Studied by 2 people
unimolecular/bimolecular/termolecular reaction
one/two/three reactant molecules involved
intermediate
produced in an earlier step and used as a reactant in a later step
how to find rate law of an elementary step
coefficients for stoichiometry are order for each reactant
reaction rate maxwell-boltzman graph
higher temp/wider distribution = more molecules moving at faster speeds = more have sufficient energy for reaction
activation energy
Ea, the minimum amount of energy required to activate atoms or molecules to where they can do the reaction, between starting energy and peak of graph
enthalpy change
ΔH, amount of energy given off/absorbed by a reaction, positive = endothermic, negative = exothermic
arrhenius equation main point
as temp goes up, reaction rate goes up
catalyst
lower Ea to make reaction faster, used up in an early step but formed in a later step, starting reactant and at the end
what the rate law/reaction order is set by
slowest elementary step
activation energy when reversing reaction
ΔH + original Ea
things that affect reaction rate
concentration, temp, surface area (higher = faster), catalysts
reaction order
how important the concentration of a given reactant is for how quickly the reaction progresses
zero order y axis
[A]
first order y axis
ln [A]
second order y axis
1/[A]
how to tell slow/fast steps from graph of reaction
peak with higher energy is slower step
how catalysts increase reaction rate
introducing more collisions or improving collision orientation
homogenous catalyst
same phase as reactants
heterogeneous catalyst
in different phase than reactants
0 order k units
M s^-1
1st order k units
s^-1
2nd order k units
M^-1 s^-1
3rd order k units
M^-2 s^-1
