MediaWiki API result

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            "*": "Subscribe to the mediawiki-api-announce mailing list at <https://lists.wikimedia.org/postorius/lists/mediawiki-api-announce.lists.wikimedia.org/> for notice of API deprecations and breaking changes."
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            "16382": {
                "pageid": 16382,
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                "title": "Reaction",
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                        "*": "The term reaction refers to an event in which there is an interaction between two or more reactant substances to form a final product.<noinclude>\n\n==Odkazy==\n===Souvisej\u00edc\u00ed \u010dl\u00e1nky===\n*[[Acid-base reactions|Acid-base reaction]]\n*[[Endergonic Reaction|Endergonic reaction]]"
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            "14699": {
                "pageid": 14699,
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                "title": "Reaction Rate",
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                        "*": "<!------------------------------------------------ -------------------------------------------------- --------------\n* EMBEDDED ARTICLE\n* Attention - this article is used by other articles in which it is inserted. Please be careful when editing it:\n* 1. Do not delete <noinclude> </noinclude> statements. They indicate the parts of the article that are not transferred when pasted.\n* 2. Do not change the levels of the headings used. Injudicious use of top-level headings could make other articles confusing.\n* 3. More extensive editing, expansion or shortening of the article could disrupt the concept of other articles. Discuss the changes in the discussion.\n* For a list of articles in which this article is embedded, see the list of referring articles under the \"Links here\" link.\n*\n* Please do not delete this comment. In case of confusion, contact the editors (redakce@wikiskripta.eu)\n*\n* This notice is inserted with the template {{subst:Embedded article}}\n-------------------------------------------------- -------------------------------------------------- ---------->[[Category:Embedded articles]]\n\n[[Chemical kinetics|chemical kinetics]] deals with the study of reaction rate.\n\nIn order for two or more substances to react, their molecules must \"collide\". The probability of a collision increases with increasing temperature, pressure, and [[Concentration|concentration]] of substances.\n\n\"Reaction rate (v)\" can be defined as the rate of \"decrease of reactants\" or the rate of \"increase of products\", i.e. for the reaction a A + b B \u2192 c C + d D:\n\n::<math>v = -\\frac{1}{a} \\cdot \\frac{d[A]}{dt} = -\\frac{1}{b} \\cdot \\frac{d[B]}{ dt} = \\frac{1}{c} \\cdot \\frac{d[C]}{dt} = -\\frac{1}{d} \\cdot \\frac{d[D]}{dt}</math >\n\nLet's take a closer look at the relationship between reaction rate and reactant concentration. Consider a simple reaction X \u2192 Y. Its rate will be proportional to [X] according to the equation:\n\n{| align = right\n| (15)\n|}\n:<math>v = -\\frac{d[X]}{dt} = k \\cdot [X]</math>\n\n\nwhere k is the '''rate constant'''.\n\nIn some cases, the rate may be proportional to [X]<sup>2</sup>, may depend more complexly on [X], or conversely may not depend on [X] at all (in which case the reaction proceeds at a constant rate). The exact relationship between the reaction rate and the concentration of the reactants is an ``empirical fact'' and - especially if we consider reactions with more complex reaction mechanisms - cannot be derived only from the stoichiometry of the observed transformation.\n\nChemists define the ``kinetic order of a reaction'' by the number of terms whose concentrations affect the rate. If the speed does not depend on the concentration, and therefore the equation v = k applies, we speak of the zeroth order. If the rate is directly proportional to the concentration of one of the reactants, it is first-order kinetics (as in the case of the above-mentioned reaction (15)). If the rate is affected by the concentration of two reactants or if it is an exponential relationship of one reactant (v = k \u00b7 [X] \u00b7 [Y] or v = k \u00b7 [X]<sup>2</sup>), we speak of second-order kinetics etc.\n\nSometimes we want to predict how much reactant X will remain unreacted after a time t from the start of the reaction, or how long it will take for [X] to halve. For zero-order reactions, the calculation is simple, but for higher orders it gets complicated.\n\nFor a ''first-order'' reaction:\n\n{| align = right\n| (16)\n|}\n: <math>-\\frac{d[X]}{dt} = k \\cdot [X]</math>\n\nIntegrating equation (16) we get:\n\n: <math>-\\frac{1}{[X]} \\cdot \\frac{d[X]}{dt} = k \\cdot [X]</math>\n\n: <math>-\\int{\\frac{1}{[X]} \\cdot \\frac{d[X]}{dt}} = \\int{k \\cdot [X]}</math>\n\n{| align = right\n| (17)\n|}\n: <math>-ln[X] = k \\cdot t + c</math>\n\n\nBy solving for the beginning of the reaction, i.e. for t = 0 (while we denote the initial concentration of substance X at this time as [X]<sub>0</sub>), we get\n\n{| align = right\n| (18)\n|}\n:<math>c = -ln[X]_0</math>\n\n:<math>-ln[X] = k \\cdot t - ln[X]_0</math>\n\n:<math>-ln[X] + ln[X]_0 = k \\cdot t </math>\n\n:<math>-ln{\\frac{[X]}{[X]_0}} = k \\cdot t </math>\n\n:<math>\\frac{[X]}{[X]_0} = e^{-k \\cdot t} </math>\n\n{| align = right\n| (19)\n|}\n:<math>[X] = [X]_0 \\cdot e^{-k \\cdot t} </math>\n\n\nThis equation describes the '''exponential decay'' of X concentration over time. A useful parameter of exponential decay is the time required to reduce the initial concentration (or amount) of substance X by half. It is called the '''half-time'''' (t<sub>1/2</sub>). From equation (19), we can express the half-time as:\n\n:<math>t_{1/2} = \\frac{ln2}{k}</math>\n\n[[File:Halftime.png|center|300px]]\n\n\n<noinclude>\n{{Navbox - transformation of substances and energy in the cell}}\n</noinclude>\n[[Category:Biochemistry]]\n[[Category:FBLT]]"
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