{"id":1209,"date":"2015-12-03T15:16:59","date_gmt":"2015-12-03T15:16:59","guid":{"rendered":"http:\/\/www.oxidationtech.com\/blog\/?p=1209"},"modified":"2015-12-01T15:23:14","modified_gmt":"2015-12-01T15:23:14","slug":"ozone-reactions-with-chemical-compounds","status":"publish","type":"post","link":"https:\/\/www.oxidationtech.com\/blog\/ozone-reactions-with-chemical-compounds\/","title":{"rendered":"Ozone reactions with chemical compounds"},"content":{"rendered":"

Many organic and inorganic compounds react with ozone. These reactions can vary greatly depending upon the state of ozone (gaseous or aqueous), and the other chemicals involved in the reaction.<\/strong><\/p>\n

Below is an outline of basic chemical reactions between ozone and certain compounds. This is for reference only, as there are many other variables involved in actual processes. However, this data is helpful as a baseline to understand the fundamentals of ozone reactions and oxidation in general.<\/strong><\/p>\n

Click HERE for info on ozone effect on pathogens<\/strong><\/a><\/em><\/p>\n

For additional details or help with any potential reactions\u00a0<\/span>please contact our application engineers for help!<\/a><\/p>\n

ACIDS, ALCOHOLS, ALDEHYDES, AND KETONES<\/em>.<\/strong><\/h2>\n

ACETIC ACID<\/strong>, Formula: CH3COOH
\nReaction with Ozone: C2H402\u00a0<\/span>+ 4 03\u00a0<\/span>—-> 2 C02\u00a0 +\u00a0 2 H2O +\u00a0 4 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 2<\/p>\n

ACETONE<\/strong>, Formula: CH3COCH3,
\nReaction with Ozone: C3H6O + 8 03\u00a0<\/span>—-> 3 C02\u00a0<\/span>+ 3 H2O + 8 O2 .\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 4<\/p>\n

n-BUTYL ACETATE<\/strong>\u00a0<\/span>Formula C6H12O2.
\nReaction with Ozone: C6H12O2\u00a0<\/span>+ 16 O3\u00a0<\/span>—-> 6 C02\u00a0<\/span>+ 6 H2O\u00a0 +\u00a0 16 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 8<\/p>\n

BUTOXYETHANOL<\/strong>\u00a0<\/span>Fonnula: C6HI4O2.
\nReaction wtih Ozone: C6HI4O2\u00a0<\/span>+ 17 O3\u00a0<\/span>—- > 6 CO2\u00a0<\/span>\u00a0 + 7 H2O +\u00a0 4 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 20.5<\/p>\n

CETYL AlCOHOL<\/strong>\u00a0<\/span>Formula CH3(CH2)15 OH
\nReaction with Ozone: CH3(CH2)15 OH + 48 03\u00a0<\/span>—-> 16 CO2\u00a0<\/span>+ 17 H2O + 4 O2\u00a0<\/span>. Number of O2molecules consumed per molecule of compound = 24<\/p>\n

FORMALDEHYDE<\/strong>Formula HCHO
\nReaction with Ozone: HCHO + 2 O3\u00a0<\/span>—-> C02\u00a0<\/span>+ H2O + 2 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 1<\/p>\n

ISOPROPYL ALCOHOL<\/strong>\u00a0<\/span>Fornula CH3CHOHCH5
\nReaction with Ozone: CH3CHOHCH5\u00a0<\/span>+\u00a0 9 O3\u00a0<\/span>—- > 3 CO2\u00a0<\/span>+ 4 H2O + 9 O2\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 4.5<\/p>\n

GLYCEROL<\/strong>\u00a0<\/span>Formula CH2OHCHOHCH2OH
\nReaction with Ozone: CH2OHCHOHCH2OH + 7 O3\u00a0<\/span>—- > 3C02\u00a0<\/span>+ 4H2O + 7 O2\u00a0 Number of O2molecules consumed per molecule of compound = 4.5<\/p>\n

METHACRYLIC ACID<\/strong>(glacial) Formula CH2C (CH3) COOH
\nReaction wtih Ozone: CH2C (CH3) COOH + 9 O3\u00a0<\/span>—- > 4 CO2\u00a0<\/span>+ 3 H20 + 9 O2\u00a0<\/span>. Number of O2\u00a0molecules consumed per molecule of compound = 4.5<\/p>\n

