{"id":1177,"date":"2019-12-03T13:40:03","date_gmt":"2019-12-03T13:40:03","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=1177"},"modified":"2019-12-03T13:40:09","modified_gmt":"2019-12-03T13:40:09","slug":"catalytic-reactions","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/catalytic-reactions\/","title":{"rendered":"Catalytic Reactions"},"content":{"rendered":"\n<h2>Introduction<\/h2>\n\n\n\n<ul><li><strong>What is a catalyst?<\/strong><\/li><\/ul>\n\n\n\n<p>A\ncatalyst is a substance that is used to speed up a chemical reaction but it is\nnot consumed by the reaction.<\/p>\n\n\n\n<ul><li><strong>What is catalysis?<\/strong><\/li><\/ul>\n\n\n\n<p>Catalysis\nis a process of increasing the rate of a chemical reaction by adding a chemical\nsubstance which is known as a catalyst.<\/p>\n\n\n\n<p>A very\nsmall amount of catalyst is required to alter the reaction rate.<\/p>\n\n\n\n<h2>What is a catalyzed reaction?<\/h2>\n\n\n\n<p>A catalyzed reaction is\ntypically used to accelerate the rate by which specific chemistry is to\nproceed.<\/p>\n\n\n\n<p>Generally, the role of the catalyst is to provide an alternative, low energy pathway for a reaction. For this to happen, the catalyst interacts with a reactant and forms an intermediate compound. This intermediate is temporary in that after it forms, it breaks apart and leaves the original catalyst species unchanged.<\/p>\n\n\n\n<h2>Types of catalyzed reactions<\/h2>\n\n\n\n<p>There are two major types of\ncatalyzed reactions<\/p>\n\n\n\n<ol><li>Heterogeneous Catalyzed Reaction<\/li><li>Homogeneous Catalyzed Reaction<\/li><\/ol>\n\n\n\n<p>A heterogeneously catalyzed\nreaction occurs when the catalyst and the reactant exist in two different\nphases i.e. a solid catalyst in the presence of a reactant in solution.<\/p>\n\n\n\n<p>A homogeneously catalyzed\nreaction occurs when the catalyst and the reactant are in the same phase i.e.\nwhen the catalyst and the reactants are dissolved in the same solution.<\/p>\n\n\n\n<p>Now let&#8217;s have a look that what a phase is?<\/p>\n\n\n\n<h2>What is a phase?<\/h2>\n\n\n\n<p>Consider a mixture. Now observe a mixture carefully. You will see that there is a boundary between two of the components which indicates that the substances are in different phases. A mixture that contains a solid and a liquid consists of two different phases while a mixture that contains various chemicals in a single solution consists of only one phase because there is no apparent boundary between them.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"394\" height=\"255\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-39.png\" alt=\"\" class=\"wp-image-1178\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-39.png 394w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-39-300x194.png 300w\" sizes=\"(max-width: 394px) 100vw, 394px\" title=\"\"><\/figure><\/div>\n\n\n\n<p>You might think that the why phase differs from the term physical state (solid, liquid or gas). It may include solids, liquids, and gases but is a bit more general. It can also be applied to the liquids that do not dissolve into each other but forms a boundary between the two liquids i.e. oil and water.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"382\" height=\"239\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-41.png\" alt=\"\" class=\"wp-image-1180\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-41.png 382w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-41-300x188.png 300w\" sizes=\"(max-width: 382px) 100vw, 382px\" title=\"\"><\/figure><\/div>\n\n\n\n<h2>Explanation<\/h2>\n\n\n\n<p><strong>Heterogeneous\ncatalysis<\/strong><\/p>\n\n\n\n<p>This type includes the use of\na catalyst in a different phase from the reactants. The common examples involve\na solid catalyst with the reactants as either liquids or gases.<\/p>\n\n\n\n<p><strong>Working\nprinciple of a heterogeneous catalyst<\/strong><\/p>\n\n\n\n<p>Majority of the examples of\nthe heterogeneous catalysis go through the same stages<\/p>\n\n\n\n<p>One or more than one of the reactants\nare <strong>adsorbed<\/strong> on to the surface of\nthe catalyst at <strong>active sites.<\/strong><\/p>\n\n\n\n<p>Adsorption is the process in\nwhich atoms, ions or molecules from different substances like solid, liquid or\ngas adhere to a surface of the adsorbent. On the other side absorption is a process\nin which a fluid is completely dissolved by an absorbent.<\/p>\n\n\n\n<p>An active site includes that\npart of a surface which is particularly good at adsorbing things and also help\nthem to react.