Chapter 10: Kinetics

reaction rates

the concentration of a substance at different points in time of a reaction

kinetic curve

graph of reaction rate

rate of production

the slope of kinetic curve

concentration effect on reaction rate

if substance is in the rate law, increasing the concentration will increase reaction rate

temperature effect on reaction rate

exponentially related to kelvin temperature

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

catalyst as a reaction rate

catalysts lower activation energy and provide larger rate constat

k

rate constant

order of reaction

found by adding up the exponents of the reactants

Arrhenius equation

k = Ae^(-Ea/RT)

R in Arrhenius Equation

8\.314

zero order reaction rate law

Rate = k

First order rate law

Rate = k\[A\]

integrated first order equation

ln \[A\]0 - ln \[A\]t = kt

half life first order equation

t(1/2) = .693/k

second order rate law

Rate = k\[A\]^2

collision theory

rate of chemical equation is based on collision rate, orientation, and minimum energy

transition state theory

kinetic converts to potential energy, if potential exceeds Ea, reaction occurs and become products

reaction mechanisms

series of steps that occur in a reaction from start to finish

elementary reactions

the smaller reactions that occur in an overall reaction