{"id":20,"date":"2024-04-04T07:30:15","date_gmt":"2024-04-04T04:30:15","guid":{"rendered":"https:\/\/sisu.ut.ee\/huvitavkeemia\/33-keemiline-tasakaal-ja-selle-nihkumine\/"},"modified":"2025-04-01T22:56:14","modified_gmt":"2025-04-01T19:56:14","slug":"33-keemiline-tasakaal-ja-selle-nihkumine","status":"publish","type":"page","link":"https:\/\/sisu.ut.ee\/huvitavkeemia\/33-keemiline-tasakaal-ja-selle-nihkumine\/","title":{"rendered":"3.3. Keemiline tasakaal ja selle nihkumine"},"content":{"rendered":"<h2>Millal saabub tasakaal<\/h2>\n<p style=\"margin-bottom: 11.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Eelmises osas n\u00e4gime, et p\u00f6\u00f6rduvad reaktsioonid v\u00f5ivad kulgeda m\u00f5lemas suunas. V\u00f5tame seekord vaatluse alla \u00fche h\u00fcpoteetilise reaktsiooni <\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11pt; padding-left: 40px;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">A+B <\/span><\/span><\/span><\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\">\u00a0<span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">C+D.<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui l\u00e4hteained A ja B segada, siis hakkab reaktsioon toimuma kiirusega\u00a0 <i>v<\/i><sub>otse<\/sub>. Koolis sa reaktsiooni kiiruse v\u00f5rrandit ei \u00f5pi, aga selguse m\u00f5ttes toome selle siin \u00e4ra. Reaktsiooni kiirust saab arvutada j\u00e4rgmise v\u00f5rrandi abil:<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11pt; margin-left: 40px;\"><span style=\"background: white;\"><i><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">v<\/span><\/span><\/span><\/i><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">otse<\/span><\/span><\/span><\/sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> = <i>k<\/i><sub>otse<\/sub><\/span><\/span><\/span> <span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00d7<\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> c<sub>A<\/sub><i>\u00a0<\/i><\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00d7 <\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00a0c<sub>B<\/sub><\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">kus [A]<\/span><\/span><\/span><i>\u00a0<\/i><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">ja [B]\u00a0on l\u00e4hteainete kontsentratsioonid\u00a0ja\u00a0 <i>k<\/i><\/span><\/span><\/span><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">otse<\/span><\/span><\/span><\/sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> on otsereaktsiooni kiiruskonstant. Kuna l\u00e4hteainete kontsentratsioonid reaktsiooni k\u00e4igus v\u00e4henevad, siis peab j\u00e4relikult v\u00e4henema ka otsereaktsiooni kiirus. <\/span><\/span><\/span><\/span><\/p>\n<h5>Reaktsioon on tasakaaluolekus siis, kui otse- ja p\u00f6\u00f6rdreaktsiooni kiirused on v\u00f5rdsed.\u00a0<br>\u00a0 \u00a0<em>v<\/em><sub>otse<\/sub>\u00a0= <em>v<\/em><sub>p\u00f6\u00f6rd<\/sub><\/h5>\n<p>Kuna saadusi tekib j\u00e4rjest juurde, siis hakkab toimuma ka p\u00f6\u00f6rdreaktsioon kiirusega <i>v<\/i><sub>p\u00f6\u00f6rd<\/sub>.\u00a0 P\u00f6\u00f6rdreaktsiooni kiiruse saame avaldada:<\/p>\n<p style=\"margin-bottom: 11pt; margin-left: 40px;\"><span style=\"background: white;\"><i><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">v<\/span><\/span><\/span><\/i><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">p\u00f6\u00f6rd\u00a0<\/span><\/span><\/span><\/sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">= <i>k<\/i><sub>p\u00f6\u00f6rd <\/sub><\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00d7<\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00a0 c<sub>C<\/sub><i>\u00a0<\/i><\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00d7<\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> c<sub>D<\/sub><\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">P\u00f6\u00f6rdreaktsioon on alguses aeglane, sest saadusi on v\u00e4he, kuid aja jooksul p\u00f6\u00f6rdreaktsiooni kiirus j\u00e4rjest kasvab, kuni saab v\u00f5rdseks otsereaktsiooni kiirusega:<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11pt; margin-left: 40px;\"><span style=\"background: white;\"><i><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">v<\/span><\/span><\/span><\/i><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">otse<\/span><\/span><\/span><\/sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00a0 = <i>v<\/i><sub>p\u00f6\u00f6rd<\/sub> <\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 11.