<\/p>\n\n\n\n<p>There is some kind of interaction between the surface of the catalyst and the reactant molecules which makes them more reactive. This might involve an actual reaction with the surface or some weakening of the bonds in the attached molecules.<\/p>\n\n\n\n<p>The reaction occurs and at\nthis stage, both of the reactant molecules might attach themselves to the\nsurface or one might get attached and hit by the other one that moves freely in\nthe gas or liquid.<\/p>\n\n\n\n<p>The product molecules are <strong>desorbed.<\/strong><\/p>\n\n\n\n<p>Desorption generally means the\nbreakdown of the product molecules. This makes a space available at active\nsites for the new molecules to come, attach and to react.<\/p>\n\n\n\n<p>A catalyst is considered as a\ngood catalyst that is adsorbed to the reactant molecules strong enough that\nthey react but not that much stronger than the product molecules stick more or\nless permanently to the surface.<\/p>\n\n\n\n<p>For example, silver is not\nconsidered a good catalyst because it does not attach strongly with the\nreactant molecules while tungsten too is not considered a good catalyst as it\nadsorbs too strongly with the reactant molecules.<\/p>\n\n\n\n<p>Metals like platinum and\nnickel are considered as a good catalyst because they absorb strongly to hold\nand activate the reactants but not that much strongly that the products can\u2019t\nbreak away.<\/p>\n\n\n\n<h2>Example of heterogeneous reactions<\/h2>\n\n\n\n<p><strong>The\nhydrogenation of a carbon-carbon double bond<\/strong><\/p>\n\n\n\n<p>the simplest example of this\ntype of reaction is between ethene and hydrogen in the presence of a nickel\ncatalyst.<\/p>\n\n\n\n<p>CH<sub>2 <\/sub>= CH<sub>2<\/sub> + H<sub>2<\/sub>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Ni&nbsp;as&nbsp;&nbsp;catalyst&nbsp;         CH<sub>3<\/sub>CH<sub>3<\/sub><\/p>\n\n\n\n<p>In actual, this is a useless\nreaction, because you are converting the very useful ethene into the relatively\nuseless ethane. However, the same reaction will occur with any compound that\ncontains a carbon-carbon double bond.<\/p>\n\n\n\n<p>One of the important\nindustrial use is in the hydrogenation of vegetable oils to make margarine,\nwhich also involves reacting a carbon-carbon double bond in the vegetable oil\nwith hydrogen in the presence of a nickel catalyst.<\/p>\n\n\n\n<p>Ethene molecules are adsorbed on the surface of the nickel. There is a breakdown of a double bond between carbon atoms and hence the electrons are used to bond it to the nickel surface.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"433\" height=\"148\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-42.png\" alt=\"\" class=\"wp-image-1182\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-42.png 433w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-42-300x103.png 300w\" sizes=\"(max-width: 433px) 100vw, 433px\" title=\"\"><\/figure><\/div>\n\n\n\n<p>There is adsorption of hydrogen molecules on to the surface of the nickel. When this takes place, the hydrogen molecules break into atoms. These can move around on the surface of the nickel.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"433\" height=\"190\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-43.png\" alt=\"\" class=\"wp-image-1183\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-43.png 433w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-43-300x132.png 300w\" sizes=\"(max-width: 433px) 100vw, 433px\" title=\"\"><\/figure><\/div>\n\n\n\n<p>If there is a diffusion of hydrogen atoms close to one of the bonded carbons, the bond between the carbon and the nickel is replaced by one between the carbon and hydrogen.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"385\" height=\"189\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-44.png\" alt=\"\" class=\"wp-image-1184\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-44.png 385w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-44-300x147.png 300w\" sizes=\"(max-width: 385px) 100vw, 385px\" title=\"\"><\/figure><\/div>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"433\" height=\"157\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-45.png\" alt=\"\" class=\"wp-image-1185\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-45.png 433w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-45-300x109.png 300w\" sizes=\"(max-width: 433px) 100vw, 433px\" title=\"\"><\/figure><\/div>\n\n\n\n<p>Now that end of the original\nethene breaks free of the surface, and eventually, the same thing will occur at\nthe other end.