First-order reactions: Difference between revisions

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|Meaning=A chemical reaction involving only one chemical species, in which the rate of  decrease of the concentration of the reactant is directly proportional to its concentration.
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|Explanation=The constant of proportionality is the first-order [[rate coefficient]] ''k'', which has units of inverse  time: [[File:ams2001glos-Fex01.gif|link=|ams2001glos-Fex01]], where [''A''] is the concentration of species ''A''. The first-order rate equation  is often expressed in its integrated form, [[File:ams2001glos-Fex02.gif|link=|ams2001glos-Fex02]], where [''A'']<sub>0</sub> is the initial concentration  of species ''A''. A common example of a first-order reaction is a radioactive decay process. In the  [[atmosphere]], [[photolysis]] reactions obey first-order kinetics. Also, unimolecular decomposition  reactions at their high-pressure limit empirically follow first-order kinetics.
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== first-order reactions ==
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<div class="definition"><div class="short_definition">A chemical reaction involving only one chemical species, in which the rate of  decrease of the concentration of the reactant is directly proportional to its concentration.</div><br/> <div class="paragraph">The constant of proportionality is the first-order [[rate coefficient]] ''k'', which has units of inverse  time: <div class="inline-formula">[[File:ams2001glos-Fex01.gif|link=|ams2001glos-Fex01]]</div>, where [''A''] is the concentration of species ''A''. The first-order rate equation  is often expressed in its integrated form, <div class="inline-formula">[[File:ams2001glos-Fex02.gif|link=|ams2001glos-Fex02]]</div>, where [''A'']<sub>0</sub> is the initial concentration  of species ''A''. A common example of a first-order reaction is a radioactive decay process. In the  [[atmosphere]], [[photolysis]] reactions obey first-order kinetics. Also, unimolecular decomposition  reactions at their high-pressure limit empirically follow first-order kinetics.</div><br/> </div>
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Latest revision as of 12:20, 30 March 2024

A chemical reaction involving only one chemical species, in which the rate of decrease of the concentration of the reactant is directly proportional to its concentration.

The constant of proportionality is the first-order rate coefficient k, which has units of inverse time: ams2001glos-Fex01, where [A] is the concentration of species A. The first-order rate equation is often expressed in its integrated form, ams2001glos-Fex02, where [A]0 is the initial concentration of species A. A common example of a first-order reaction is a radioactive decay process. In the atmosphere, photolysis reactions obey first-order kinetics. Also, unimolecular decomposition reactions at their high-pressure limit empirically follow first-order kinetics.

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