Rates of Reaction

what is kinetics

kinetics tells us how fast a chemical reaction occurs, so how quickly a reactant turn into a product

how does kinetics apply to pharmaceutics

• drug stability & shell life - how long left before a drug expires & how long it will remain active

• dosing schedules in the body

• how enzymes break down drugs in the body

• kinetics helps calculate the right dose of radioactive drugs for imaging or treatment

what is stability

Stability refers to the ability of a drug to maintain its potency and effectiveness over time under specific storage conditions, influencing its expiration and shelf life

• a drug can be thermodynamically unstable but last a long time due to kinetic stability

what is activation energy

what makes the reaction slow or fast e.g wod can burn but need a spark (Ea) to start

what are elementary reaction

Reactions that occur in a single step, with a simple transition state, and follow a specific rate law.

what is bimolecular

A reaction involving two reactant molecules. Bimolecular reactions can occur in one step or through multiple stages and are characterized by a second-order rate law.

what is rate law

An equation that relates the rate of a reaction to the concentration of its reactants, typically expressed as rate = k[A]^m[B]^n.

what is this k[A]^m[B]^n

k is the rate constant, A & B are the conc of reactant, and m & n are the reaction orders with respect to each reactant which tells us how changes in concentration affect A or B

what is zero order reaction

is when the rate stays the same, so the rate of reaction does not change, even if you add more reactant. Rate=k [A]=[A]₀-kt

what is first order reaction

A reaction where the rate is directly proportional to the concentration of one reactant, expressed as rate = k[A], meaning that doubling the concentration of A will double the rate. In[A]_t=In[A]₀-kt

what is second order reaction

A reaction where the rate is proportional to the square of the concentration of one reactant or the product of the concentrations of two reactants. This is expressed as rate = k[A]² or rate = k[A][B], indicating that doubling the concentration leads to a quadrupling of the rate.