METHYL-ETHYL-KETONE<\/strong>\u00a0<\/span>Formula CH3COC2H5.
\nReaction wtih Ozone: CH3COC2H5\u00a0<\/span>+ 11 O3\u00a0<\/span>—- > 4C02\u00a0<\/span>+ 4 H2O + 11 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 5.5<\/p>\n

PROPYLENE GLYCOL<\/strong>\u00a0<\/span>Formula C3H8O2.
\nReaction wtih Ozone: C3H8O2\u00a0<\/span>+ 8 O3\u00a0<\/span>—- > 3 CO2\u00a0<\/span>+ 4 H2O + 8 O2\u00a0 Number of O2\u00a0\u00a0<\/span>molecules consumed per molecule of compound = 4<\/p>\n

\nAROMATIC COMPOUNDS<\/em><\/strong><\/h2>\n

BENZENE<\/strong>Formula C6H6
\nReaction with Ozone C6H6\u00a0<\/span>+ 11 O3\u00a0<\/span>—- > 6C02\u00a0<\/span>+ 3 H2O + 11 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 5.5<\/p>\n

BENZYL ALCOHOL<\/strong>.\u00a0<\/span>Formula C6H5CH2OH
\nReaction wtih Ozone. C6H5CH2OH + 17 O3\u00a0<\/span>—-> 7 C02\u00a0<\/span>+ 4 H20 + 17 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 8.5<\/p>\n

N.BUTYL PHTHALATE<\/strong>\u00a0<\/span>Formula CI2H14O4.
\nReaction with Ozone:\u00a0 CI2H14O4\u00a0<\/span>+ 27 O3—-> 12 C02\u00a0<\/span>+ 7 H20 + 27 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 13.5<\/p>\n

CAMPHOR<\/strong>Formula C10H16O
\nReaction Wlih Ozone: C10H16O + 27 O3\u00a0<\/span>—- > 10 C02\u00a0<\/span>+ 8 H2O + 27 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 13.5<\/p>\n

PARA-PHENYLENEDIAMINE<\/strong>\u00a0 Formula C6H8N2
\nReaction with Ozone: C6H8N2\u00a0<\/span>+ 16 O3\u00a0<\/span>—-> 6 C02\u00a0<\/span>+ 4 H2O + N2\u00a0<\/span>+ 16 O2\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 8<\/p>\n

RESORCINOL<\/strong>Formula C6H6O2
\nReaction with Ozone: C6H6O2\u00a0<\/span>+ 13 O3\u00a0<\/span>—-> 6 C02\u00a0<\/span>+ 3 H20 + 13 O2\u00a0 Number of O2\u00a0<\/span>\u00a0 molecules consumed per molecule of compound = 6.5<\/p>\n

STYRENE<\/strong>\u00a0<\/span>Formula:C6H5CHCH2\u00a0<\/span>
\nReaction with Ozone: C6H5CHCH2\u00a0 + 20 O3\u00a0<\/span>—- > 8 C02\u00a0<\/span>+ 4 H2O + 20 O2\u00a0<\/span>. Number of O2molecules consumed per molecule of compound = 10<\/p>\n

TRICRESYL<\/strong>\u00a0<\/span>Formula C21H21PO4.
\nReaction with Ozone C21H21PO4.. + 102 O3\u00a0<\/span>—- > 42 C02\u00a0<\/span>+ 21 H2O + P2O5\u00a0<\/span>+ 102 O2\u00a0<\/span>Number of O2 molecules consumed per molecule of compound = 51<\/p>\n

TOULENE<\/strong>\u00a0<\/span>Formula C6H5CH3.
\nReactlon with Ozone: C6H5CH3\u00a0<\/span>.+ 18 O3\u00a0<\/span>—-> 7 CO2\u00a0<\/span>+ 4 H2O + 18 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule ot compound = 9<\/p>\n

XYLENE<\/strong>\u00a0<\/span>Formula C6H4(CH3)2
\nReaction with Ozone C6H4(CH3)2\u00a0 + 21 O3\u00a0<\/span>—-> 8 CO2\u00a0<\/span>+ 5 H2O + 21 O2\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 10.5<\/p>\n

\nALIPHATIC COMPOUNDS<\/i><\/em><\/strong><\/h2>\n

BUTANE<\/strong>\u00a0<\/span>Formula C4H10
\nReaction with Ozone: C4H10\u00a0<\/span>+ 13 O3\u00a0<\/span>—-> 4 CO2\u00a0<\/span>+ 5 H2O + 13 O2\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 6.5<\/p>\n

