Chemistry Unit 10 Kinetics and Equilibrium (Jones - TJHSST)
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Last updated 11:41 PM on 4/30/23
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13 Terms
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Collision Theory
proposes that atoms, molecules, or ions must collide in order to react
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Transition State
associated with activated complex, can form prodcuts or reform reactants
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Activation Energy
Minimum amount of energy needed to form activated complex
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Instantaneous Rate
Reaction Rate calculated by finding slope of line tangent to curved plot of \[reactant\] = f(time) at specific instant in time
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Rate Law
Quantitative relationship between reaction rate and reactant concentrations
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Specific Rate Constant (k)
characteristic constant associated with reaction at given temperature
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Inhibitor
species that decelerates reaction rates
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Complex Reaction
multi-step reaction that consists of two or more elementary steps
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reactive intermediate
species produced in one elementary step of mechanism and then consumed in subsequent elementary step of same mechanism
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catalyst
species that speeds up reaction rates and is recycled
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Reaction Order
Defines how reaction rate depends on concentration on certain reaction
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Reaction Mechanism
complete sequence of elementary steps in multi-step reaction (Mechanism = Pathway)
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Rate - Determining Step
Slowest or “Bottleneck” elementary step in multi-step reaction