<\/p>\n\n\n\n<p>As earlier, one of the\nhydrogen atoms forms a bond with the carbon and that end also breaks free. Now\nthere is a space on the surface of the nickel for new reactants molecules to go\nthrough the whole process again.<\/p>\n\n\n\n<h2>Catalytic Converters<\/h2>\n\n\n\n<p>Catalytic converters change\npoisonous molecules like carbon monoxide and different nitrogen oxides in car\nexhaust into less harmless molecules like carbon dioxide and nitrogen. The\nexpensive metals are used like rhodium, platinum, and palladium as they are a\nheterogeneous catalyst.<\/p>\n\n\n\n<p>The metals are deposited on a\nceramic honeycomb as thin layers. This increases the surface area and minimizes\nthe use of metal.<\/p>\n\n\n\n<p>The reaction between carbon\nmonoxide and nitrogen monoxide can be written as<\/p>\n\n\n\n<p>2CO + 2NO&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Pt\/ Pd \/ Rhconverts to &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2CO<sub>2<\/sub> +N<sub>2<\/sub><\/p>\n\n\n\n<p><strong>Homogeneous\nCatalytic Reactions<\/strong><\/p>\n\n\n\n<p>In these reactions, the\ncatalyst is in the same phase as the reactants. Generally, everything will be\npresent as a gas or contained in a single liquid phase.<\/p>\n\n\n\n<h2>Examples of homogeneous catalytic reactions<\/h2>\n\n\n\n<p><strong>The\nreaction between persulphate ions and iodide ions<\/strong><\/p>\n\n\n\n<p>Persulphate ions are very\nstrong oxidizing agents while iodide ions are very easily oxidized to form\niodine. In water, these reactions are very slow.<\/p>\n\n\n\n<p>The reaction equation is given\nbelow<\/p>\n\n\n\n<p>S<sub>2<\/sub>O<sub>8<\/sub><sup>2-<\/sup>&nbsp; +&nbsp; 2I<sup>&#8211;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;converts to &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; <\/sup>2SO<sub>4<\/sub><sup>2-<\/sup> + I<sub>2<\/sub><\/p>\n\n\n\n<p>The reaction requires a\ncollision between the two negative ions. The catalyzed reaction avoids that\nproblem fully. The catalyst used here can either be an iron II or iron III ions\nthat are added to the same solution.<\/p>\n\n\n\n<p>Another good example of the\nuse of the transition metal compounds as catalysts because of having an ability\nto change oxidation state.<\/p>\n\n\n\n<p>First, we will take iron II\nions as a catalyst but after some time you will observe that it doesn&#8217;t matter\nat all whether you use iron II or iron III ions<\/p>\n\n\n\n<p>The persulphate ions oxidize\nthe iron II to iron III ions. During this reaction, the persulphate ions are\nreduced to sulphate ions.<\/p>\n\n\n\n<p>&nbsp; S<sub>2<\/sub>O<sub>8<\/sub><sup>2-&nbsp; <\/sup>+&nbsp; 2Fe<sup>2+<\/sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;converts to &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2SO<sub>4<\/sub><sup>2-&nbsp;&nbsp; <\/sup>+&nbsp; 2Fe<sup>3+<\/sup><\/p>\n\n\n\n<p>The iron III ions are much\nstrong that they oxidize the iodide ions to iodine easily. In this process,\nthey are reduced back to iron II ions again. <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2Fe<sup>3+&nbsp; <\/sup>+ 2I<sup>&#8211; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<\/sup>converts to <sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; <\/sup>2Fe<sup>2+&nbsp; <\/sup>+ I<sub>2<\/sub><\/p>\n\n\n\n<p>In an overall reaction, both\nof these individual stages involve a collision between positive and negative\nions. This will be a much successful reaction in the presence of a catalyst\nother than in an uncatalyzed reaction.<\/p>\n\n\n\n<h2>Other examples of Catalytic Reactions<\/h2>\n\n\n\n<ul><li><strong>The halogenation of benzene<\/strong><\/li><\/ul>\n\n\n\n<p>Benzene\nreacts with chlorine or bromine in the presence of a catalyst. The catalyst\nused can either be aluminum chloride or iron.<\/p>\n\n\n\n<p>Strictly\ntalking about iron is not a catalyst, because it gets permanently changed\nduring the reaction. It reacts with chlorine or bromine to form iron III\nchloride, FeCl<sub>3<\/sub> or iron III bromide, FeBr<sub>3<\/sub>.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2Fe + 3Cl<sub>2 <\/sub>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;converts to &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;2FeCl<sub>3<\/sub><\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2Fe +3Br<sub>2<\/sub>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;converts to &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; 2FeBr<sub>3<\/sub><\/p>\n\n\n\n<p>These\ncompounds act as a catalyst and act exactly the same as aluminum chloride in\nthese reactions.