Lei de ação das massas: diferenças entre revisões
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In biochemistry, there has been significant interest in the appropriate mathematical model for chemical reactions occurring in the intracellular medium. This is in contrast to the initial work done on chemical kinetics, which was in simplified systems where reactants were in a relatively dilute, ph-buffered, aqueous solution. In more complex environments, where bound particles may be prevented from disassociation by their surroundings, or diffusion is slow or anomalous, the model of mass action does not always describe the behavior of the reaction kinetics accurately. Several attempts have been made to modify the mass action model, but consensus has yet to be reached. Popular modifications replace the rate constants with functions of time and concentration. As an alternative to these mathematical constructs, one school of thought is that the mass action model can be valid in intracellular environments under certain conditions, but with different rates than would be found in a dilute, simple environment {{Fact|date=July 2007}}.
The fact that Guldberg and Waage developed their concepts in steps from 1864 to 1867 and 1879 has resulted in much confusion in the literature as to which equation the Law of Mass Action refers. It has been a source of some textbook errors.<ref>"Textbook errors IX: More About the Laws of Reaction Rates and of Equilibrium", E.A. Guggenheim, ''J. Chem. Ed''., (1956) '''33''', 544-545</ref> Thus, today the "law of mass action" sometimes refers to the (correct) equilibrium constant formula<ref>[http://www.chem.purdue.edu/gchelp/gloss/lawmaction.html Law of Mass Action
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<ref>http://www.chem.sc.edu/goode/C112Web/CH14NF/sld007.htm</ref>
<ref>[http://www.luc.edu/faculty/afitch/chap13/sld011.htm The Law of Mass Action
--> <!-- Bot generated title --> <!-- ]</ref> <ref>http://funnel.sfsu.edu:16080/courses/geol480/lectures/lecture4.pdf</ref>
<ref>[http://www.chemistry.wustl.edu/~courses/genchem/Tutorials/Buffers/fundamental.htm Recap of FundamentRecap of Fundamental Acid-Base Concepts
--> <!-- Bot generated title --> <!-- ]</ref> <ref>[http://www.chm.davidson.edu/ChemistryApplets/equilibria/BasicConcepts.html Chemical Equilibria: Basic Concepts
--> <!-- Bot generated title --> <!-- ]</ref> <ref>[http://www.science.uwaterloo.ca/~cchieh/cact/c123/massacti.html Chemical equilibrium - The Law of Mass Action
--> <!-- Bot generated title --> <!-- ]</ref> <ref>http://www.chem.indiana.edu/academics/ugrad/Courses/s117/documents/kr_110606.pdf</ref>
<ref>http://www.nuc.berkeley.edu/courses/classes/E-115/Slides/Sect_10_thermo_chemical_reactions.ppt</ref>
<ref>[http://antoine.frostburg.edu/chem/senese/101/acidbase/faq/equivalence-point-HF-NaOH.shtml General Chemistry Online: FAQ: Acids and bases: What is the pH at the equivalence point an HF/NaOH titration?
-- and at other times to the (usually incorrect) <math>r_f</math> rate formula.<ref>[http://www.biochem.northwestern.edu/holmgren/Glossary/Definitions/Def-L/law_of_mass_action.html law of mass action definition<!-- Bot generated title -->]</ref>▼
<ref>[http://www.caam.rice.edu/~bpeercy/math468/lab4.html Lab 4 - Slow Manifolds<!-- Bot generated title -->]</ref>▼
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▲and at other times to the (usually incorrect) <math>r_f</math> rate formula.<ref>[http://www.biochem.northwestern.edu/holmgren/Glossary/Definitions/Def-L/law_of_mass_action.html law of mass action definition
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▲<ref>[http://www.caam.rice.edu/~bpeercy/math468/lab4.html Lab 4 - Slow Manifolds
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== Referências ==
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