AP Kinetics and Reaction Rates Review Summary
Rate Laws (r = k[A][B])
- Using reactant concentrations ONLY to calculate
- Reaction orders:
o 1st order: A1 21 = 2 (Concentration multiplications to the power of
1)
Use: ln[A]t – ln[A]o = -kt
Make sure to ex answer to get [A] values
o 2nd order: A2 22 = 4 (Concentration multiplications to the power of
2)
Use: 1/[A]t – 1/[A]o = kt
Make sure to 1/X answer to get [A] values
o Zero Order A0 20 = 1 (Concentration multiplications to the power
of 0 = change in concentration does not affect rate)
Use: [A]t = -kt + [A]o
- Differentiated Rate Law: Rate Law determined using experimental data
(given)
- Integrated Rate Law: Rate Law determined using graphs or rate
equations
o Concentration vs. Time
Straight graph representing a zero-order reaction
Concentration v.s. Time
Graph
0.300
[A] (mol/L)
0.200
0.100
0.000
0 10 20 30 40 50 60 70 80
Time (s)
o
o 1/Concentration vs. Time
Straight graph representing a second order reaction
Rate Laws (r = k[A][B])
- Using reactant concentrations ONLY to calculate
- Reaction orders:
o 1st order: A1 21 = 2 (Concentration multiplications to the power of
1)
Use: ln[A]t – ln[A]o = -kt
Make sure to ex answer to get [A] values
o 2nd order: A2 22 = 4 (Concentration multiplications to the power of
2)
Use: 1/[A]t – 1/[A]o = kt
Make sure to 1/X answer to get [A] values
o Zero Order A0 20 = 1 (Concentration multiplications to the power
of 0 = change in concentration does not affect rate)
Use: [A]t = -kt + [A]o
- Differentiated Rate Law: Rate Law determined using experimental data
(given)
- Integrated Rate Law: Rate Law determined using graphs or rate
equations
o Concentration vs. Time
Straight graph representing a zero-order reaction
Concentration v.s. Time
Graph
0.300
[A] (mol/L)
0.200
0.100
0.000
0 10 20 30 40 50 60 70 80
Time (s)
o
o 1/Concentration vs. Time
Straight graph representing a second order reaction
