Chapter 13
Chemical Kinetics
By Boundless
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Reaction rates are determined by observing the changes in the concentrations of reactants or products over a specific time frame.
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Reaction stoichiometry studies the quantitative relationships between reactants and products within a given chemical reaction.
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The rate law for a chemical reaction relates the reaction rate with the concentrations or partial pressures of the reactants.
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A first-order reaction depends on the concentration of one reactant, and the rate law is:
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A second-order reaction is second-order in only one reactant, or first-order in two reactants.
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A zero-order reaction has a constant rate that is independent of the concentration of the reactant(s); the rate law is simply
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The integrated rate laws derive from calculus, and they relate the concentrations of reactants with time.
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The half-life of a reaction is the amount of time it takes for the concentration of a reactant to decrease to one-half of its initial value.
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Collision theory provides a qualitative explanation of chemical reactions and the rates at which they occur, appealing to the principle that molecules must collide to react.
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The rate of a chemical reaction depends on factors that affect whether reactants can collide with sufficient energy for reaction to occur.
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The Arrhenius equation is a formula that describes the temperature-dependence of a reaction rate.
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In a given chemical reaction, the hypothetical space that occurs between the reactants and the products is known as the transition state.
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The rate law for an elementary step is derived from the molecularity of that step.
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The rate of a multi-step reaction is determined by the slowest elementary step, which is known as the rate-determining step.
Rate laws for reactions are affected by the position of the rate-determining step in the overall reaction mechanism.
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The steady state approximation can be used to determine the overall rate law when the rate-determining step is unknown.
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Reaction rates can be determined experimentally by measuring the concentration of a reactant and/or product over time.
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Heterogeneous catalysis is a type of catalysis in which the catalyst occupies a different phase than the reaction mixture.
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Homogeneous catalysis is a class of catalysis in which the catalyst occupies the same phase as the reactants.
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Enzymes are proteins that accelerate biochemical transformations by lowering the activation energy of reactions.