13.4. Mechanisms I. Macroscopic Effects: Temperature and Energetics

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Kinetics : ArrheniusActEnergy (4 Variations)
The rate constant for the first-order dehydration of tert-butyl alcohol at 500^{o}C is 1.20 x 10^{ -4 } s^{ -1}. The rate constant for this process at 600^{o}C is 6.80 x 10 ^{ -3} s^{ -1}. Calculate the activation energy for this reaction in kJ/mol. (R = 8.314 J/mol K)

Kinetics |

Chemometrics

Kinetics : ArrheniusTemp (3 Variations)
The activation energy for the isomerization of cyclopropane to propene is 274 kJ/mol. By what factor does the rate of reaction increase as the temperature rises from 500^{o}C to 550^{o}C assuming all else remains constant? (R = 8.314 J/mol k)

Hint: This is asking for the ratio of rates which is proportional to the ratio of the rate constants, all else being equal.

Kinetics |

Chemometrics

Kinetics : CompareEnergyProfile (11 Variations)
Consider the following reactions that take place at the same temperature, begin with the same molar concentrations, and whose energy profiles are presented below:

Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) ComplexesRichard S. Herrick, Kenneth V. Mills, and Lisa P. Nestor Describes an experiment that introduces students to integrated rate laws, the search for a mechanism that is consistent with chemical and kinetic data, and the concept of activation barriers and their measurement in a curriculum whose pedagogical philosophy makes the laboratory the center of learning for undergraduates in their first two years of instruction. Herrick, Richard S.; Mills, Kenneth V.; Nestor, Lisa P. J. Chem. Educ.2008, 85, 1120.

Coordination Compounds |

Kinetics |

Mechanisms of Reactions |

Rate Law |

UV-Vis Spectroscopy

An Experimental Approach to Teaching and Learning Elementary Statistical MechanicsFrank B. Ellis and David C. Ellis This article details demonstrations that show how equilibrium changes with temperature, energy, and entropy and involve exothermic and endothermic reactions, the dynamic nature of equilibrium, and Le Châtelier's principle. Ellis, Frank B.; Ellis, David C. J. Chem. Educ.2008, 85, 78.

Equilibrium |

Kinetics |

Statistical Mechanics |

Thermodynamics

Visualizing the Transition State: A Hands-on Approach to the Arrhenius EquationThomas S. Kuntzleman, Matthew S. Swanson, and Deborah K. Sayers Pennies and dice are used to simulate the kinetics of two irreversible "reactions" with a hands-on, Monte Carlo approach. Arrhenius plots of the data generated yield activation energies comparable to assigned values and pre-exponential factors close to what would be expected based on the probability of a "reactant" achieving the correct orientation for conversion into "product". A comparison of the values obtained for the pre-exponential factors for the different simulations allows students to semi-quantitatively discuss the orientational requirement that is contained within this factor. Kuntzleman, Thomas S.; Swanson, Matthew S.; Sayers, Deborah K. J. Chem. Educ.2007, 84, 1776.

Kinetica; An Excel program to Stimulate or Analyze Kinetic DataLeonel Vera, Pedro Ortega, Miguel Guzmán The Excel spreadsheet Kinetica both simulates and analyzes kinetic data for simple rate equations of the form: - d[A]/dt = k [A]^n Instructors or students can generate simulated kinetic data using parameters they specify, or using parameters randomized by Kinetica. The data set that is generated may then be exported for use in exercises, homework, and exams, or may be analyzed directly within Kinetica. A kinetics data set may also be imported from an external source into Kinetica for analysis.

Kinetics

An Excel Program to Study First-Order KineticsKen Muranaka User data can be analyzed to determine what parameter values of the first order rate expression give the closest fit, or data can be generated using user-input values of the rate parameters and random noise levels. Statistical characterizations such as confidence limits and variance are calculated.

Kinetics

ChemPaths 104 F Feb 18John W. Moore Today in Chem 104:
* Lecture: Rates of Reaction
* Reading:
Kotz: Ch. 15, Sec. 1-2
Moore, Ch 13, Sec. 1-2
* Homework #5 due by 11:55 pm F Feb 26
* Excel Assignment due at first discussion section
next week (week of Feb. 21)