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">ning <strong>reaktsioon on saavutanud tasakaaluoleku. <\/strong><\/span><\/span><\/span><\/span><\/p>\n<h2>Kui tasakaal on saabunud, kas siis reaktsioon enam ei toimu<\/h2>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"background: white;\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui tasakaaluolek on saabunud, siis l\u00e4hteainete ja saaduste kontsentratsioonid enam ei muutu. \u00c4sja kirjutasime v\u00f5rduse juhuks, kui otse- ja p\u00f6\u00f6rdreaktsiooni kiirused on v\u00f5rdsed. Kuna need kiirused kumbki ei ole nullid, siis peavad reaktsioonid m\u00f5lemas suunas edasi toimuma.\u00a0Sellist n\u00e4htust nimetatakse <strong>d\u00fcnaamiliseks tasakaaluks<\/strong>.<\/span><\/span><\/span><\/span><\/span><\/p>\n<h2>Kas tasakaaluolekut saab millegagi m\u00f5jutada<\/h2>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">N\u00fc\u00fcd vaatame, kuidas reaktsiooni tasakaalu m\u00f5jutada, n\u00e4iteks et saada tasakaalulisest reaktsioonist rohkem saadusi.<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt; text-align: center;\"><\/p><div class=\"ratio ratio-16x9 mb-3\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--16x9\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n<h6 style=\"margin-bottom: 12pt; text-align: center;\"><em><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Allikas:\u00a0<\/span><\/span><\/span><\/span><a title=\"\" href=\"https:\/\/youtu.be\/RqpanAUUDNw\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/youtu.be\/RqpanAUUDNw\">https:\/\/youtu.be\/RqpanAUUDNw<\/a><\/em><\/h6>\n<h3>Kontsentratsiooni m\u00f5ju<\/h3>\n<h5>Kui lisada l\u00e4hteaineid, siis nihkub tasakaal saaduste suunas, sest tasakaalukonstant ei muutu.<\/h5>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Vaatame \u00fcldist reaktsiooni <\/span><span style=\"color: black;\">A+B <\/span><\/span><\/span><\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> C+D.<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui tasakaalulisele s\u00fcsteemile lisada \u00fchte (v\u00f5i m\u00f5lemat) l\u00e4hteainet (A-d ja v\u00f5i B-d), siis otsesuunalise reaktsiooni kiirus kasvab ning s\u00fcsteem ei ole enam tasakaaluolekus. Reaktsiooni k\u00e4igus hakkavad A ja B kontsentratsioonid v\u00e4henema ning C ja D kontsentratsioonid suurenema: reaktsioon toimub p\u00e4risuunas edasi, kuni saabub taas tasakaal ehk otse- ja p\u00f6\u00f6rdprotsessi kiirused v\u00f5rdsustuvad. <\/span><\/span><\/span><\/span><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Samuti kui eemaldada reaktsiooni saadusi (C-d ja v\u00f5i D-d) tekib eelnimetatuga analoogne olukord ning otsesuunalise reaktsiooni kiirus kasvab ja tasakaaluolek l\u00f5ppeb.<\/span><\/span><\/span><\/span><\/p>\n<h3>R\u00f5hu m\u00f5ju<\/h3>\n<h5>Kui r\u00f5hku suurendada, siis nihkub reaktsioon selles tekke suunas, kus on v\u00e4hem gaasimolekule.<\/h5>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">R\u00f5hu muutus m\u00f5jutab selliseid reaktsioone, milles gaasi moolide arv muutub. Kui reaktsioonisegu <\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt; padding-left: 40px;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">N<sub>2<\/sub>O<sub>4<\/sub><\/span><\/span><\/span>(g) <\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> 2NO<sub>2<\/sub>(g)<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">r\u00f5hku suurendada, siis nihkub tasakaal N<sub>2<\/sub>O<sub>4<\/sub> tekke suunas, mille tulemusena hakkab gaasisegu r\u00f5hk v\u00e4henema, sest reaktsiooniv\u00f5rrandi vasakul pool on v\u00e4hem gaasimolekule.