<\/p>\n\n\n\n<ul><li><strong>The reaction with chlorine<\/strong><\/li><\/ul>\n\n\n\n<p>The reaction between benzene and chlorine in the presence of either aluminum chloride or iron gives chlorobenzene.<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter size-large\"><img loading=\"lazy\" width=\"279\" height=\"75\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-46.png\" alt=\"\" class=\"wp-image-1186\" title=\"\"><\/figure><\/div>\n\n\n\n<ul><li><strong>The reaction with bromine<\/strong><\/li><\/ul>\n\n\n\n<p>The\nreaction between benzene and bromine in the presence of either aluminum bromide\nor iron gives bromobenzene. Generally, iron is used because it is not very\nexpensive and easily available.<\/p>\n\n\n\n<p class=\"has-text-align-center\">C<sub>6<\/sub>H<sub>6&nbsp; + <\/sub>Br<sub>2<\/sub> &nbsp;converts to&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; C<sub>6<\/sub>H<sub>5<\/sub>Br + HBr<\/p>\n\n\n\n<ul><li><strong>The Friedel-crafts alkylation of benzene<\/strong><\/li><\/ul>\n\n\n\n<p>Alkylation\nincludes the replacement of a hydrogen atom on a benzene ring by an alkyl group\nlike methyl or ethyl. This represents another example of the use of aluminum\nchloride as a catalyst. Benzene is allowed to react with chloroalkane in the\npresence of aluminum chloride as a catalyst. The below equation shows the\nreaction by using a methyl group but any other alkyl group can be used in the\nsame manner.<\/p>\n\n\n\n<p>Substituting\na methyl group gives methylbenzene, which was once known as toluene.<\/p>\n\n\n\n<p>C<sub>6<\/sub>H<sub>6 + <\/sub>CH<sub>3<\/sub>Cl&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;converts to&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; C<sub>6<\/sub>H<sub>5<\/sub>CH<sub>3<\/sub> + HCl<\/p>\n\n\n\n<h4>References<\/h4>\n\n\n\n<ul><li><a href=\"https:\/\/chem.libretexts.org\/Bookshelves\/Inorganic_Chemistry\/Supplemental_Modules_(Inorganic_Chemistry)\/Catalysis\/Examples\/Examples_of_Catalysis\/5._Examples_of_Other_Catalytic_Reactions_in_Organic_Chemistry\" target=\"_blank\" rel=\"noopener\">https:\/\/chem.libretexts.org\/Bookshelves\/Inorganic_Chemistry\/Supplemental_Modules_(Inorganic_Chemistry)\/Catalysis\/Examples\/Examples_of_Catalysis\/5._Examples_of_Other_Catalytic_Reactions_in_Organic_Chemistry<\/a><\/li><li><a href=\"https:\/\/en.wikipedia.org\/wiki\/Catalysis\" target=\"_blank\" rel=\"noopener\">https:\/\/en.wikipedia.org\/wiki\/Catalysis<\/a><\/li><li><a href=\"https:\/\/www.mt.com\/my\/en\/home\/applications\/L1_AutoChem_Applications\/L2_ReactionAnalysis\/Catalytic-Reactions.html\" target=\"_blank\" rel=\"noopener\">https:\/\/www.mt.com\/my\/en\/home\/applications\/L1_AutoChem_Applications\/L2_ReactionAnalysis\/Catalytic-Reactions.html<\/a><\/li><li><a href=\"https:\/\/www.chemguide.co.uk\/physical\/catalysis\/introduction.html\" target=\"_blank\" rel=\"noopener\">https:\/\/www.chemguide.co.uk\/physical\/catalysis\/introduction.html<\/a><\/li><\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Introduction What is a catalyst? A catalyst is a substance that is used to speed up a chemical reaction but it is not consumed by the reaction. What is catalysis? Catalysis is a process of increasing the rate of a chemical reaction by adding a chemical substance which is known as a catalyst. A very &#8230; <a title=\"Catalytic Reactions\" class=\"read-more\" href=\"https:\/\/chemdictionary.org\/catalytic-reactions\/\" aria-label=\"More on Catalytic Reactions\">Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[1],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":4,"star_result":4,"total_max_option_value":5,"adjusted_score_result":4,"score_result":4,"percentage_result":80,"adjusted_percentage_result":80,"count":1,"post_id":1177}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1177"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=1177"}],"version-history":[{"count":6,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1177\/revisions"}],"predecessor-version":[{"id":1319,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1177\/revisions\/1319"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=1177"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=1177"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=1177"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}