Study Set Content:
if it is zero order
the rate of the reaction is not affected by the concentration of that reactant.
If m or n is zero, the reaction is
zero order
sum of the orders with respect to each reactant.
overall reaction order
– is one where the rate is independent of conc. reactant or reactants
Zero-order reactions
is a reaction whose rate depends on the concentration of one reactant raised to the 2nd power or on the concentrations of two different reactants, each raised to the 1st power.
Second-order reaction
is a reaction whose rate depends on the reactant concentration raised to the 1st power. For a first-order reaction, doubling the concentration of the reactant doubles the rate.
First-order reaction
a theory that assumes that, for reaction to occur, reactant molecules must collide with an energy greater than some minimum value and with the proper orientation.
Collision Theory
The reacting species must collide in an orientation that allows contact between the atoms that will become bonded together in the product.
The reacting species must collide in an orientation that allows contact between the atoms that will become bonded together in the product.
is one in which the experimentally determined rate of reaction is found to be proportional to the conc. of each of 3 reactants, or proportional to the conc. of one of 2 reactants and to the 2nd power of the conc. of the other, or proportional to the 3rd power of the conc. of a single reactant. Third-order reactions are very rare.
Third-order reaction
a temporary species formed by the reactant molecules as a result of the collision before they form the product
Activated complex or transition state:
minimum energy of collision required for two molecules to react
Activation energy
The collision must occur with adequate energy to permit mutual penetration of the reacting species’ valence shells so that the electrons can rearrange and form new bonds (and new chemical species).
The collision must occur with adequate energy to permit mutual penetration of the reacting species’ valence shells so that the electrons can rearrange and form new bonds (and new chemical species).
Also called reaction path
Reaction mechanism
The rate of a reaction is proportional to the rate of reactant collisions
The rate of a reaction is proportional to the rate of reactant collisions
number of molecules on the reactant side of an elementary reaction
Molecularity
involves one reactant molecule
Unimolecular reaction
species produced in one step and consumed in a subsequent step
Intermediates
a series of simple reactions that represent the progress of the overall reaction at the molecular level
Elementary reaction
gas-phase reactions; involves 3 reactant molecules
Termolecular reaction
: involves 2 reactant molecules; most common
Bimolecular reaction