ISOBUTANE.<\/strong>\u00a0<\/span>Formula (CH3)3CH (need to check for accuracy)<\/p>\n

LIQUEFIED PETROLEUM GAS<\/strong>\u00a0<\/span>[LPG] General Formula CnH2N+2. Both LPG (Liquefied petroleum gas) is a mixture of aliphatic, saturated hydrocarbons, therefore only a generic formula was used to describe the reaction with Ozone .
\nReaction wtih Ozone: CnH2N+2\u00a0<\/span>+ O3\u00a0<\/span>—- > nC02\u00a0<\/span>+ (n+1) H2O + O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound: 3\/2 n + 1\/2 O<\/p>\n

MINERAL SPIRITS<\/strong>\u00a0<\/span>General Formula Cn H2n+2\u00a0<\/span>
\nMineral spirits are mixtures of aliphatic, saturated hydrocarbons, therefore only a generic formula was used to describe the reaction with Ozone. Reaction wtih Ozone: Cn H2n+2\u00a0 + O3\u00a0<\/span>—- > nCO2\u00a0<\/span>+ (n+ 1) H2O + O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound: 3\/2 n + 1\/2 O<\/p>\n

PROPANE<\/strong>\u00a0<\/span>Formula C3H8
\nReaction wtih Ozone: C3H8\u00a0<\/span>+ 10 O3\u00a0<\/span>:—-> 3CO2\u00a0<\/span>+ 4 H2O + 10 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 5<\/p>\n

\nCHLORIDES<\/em><\/strong><\/h2>\n

Chlorides are organic compounds which have one or more chlorine atoms in their structure. These compounds react with Ozone to produce hypochloride which in turn decompose to produce chloride and release oxygen, as shown in the following reaction: CL2O —- > 2CL-1\u00a0<\/span>+ 1\/2 O2<\/p>\n

METHYLENE CHLORIDE<\/strong>\u00a0<\/span>(Dichloromethane), Formula CH2CL2
\nReaction with Ozone: 2CH2CL2\u00a0<\/span>+ 4 O3\u00a0<\/span>—- > CO2 + H2O + CL2O + 4 O Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 1<\/p>\n

CHLOROFORM<\/strong>,\u00a0<\/span>Formula CHCL3.
\nReaction wtih Ozone: 6 CHCL3\u00a0<\/span>+ 6 O3\u00a0<\/span>— > 6 CO2\u00a0<\/span>+ 3 H2O + 9 CL2O Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 2\/9 O<\/p>\n

METHYL CHLOROFORM<\/strong>,\u00a0<\/span>Formula CH3CCL3
\nReaction with Ozonee: 2CH3CCL3\u00a0<\/span>+ 14 O3\u00a0<\/span>—- > 4 CO2\u00a0<\/span>+ 3 H2O + 3 CL2O + 14 O2\u00a0<\/span>Number of O2molecules consumed per molecule of compound = 3.5<\/p>\n

PERCHLOROETHYLENE<\/strong>Formula CCL2CCL2
\nReaction with Ozone: CCL2CCL2\u00a0<\/span>+ 6 O3\u00a0<\/span>—- > 2 CO2\u00a0<\/span>+ 2 CL2O +\u00a0 6 O2\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 1.5<\/p>\n

TRICHLOROETHYLENE<\/strong>Formula CHCLCCL2
\nReaction with Ozone: 2 CHCLCCL2\u00a0<\/span>+ 12 O3\u00a0<\/span>—- > 4 CO2\u00a0<\/span>+ H2O + 3 CL2O + 12 O2\u00a0<\/span>. Number of O2molecules consumed per molecule of compound = 3<\/p>\n

\nNITROGEN CONTAINING COMPOUNDS<\/em><\/strong><\/h2>\n

HYDROGEN CYANIDE<\/strong>\u00a0<\/span>Formula HCN
\nReaction with Ozone: 2HCN + 5 O3\u00a0<\/span>—- > 2 CO2\u00a0<\/span>+ H2O + N2\u00a0<\/span>+ 5 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 1.25<\/p>\n

AMINO PHENOL<\/strong>\u00a0<\/span>General Formula CH3C6H4NH2\u00a0<\/span>(need to check for accuracy)<\/p>\n

