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Chemical Kinetics
Chemical Kinetics
Unit 1. Definitions and Collision Theory
Describe the main factors that can increase the rate of a reaction.
Describe the collision theory of chemical kinetics.
Define effective collision and activation energy.
Determine the average rate of a reaction given appropriate data.
Determine the instantaneous rate of a reaction given a graph.
Use the stoichiometry of a reaction to express the rate of a reaction in terms of a reactant or product.
Define reaction order and provide examples of a zeroth-, first- and second-order reaction rate law.
The Rate of Reactions
The Rate of Reactions
https://youtu.be/6mAqX31RRJU (6:24)
Bozeman Science - In this video Paul Andersen defines the rate of a reaction as the number of reactants that are consumed during a given period of time. The rate of the reaction can be affected by the type of reaction as well as the concentration, pressure, temperature and surface area.
The Rate Law
The Rate Law
https://youtu.be/WDXzVI8SmfE (8:43)
Bozeman Science - Paul Andersen explains how the rate law can be used to determined the speed of a reaction over time. Zeroth-order, first-order and second-order reactions are described as well as the overall rate law of a reaction. The rate of a reaction can be determined experimentally.
Unit 2. Determination of Rate Law
Produce the rate law of a reaction given experimental data.
Predict the units of the rate constant k for a reaction.
Determine the order of a reaction from its rate law.
Determine the concentration of reactant using the integrated rate law for the reaction.
Calculate the half-life (t½) of a reaction.
Calculate the amount of reactant remaining after a certain period of time given the half-life and order of the reaction.
Determine the rate constant or activation energy of a reaction using the Arrhenius equation.
Kinetics: Initial Rates and Integrated Rate Laws
Kinetics: Initial Rates and Integrated Rate Laws
Integrated Rate Laws - Zero, First, & Second Order Reactions - Chemical Kinetics
Integrated Rate Laws - Zero, First, & Second Order Reactions - Chemical Kinetics
Duration: 48+ minutes
This chemistry video tutorial provides a basic introduction into chemical kinetics. It explains how to use the integrated rate laws for a zero order, first order, and a second order reaction to solve problems. It explains how to calculate the units of the rate constant k, how to find the final concentration of the reactant, and how to solve half life problems.
Unit 3. Mechanisms
Define reaction mechanism.
Determine the rate law of a reaction given its rate determining step.
Understand the criteria that must be met for a proposed mechanism to be plausible.
Define elementary reaction.
Define catalyst and intermediate.
Describe the major types of catalysis: heterogeneous, homogeneous and enzymatic.
Collision Theory - Arrhenius Equation & Activation Energy - Chemical Kinetics
Collision Theory - Arrhenius Equation & Activation Energy - Chemical Kinetics
Duration: 31+ minutes
This video provides a basic introduction into collision theory. It also provides the Arrhenius equation and related formulas needed to calculate quantities such as the forward and reverse activation energy of a reaction, the rate constant k, and the associated temperature.
Writing Rate Laws of Reaction Mechanisms Using The Rate Determining Step - Chemical Kinetics
Writing Rate Laws of Reaction Mechanisms Using The Rate Determining Step - Chemical Kinetics
Duration: 18+ minutes
This chemistry video tutorial provides a basic introduction into reaction mechanisms within a chemical kinetics setting. It explains how to write the rate law expression for a reaction mechanism. A reaction mechanism consist of a series of elementary steps or elementary reactions whose rate law can be written from its molecularity - that is from the coefficients of the balanced reaction. The rate of a reaction mechanism is completely dependent on the slow step or the rate-determining step. This video explains how to substitute an intermediate when writing rate law expressions. It contains plenty of examples and practice problems.
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