Sections
Enzymes
Enzyme-Substrate Complex
Lock and Key Vs. Induced Fit Models
Optimal Enzyme Conditions
Activation Energy
Types of Enzymes
Cofactor
Catalysis
Electrostatic and Metal Ion Catalysis
Covalent Catalysis
Reaction Rate
Enzyme Kinetics
Rate Constants and Rate Law
Reaction Orders
Rate Constant Units
Initial Velocity
Vmax Enzyme
Km Enzyme
Steady-State Conditions
Michaelis-Menten Assumptions
Michaelis-Menten Equation
Lineweaver-Burk Plot
Michaelis-Menten vs. Lineweaver-Burk Plots
Shifting Lineweaver-Burk Plots
Calculating Vmax
Calculating Km
Kcat
Specificity Constant

Concept #1: Introduction to Reaction Orders

Practice: The rate law for an elementary and/or nonelementary reaction is _________________________:

Concept #2: Zero-Order Reactions

Example #1: Zero Order Kinetics: Does increasing the # of cars also increase the rate that the cars cross the 1-lane bridge?

Concept #3: 1st Order Reactions

Concept #4: 2nd Order Reactions

Practice: What is the overall reaction order for the following rate law? v = k [A] 1 [B]1 [C]0

Concept #5: Pseudo 1st Order Reactions

Practice: Which of the following options is true for a reaction with the provided rate law: v = k [NO]2 [O2]

Practice: Consider the nonenzymatic elementary reaction from A → B. When the initial [A] = 20 mM, the reaction velocity is measured as 5 μM/min. Determine the reaction order and calculate the rate constant for the reaction.

Practice: Consider the nonenzymatic elementary reaction A  B.  When the [A] = 20 mM, the reaction velocity is measured as 5 µM of “B” produced per minute.  Calculate the rate constant for the reaction. Hint: Consider the rate law.

Practice: The hypothetical elementary reaction 2A --> B + C has a rate constant of 10-6 M-1s-1.  What is the reaction velocity when the concentration of A is 10 mM?