AMMONIA<\/strong>. Formula NH3
\nReaction with Ozone: 2NH3\u00a0<\/span>+ 3 O3\u00a0<\/span>—-> N2 + 3 H20 + 3 O2 .\u00a0<\/span>Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 0.75<\/p>\n

AMMONIUM HYDROXIDE<\/strong>Formuta NH4OH
\nReaction with Ozone: 2NH4OH +3 O3\u00a0<\/span>—-> N2\u00a0<\/span>+5 H2O + 3 O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 0.75<\/p>\n

BENZOPMETHYLENE CHLORIDECHLOROFORM,METHYL CHLOROFORM,PERCHLOROETHYLENETRICHLOROETHYLENEHYDROGEN CYANIDEAMINO PHENOLAMMONIAAMMONIUM HYDROXIDE Formula C<\/strong>20<\/strong>H<\/strong>12<\/strong>
\nYRENE<\/strong>\u00a0<\/span>Formula C20H12
\nReaction with Ozone: 3C20H12\u00a0<\/span>+ 46 O3\u00a0<\/span>—- > 60 CO2\u00a0<\/span>+ 18 H2O . Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 17<\/p>\n

EDTA<\/strong>\u00a0<\/span>(Ethylene Diamine Tetracetic Acid) Formula C10H16N2O8
\nReaction with Ozone: C10H16N2O8\u00a0<\/span>+ 20 O3\u00a0<\/span>—- > 10 CO2\u00a0<\/span>+ 8 H2O + N2\u00a0<\/span>+ 2 O2\u00a0<\/span>[possible error, original document listed “2 CO2” at the end, but it didn’t make sense to me]. Number of O2molecules consumed per molecule of compound = 30<\/p>\n

ETHANOLAMINE<\/strong>\u00a0<\/span>Formula NH2CH2CH2OH
\nReaction with Ozone: 2NH2CH2CH2OH + 13 O3\u00a0<\/span>—- > 4 CO2\u00a0<\/span>+ 7 H2O + 13 O2\u00a0<\/span>+ N2\u00a0<\/span>. Number of O2molecules consumed per molecule of compound: = 3.25<\/p>\n

PHENACETIN<\/strong>.\u00a0<\/span>Formula CH3CONHC6H4OC2H5.
\nReaction with Ozone : CH3CONHC6H4OC2H5.\u00a0<\/span>+ 49 O3\u00a0<\/span>.—- > 20 CO2\u00a0<\/span>+ 13 H2O + N2\u00a0<\/span>+ 49 O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 24.5<\/p>\n

\nSULFUR CONTAINING COMPOUNDS<\/em><\/strong><\/h2>\n

These compounds react with OZONE to produce sulfur trioxide (S03), which in the presence of water forms\u00a0<\/span>sulfuric acid<\/strong>, a strong mineral acid.<\/p>\n

AMMONIUM PERSULFATE<\/strong>Formula (NH4)2S2O8
\nPersulfuric acid (H2S2O8) is a very unstable acid which releases oxygen upon exposure to heat. Its decomposition product is\u00a0<\/span>sulfuric acid<\/strong>\u00a0<\/span>(H2S04) a very strong mineral acid.<\/p>\n

Reaction with Ozone: (NH4)2S2O8\u00a0<\/span>+ 3 O3\u00a0<\/span>—- >N2\u00a0<\/span>+ H2S2O8\u00a0<\/span>+ 3 H2O + 3 O2\u00a0 Number of O2molecules consumed per molecule of compound = 1\/5 O<\/p>\n

AMMONIUM THlIOGLYCOLATE<\/strong>\u00a0<\/span>Formula NH2COCH2SH
\nReaction with Ozone: [possible error] 2C2H5SNO + 17 O3\u00a0<\/span>—->4\u00a0 C02\u00a0<\/span>+ 5 H2O + N2\u00a0<\/span>+ 2SO3\u00a0<\/span>+ 17 O2\u00a0<\/span>Number of O2 molecules consumed per molecule of compound = 2<\/p>\n

SODIUM BISULFITE<\/strong>Formula NaHS03.
\nReaction with Ozone: NaHS03\u00a0<\/span>+ O3\u00a0<\/span>—- > NaHSO4\u00a0<\/span>+ O2\u00a0 Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 1.5<\/p>\n

