5.1
How quickly a reaction produces products
Reaction Rate
Describes the relationship between the rate of a chemical reaction and the concentrations of the reactants
Rate Law
ln[A] vs time
first order
The rate determining step is the
slow step
Formula for Reaction Rate??
Rate = -Δ[Reactant]/t or as Rate = Δ[Product]/t
What is K??
rate constant
[A] vs time
zero order
something that’s created in one step and used up in another step
Intermediates
The point at which the rate of the reaction going forwards is the same as the rate of the reaction going backward and the concentrations of the reactants and products remain constant.
Equilibirum
sum of the orders for each reactant
overall reaction order
1/[A] vs time
second order
speed up the reaction rate, present in the beginning and end of reaction and are not shown in in a balanced equation
Catalyst
The change in concentration of a reactant or product over a specific time interval
Average rate of a reaction
If we are in second order and we double the concentration of A, the rate will
quadruple
time required for the concentration of a reactant to decrease to half of its initial concentration
half life
mall reactions that make up an entire reaction. Single step
Elementary Step
The rate of the reaction at a specific point in time. Calculated by taking the limit of the average rate as the time interval approaches zero.
Instantaneous Rate of a Reaction
R equals
Rate of the reaction
All radioactive decay is done in the
first order
Formula for Half Life
0.693/k