Chapter 10: Kinetics
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Last updated 2:35 AM on 3/30/23
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20 Terms
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reaction rates
the concentration of a substance at different points in time of a reaction
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kinetic curve
graph of reaction rate
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rate of production
the slope of kinetic curve
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concentration effect on reaction rate
if substance is in the rate law, increasing the concentration will increase reaction rate
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temperature effect on reaction rate
exponentially related to kelvin temperature
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ability to meet as an effect on reaction rates
gas or solutions rapidly react because of the individual molecules. If a solid is grinded, it will react more
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catalyst as a reaction rate
catalysts lower activation energy and provide larger rate constat
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k
rate constant
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order of reaction
found by adding up the exponents of the reactants
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Arrhenius equation
k = Ae^(-Ea/RT)
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R in Arrhenius Equation
8\.314
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zero order reaction rate law
Rate = k
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First order rate law
Rate = k\[A\]
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integrated first order equation
ln \[A\]0 - ln \[A\]t = kt
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half life first order equation
t(1/2) = .693/k
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second order rate law
Rate = k\[A\]^2
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collision theory
rate of chemical equation is based on collision rate, orientation, and minimum energy
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transition state theory
kinetic converts to potential energy, if potential exceeds Ea, reaction occurs and become products
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reaction mechanisms
series of steps that occur in a reaction from start to finish
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elementary reactions
the smaller reactions that occur in an overall reaction
