Chemical Kinetics

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  1. Some rate laws depend on the concentration of more than one species. For instance, oxidation of iodide ions by persulfate ions: Rate of consumption I- = k[S2O82-][I-]. In such cases, the analysis can be simplified by ensuring that one species remains at the same _________ during the reaction so it can be used as a ______.
    • concentration
    • constant
  2. In rate laws that depend on the concentration of more than one species, explain a technique used to keep one of the species constant.
    Starting the reaction with one of the species in such a high concentration that their concentration barely changes in the course of the reaction.
  3. In the case of the oxidation of iodide ions by persulfate ions: Rate of consumption I- = k[S2O82-][I-], if we started with so much [S2O82-] that it was practically constant throughout our reaction, what would the rate of consumption of I- be? What is k'? What order of reaction do we have know?
    • Rate of consumption of I- = k'[I-]
    • k' is the value k[S2O82-], which is another constant
    • We have gone from a second order reaction to a pseudo-first order reaction
  4. t1/2
    half life; it is the time needed for the concentration of a substance to fall one-half its initial value
  5. Write an equation that shows the relation between the rate constant and the half-life of a reactant in a first order reaction. It should show that the greater the rate constant, the ______ the half-life of a substance.
    shorter

    t1/2 = ln2/k

Card Set Information

Author:
Anonymous
ID:
328538
Filename:
Chemical Kinetics
Updated:
2017-02-16 03:34:24
Tags:
chemistry
Folders:
Midterm II
Description:
Ch 15 pt 2
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