<\/span><\/span><\/span><\/span><\/p>\n<h3>Temperatuuri m\u00f5ju<\/h3>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Temperatuuri m\u00f5ju hindamiseks vaata allolevat joonist ja p\u00fc\u00fca selgitada, kas reaktsioon N<sub>2<\/sub>O<sub>4<\/sub><\/span><\/span><\/span> <\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> 2NO<\/span><\/span><\/span><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">2 <\/span><\/span><\/span><\/sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">on endo- v\u00f5i eksotermiline? Vasakul on ampull gaasiseguga paigutatud j\u00e4\u00e4sse, keskel on j\u00e4\u00e4 ja vee segus (st null kraadi juures) ja paremal on ampull toatemperatuuril. <\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt; text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1368\" height=\"910\" class=\"wp-image-106 aligncenter\" style=\"width: 600px; height: 399px;\" title=\"screenshot_2022-03-25_at_14.38.50.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_14.38.50.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_14.38.50.png 1368w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_14.38.50-300x200.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_14.38.50-1024x681.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_14.38.50-768x511.png 768w\" sizes=\"auto, (max-width: 1368px) 100vw, 1368px\"><\/p>\n<h6 style=\"text-align: center;\">Joonis 1. N<sub>2<\/sub>O<sub>4<\/sub>\u00a0\u21c4\u00a02NO<sub>2<\/sub> reaktsioon erinevatel temperatuuridel. A) reaktsioonisegu on asetatud kuivaj\u00e4\u00e4sse, B) reaktsioonisegu on 0 <sup>o<\/sup>C juures, C) reaktsioonisegu on toatemperatuuril. Allikas: <a title=\"\" href=\"https:\/\/www.unf.edu\/~michael.lufaso\/chem2046\/2046chapter15.pdf\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/www.unf.edu\/~michael.lufaso\/chem2046\/2046chapter15.pdf\">https:\/\/www.unf.edu\/~michael.lufaso\/chem2046\/2046chapter15.pdf<\/a><\/h6>\n<h5>Endotermilise reaktsiooni tasakaalukonstant suureneb, kui temperatuuri t\u00f5sta.<\/h5>\n<p><span style=\"background: white;\"><span lang=\"et\"><span style=\"background: white;\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui temperatuuri t\u00f5sta, siis reaktsiooni tasakaal nihkub paremale ehk saaduste suunas. J\u00e4relikult on see reaktsioon endotermiline. <\/span><\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">V\u00f5ib-olla on temperatuuri m\u00f5just kergem aru saada, kui reaktsioon kirjutada tavap\u00e4rasest veidi erinevalt, arvestades, et endotermiline \u0394H &gt; 0 reaktsioon tarbib soojust:<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt; margin-left: 40px;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">N<sub>2<\/sub>O<sub>4<\/sub><\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00a0 (soojus) <\/span><\/span><\/span><\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> 2NO<\/span><\/span><\/span><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">2<\/span><\/span><\/span><\/sub> \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/p>\n<h5>Le Chatelier\u2019 printsiip:\u00a0kui mingi v\u00e4lism\u00f5ju (temperatuuri, kontsentratsiooni v\u00f5i r\u00f5hu muutmine) rikub keemilist tasakaalu, siis kulgeb selle m\u00f5ju tagaj\u00e4rgi v\u00e4hendav reaktsioon, mis viib s\u00fcsteemi \u00fcle uude tasakaaluolekusse.<\/h5>\n<p><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui temperatuuri t\u00f5stame, siis lisame reaktsioonisegusse soojust juurde ja endotermiline reaktsioon nihkub saaduse suunas ehk NO<sub>2<\/sub> tekke suunas.<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Tavaliselt lisatakse vajadusel viide soojusefektile selliselt:<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12pt; margin-left: 40px;\"><span style=\"background: white;\">\u00a0<span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">N<sub>2<\/sub>O<sub>4<\/sub><\/span><\/span><\/span><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u00a0<\/span><\/span><\/span><\/span><img loading=\"lazy\" decoding=\"async\" width=\"76\" height=\"62\" class=\"alignnone wp-image-95\" style=\"width: 16px; height: 13px;\" title=\"kaks-noolt.