Chapter 12: Kinetics Flashcards
(20 cards)
rate of reaction
change in molar concentration of reactants or products per unit time
average rate
rate over a given time period
instantaneous rate
rate of reaction at a specific time
initial rate
rate at time, t = 0
beginning of the reaction
relative rate of reaction
rate of reaction in terms of the decomposition of reactants and formation of products
catalyst
increases the rate of reaction by lowering the activation energy
rate law
expresses the relationship between rate of reaction and concentrations of reactants
rate constant
specific for a particular reaction at a particular temperature
proportionality constant
higher when the rate is higher, lower when the rate is lower
overall reaction order
sum of the individual reaction orders
initial rate method
determining order of reaction via measuring rate at different initial reactant concentration
integrated rate laws
relates the concentrations of reactants and time
first order reaction
one molecule involved to reach transition state
second order reaction
two molecules involved to reach transition state
zero order reaction
has no effect on rate of reaction
half life
time taken for half of the initial concentration of a species to decompose
collision theory
collisions must occur with enough energy in the proper orientation in order to reach the transition state
the rate of reaction is directly proportional to the rate of reactant collisions
activation energy
energy needed to reach the transition state
Arrhenius equation
relates the activation energy to the rate constant
reaction diagram
shows the progress of a reaction
frequency factor
frequency of collisions
collisions of proper orientation