Chemical Kinetics
Relative rates of change
Graphical determination of reaction rates
Integrated Rate laws
Activation energy
Zero order
First order
Second order
[X] = -kt + [X]0
ln[X] = -kt +ln[X]0
1/[X] = kt + 1/[X]0
half-life = [X]0/2k 🏁
half-life = 0.693/k 🏁
half-life = 1/k[X]0 🏁
lnk = -Ea/R * (1/T) + ln A
k is rate constant
Ea is activation energy
R is gas constant 8.314 J/molK
T is temperature (Kelvin)
A is frequency factor
Arrhenius equation
For the reaction xX -> yY
-(1/x)delta [X]/delta t = (1/y)delta[Y]/delta t
Average rate
Instantaneous rate
delta[X]/delta t between two points
delta[X]/delta t between two points on either side