THIOGLYCOLIC ACID<\/strong>\u00a0<\/span>Fonnula HSCH2COOH
\nReaction with Ozone: HSCH2COOH + 7 O3\u00a0<\/span>—- > 2 CO2\u00a0<\/span>+ 2 H2O + S03\u00a0<\/span>+ 7 O2\u00a0<\/span>. Number of O2molecules consumed per molecule of compound = 3.5<\/p>\n

\nOTHER<\/em><\/strong><\/h2>\n

ALKYLATED SILICATES<\/strong>\u00a0<\/span>General Formula (RnSiO)m. These silicates produce SILICA (silicon dioxide) which is considered a respiratory hazard<\/p>\n

Reaction with Ozone: (RnSiO)m\u00a0<\/span>+ O3\u00a0<\/span>—- > CO2\u00a0<\/span>+ H2O + SiO2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 4 5m<\/p>\n

NON-IONIC DETERGENTS<\/strong>\u00a0<\/span>Formula CxHy\u00a0<\/span>, Non-ionic detergents do not have a generic formula. therefore the formula CxHy\u00a0<\/span>is used to define this class of compounds.<\/p>\n

Reaction with Ozone: CxHy\u00a0<\/span>+ O3\u00a0<\/span>— > CO2\u00a0<\/span>+ H2O + O2\u00a0<\/span>. Number of O2\u00a0<\/span>molecules consumed per molecule of compound = 6x + 1.5y<\/p>\n

HYDROGEN PEROXIDE<\/strong>Formula H2O2<\/p>\n

Reaction with Ozone:\u00a0<\/span><\/em>H<\/em>2<\/em>O<\/em>2<\/em>\u00a0<\/span>+ O<\/em>3<\/em>\u00a0<\/span>—- > O<\/em>2<\/em>\u00a0<\/span>+\u00a0<\/span><\/em>2OH<\/em>–<\/sup><\/em>\u00a0<\/sup><\/em>The\u00a0<\/span>combination of Ozone and Hydrogen Peroxide<\/a>\u00a0<\/span>is an\u00a0<\/span>Advanced Oxidation Process<\/a>, that creates the\u00a0<\/span>OH-, an oxidant more powerful that ozone alone.<\/a><\/strong><\/em><\/em><\/p>\n

 <\/p>\n

NON-REACTIVE COMPOUNDS\u00a0<\/span><\/em><\/strong>The following compounds do\u00a0<\/span>not<\/strong>\u00a0<\/span>react with OZONE.<\/p>\n

CALCIUM OXIDE<\/strong>\u00a0<\/span>Formula CaO
\nPHOSPHORIC ACID<\/strong>\u00a0<\/span>Formula H3PO4
\nPOTASSIUM PERSULFATE<\/strong>. Formula K2S2O5
\nSILICAS<\/strong>Formula SiO2
\nSODIUM BROMATE<\/strong>Formula NaBrO3
\nSODIUM PERSULFATE<\/strong>Formula Na2S2O5
\nSTRONTIUM PEROXIDE<\/strong>\u00a0<\/span>Formula SrO2
\nTETRASODIUM PYROPHOSPHATE<\/strong>\u00a0<\/span>Formula Na4P2O7
\nTITANIUM DIOXIDE<\/strong>\u00a0<\/span>Formula TiO2
\nCARBON TETRACHLORIDE<\/strong>(low temperature)Formula CLC4<\/p>\n

Reference: https:\/\/www.oxidationtech.com\/ozone\/ozone-reactions.html<\/p>\n","protected":false},"excerpt":{"rendered":"

Many organic and inorganic compounds react with ozone. These reactions can vary greatly depending upon the state of ozone (gaseous or aqueous), and the other […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"aside","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"var(--ast-global-color-4)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[3],"tags":[493,494,495],"class_list":["post-1209","post","type-post","status-publish","format-aside","hentry","category-tech-tips","tag-ozone-reactions","tag-ozone-reactions-with-chemicals","tag-stoichiometric-ozone-reactions","post_format-post-format-aside"],"_links":{"self":[{"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/posts\/1209","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/comments?post=1209"}],"version-history":[{"count":1,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/posts\/1209\/revisions"}],"predecessor-version":[{"id":1210,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/posts\/1209\/revisions\/1210"}],"wp:attachment":[{"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/media?parent=1209"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/categories?post=1209"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.oxidationtech.com\/blog\/wp-json\/wp\/v2\/tags?post=1209"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}