\"130\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/molar-volume-1.png 856w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/molar-volume-1-300x46.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/molar-volume-1-768x117.png 768w\" sizes=\"auto, (max-width: 856px) 100vw, 856px\" \/><\/p>\n<h4 style=\"text-align: justify;\">5.6 GAY LUSSAC\u2019S LAW OF COMBINING VOLUMES<\/h4>\n<p style=\"text-align: justify;\">According to this law, when gases react together, under similar conditions of temperature and pressure then the ratio in which their moles react is same as the ratio in which their volumes.<\/p>\n<p style=\"text-align: justify;\">For example consider a combination between hydrogen gas and chlorine gas:<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-872 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law-2.png\" alt=\"gay-lussacs-law\" width=\"328\" height=\"66\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law-2.png 328w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law-2-300x60.png 300w\" sizes=\"auto, (max-width: 328px) 100vw, 328px\" \/><\/p>\n<p style=\"text-align: justify;\">One mole of H<sub>2<\/sub> will react with 1 mole of Cl<sub>2<\/sub> to give 2 moles of HCl, so we can say that at the same pressure and temperature one volume of hydrogen and one volume of chlorine always combine to form two volumes of HCl gas.<\/p>\n<p style=\"text-align: justify;\">The ratio between the volumes of the reactants and products in this reaction is simple, that is 1 : 1 : 2. Hence, it illustrates law of combining volumes.<\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-873 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law2-1.png\" alt=\"gay-lussacs-law2\" width=\"943\" height=\"61\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law2-1.png 943w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law2-1-300x19.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/07\/gay-lussacs-law2-1-768x50.png 768w\" sizes=\"auto, (max-width: 943px) 100vw, 943px\" \/><\/p>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"SECTION-7-CONCEPT-OF-LIMITING-REACTANT\"><\/span>SECTION 7 : CONCEPT OF LIMITING REACTANT<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p style=\"text-align: justify;\">In a reaction, reactants react in a fixed ratio of their moles, which are represented by the stoichiometric coefficients in the balanced chemical equation. If we consider 2H<sub>2<\/sub> + O<sub>2<\/sub> \u2192 2H<sub>2<\/sub>O, then we can say that 2 moles of H<sub>2<\/sub> react with 1 mole of O<sub>2<\/sub> to give 2 moles of water.<\/p>\n<p style=\"text-align: justify;\">However, in most industrial operations, exact proportions may not be present, in such a case one of the reactants gets completely consumed during the course of the reaction while the other remains unreacted as it was present in larger quantities. <strong>The reactant that gets completely consumed is called the Limiting <\/strong><strong>Reactant and the one which is left out is called the Excess Reactant.<\/strong><\/p>\n<p style=\"text-align: justify;\">To explain this better, let us consider the reaction given above, 2H<sub>2<\/sub> + O<sub>2<\/sub> \u2192 2H<sub>2<\/sub>O. If we have 3 moles of H<sub>2<\/sub> and 0.5 moles of O<sub>2<\/sub> in this process then :<\/p>\n<ol style=\"text-align: justify;\">\n<li>We know that 1 mole of O<sub>2<\/sub> reacts with 2 moles of H<sub>2<\/sub> so, 0.5 moles will react with 1 mole H<sub>2<\/sub>.<\/li>\n<li>So, in other words, O2 finishes off completely, whereas 3 \u2013 1 = 2 moles of H<sub>2<\/sub> will be left unreacted.<\/li>\n<li>As per our definitions, O<sub>2<\/sub> will be called the limiting reactant and H<sub>2<\/sub> will be called the excess reactant here.<\/li>\n<\/ol>\n<p style=\"text-align: justify;\">Also learn, that the product yield is always estimated using the limiting reactant, so if 1 mole O<sub>2<\/sub> gives 2 moles of water as per the equation, then 0.5 moles O<sub>2<\/sub> will give 1 mole of water or 18 g water.<\/p>\n<p style=\"text-align: justify;\">In order to estimate the limiting reactant, calculate the value of Moles Given\/Stoichiometric Coefficient for the given reactants. The one having the smallest value of this ratio will be the limiting reactant.<\/p>\n<div class=\"newspaper-x-tags\"><strong>TAGS: <\/strong><span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/atomic-mass\" rel=\"tag\">Atomic Mass<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/laws-of-chemical-combination\" rel=\"tag\">Laws Of Chemical Combination<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/molar-volume\" rel=\"tag\">Molar volume<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/mole-concept\" rel=\"tag\">Mole Concept<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/molecular-mass\" rel=\"tag\">Molecular mass<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/some-basic-concepts-of-chemistry\" rel=\"tag\">Some Basic Concepts of Chemistry<\/a> <\/div>\n","protected":false},"excerpt":{"rendered":"<p>SECTION 1 : LAWS OF CHEMICAL COMBINATION 1.1 THE LAW OF CONSERVATION OF MASS (LAVOISER, 1744) : This law states&nbsp;&nbsp;&#8230;.<a class=\"read_more\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/some-basic-concepts-of-chemistry\" rel=\"nofollow\">Read More >><\/a><\/p>\n","protected":false},"author":6,"featured_media":1231,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"om_disable_all_campaigns":false,"rank_math_lock_modified_date":false,"footnotes":""},"categories":[268,241,240],"tags":[331,330,346,333,345,329],"class_list":["post-852","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemistry","category-class-11th","category-neet","tag-atomic-mass","tag-laws-of-chemical-combination","tag-molar-volume","tag-mole-concept","tag-molecular-mass","tag-some-basic-concepts-of-chemistry"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/852","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/comments?post=852"}],"version-history":[{"count":8,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/852\/revisions"}],"predecessor-version":[{"id":1233,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/852\/revisions\/1233"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/media\/1231"}],"wp:attachment":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/media?parent=852"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/categories?post=852"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/tags?post=852"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}