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/kaks-noolt.png\" alt=\"nool\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\"> 2NO<\/span><\/span><\/span><sub><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">2<\/span><\/span><\/span><\/sub>\u00a0\u00a0<span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">\u0394H &gt; 0<\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Eksotermilises reaktsioonis soojus eraldub (soojus on saaduste hulgas). Kui t\u00f5sta eksotermilise reaktsiooni temperatuuri, siis nihkub tasakaal l\u00e4hteaine tekke suunas. <\/span><\/span><\/span><\/span><\/p>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\">K\u00f5ik n<span style=\"color: black;\">eed n\u00e4htused v\u00f5tab kokku Le Chatelier\u2019 printsiip:\u00a0<\/span><\/span><\/span><\/span><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Kui mingi v\u00e4lism\u00f5ju (temperatuuri, kontsentratsiooni v\u00f5i r\u00f5hu muutmine) rikub keemilist tasakaalu, siis kulgeb selle m\u00f5ju tagaj\u00e4rgi v\u00e4hendav reaktsioon, mis viib s\u00fcsteemi \u00fcle uude tasakaaluolekusse.<\/span><\/span><\/span><\/span><\/p>\n<p><span style=\"color: #000000;\">Kui p\u00e4risuunaline reaktsioon on eksotermiline (\u0394H &lt; 0, reaktsiooni toimumisel soojust eraldub ja \u00fcmbritseva keskkonna temperatuur kasvab), siis vastassuunaline reaktsioon on endotermiline (\u0394H &gt; 0, reaktsiooni toimumisel soojust neeldub ja \u00fcmbritseva keskkonna temperatuur v\u00e4heneb). Kui eksotermilise reaktsiooni korral t\u00f5stetakse temperatuuri, siis reaktsioon nihkub just endotermilise reaktsiooni ehk l\u00e4hteainete tekkimise suunas, sest endotermilise reaktsiooni k\u00e4igus temperatuur langeb. Ehk siis vastavalt Le Chatelier\u2019 printsiibile nihkub tasakaal nii, et v\u00e4lism\u00f5ju oleks v\u00e4ikseim.<\/span><\/p>\n<h2>Kas katal\u00fcsaator m\u00f5jutab tasakaalu<\/h2>\n<h5>Katal\u00fcsaator kiirendab reaktsiooni, kuid ei muuda reaktsiooni tasakaaluolekut.<\/h5>\n<p style=\"margin-bottom: 12.0pt;\"><span style=\"background: white;\"><span lang=\"et\"><span style=\"line-height: 115%;\"><span style=\"color: black;\">Katal\u00fcsaatori manulusel toimub reaktsioon sellist teed pidi, kus reaktsiooni aktivatsioonienergia on madalam. Reaktsioon saavutab tasakaaluoleku kiiremini, alaneb nii otse- kui ka p\u00f6\u00f6rdreaktsiooni aktivatsioonienergia barj\u00e4\u00e4r ning tasakaal ei muutu, sest l\u00e4hte- ja l\u00f5ppolek j\u00e4\u00e4vad samaks.<\/span><\/span><\/span><\/span><\/p>\n<p><\/p><div class=\"accordion mb-3\">\n        <div class=\"accordion-item accordion-item--white\">\n        <h2 class=\"accordion-header\" id=\"accordion-69dc4693786a2-heading\">\n            <button class=\"accordion-button collapsed\" type=\"button\" data-bs-toggle=\"collapse\" data-bs-target=\"#accordion-69dc4693786a2-collapse\" aria-expanded=\"true\" aria-controls=\"accordion-69dc4693786a2-collapse\">\u00dclesanne 1<\/button>\n        <\/h2>\n        <div id=\"accordion-69dc4693786a2-collapse\" class=\"accordion-collapse collapse\" aria-labelledby=\"accordion-69dc4693786a2-heading\">\n            <div class=\"accordion-body\">\n\n\n<div class=\"h5p-iframe-wrapper\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--fixed\" style=\"height: 366px;\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n\n\n<p><\/p><\/div>\n        <\/div>\n        <\/div>\n    <\/div>","protected":false},"excerpt":{"rendered":"<p>Millal saabub tasakaal Eelmises osas n\u00e4gime, et p\u00f6\u00f6rduvad reaktsioonid v\u00f5ivad kulgeda m\u00f5lemas suunas. V\u00f5tame seekord vaatluse alla \u00fche h\u00fcpoteetilise reaktsiooni A+B \u00a0C+D. Kui l\u00e4hteained A ja B segada, siis hakkab reaktsioon toimuma kiirusega\u00a0 votse. Koolis sa reaktsiooni kiiruse v\u00f5rrandit ei &#8230;<\/p>\n","protected":false},"author":269,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"_acf_changed":false,"inline_featured_image":false,"footnotes":""},"class_list":["post-20","page","type-page","status-publish","hentry"],"acf":[],"_links":{"self":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/20","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/users\/269"}],"replies":[{"embeddable":true,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/comments?post=20"}],"version-history":[{"count":9,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/20\/revisions"}],"predecessor-version":[{"id":1079,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/20\/revisions\/1079"}],"wp:attachment":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/media?parent=20"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}