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  2. Rate equation - Wikipedia

    en.wikipedia.org/wiki/Rate_equation

    If the concentration of a reactant remains constant (because it is a catalyst, or because it is in great excess with respect to the other reactants), its concentration can be included in the rate constant, leading to a pseudofirst-order (or occasionally pseudo–second-order) rate equation. For a typical second-order reaction with rate ...

  3. Reaction progress kinetic analysis - Wikipedia

    en.wikipedia.org/wiki/Reaction_progress_kinetic...

    [A] can provide intuitive insight about the order of each of the reagents. If plots of ⁠ v / [A] ⁠ vs. [B] overlay for multiple experiments with different-excess, the data are consistent with a first-order dependence on [A]. The same could be said for a plot of ⁠ v / [B] ⁠ vs. [A]; overlay is consistent with a first-order dependence on [B].

  4. Pseudo first order reaction - Wikipedia

    en.wikipedia.org/?title=Pseudo_first_order...

    Language links are at the top of the page across from the title.

  5. Chemical kinetics - Wikipedia

    en.wikipedia.org/wiki/Chemical_kinetics

    Chemical kinetics, also known as reaction kinetics, is the branch of physical chemistry that is concerned with understanding the rates of chemical reactions. It is different from chemical thermodynamics , which deals with the direction in which a reaction occurs but in itself tells nothing about its rate.

  6. Enzyme kinetics - Wikipedia

    en.wikipedia.org/wiki/Enzyme_kinetics

    Thus the product formation rate depends on the enzyme concentration as well as on the substrate concentration, the equation resembles a bimolecular reaction with a corresponding pseudo-second order rate constant /. This constant is a measure of catalytic efficiency.

  7. SN2 reaction - Wikipedia

    en.wikipedia.org/wiki/SN2_reaction

    The rate of an S N 2 reaction is second order, as the rate-determining step depends on the nucleophile concentration, [Nu −] as well as the concentration of substrate, [RX]. [1] r = k[RX][Nu −] This is a key difference between the S N 1 and S N 2 mechanisms.

  8. Rate-determining step - Wikipedia

    en.wikipedia.org/wiki/Rate-determining_step

    In fact, however, the observed reaction rate is second-order in NO 2 and zero-order in CO, [5] with rate equation r = k[NO 2] 2. This suggests that the rate is determined by a step in which two NO 2 molecules react, with the CO molecule entering at another, faster, step. A possible mechanism in two elementary steps that explains the rate ...

  9. Reaction rate constant - Wikipedia

    en.wikipedia.org/wiki/Reaction_rate_constant

    where A and B are reactants C is a product a, b, and c are stoichiometric coefficients,. the reaction rate is often found to have the form: = [] [] Here ⁠ ⁠ is the reaction rate constant that depends on temperature, and [A] and [B] are the molar concentrations of substances A and B in moles per unit volume of solution, assuming the reaction is taking place throughout the volume of the ...