Week 4 - Kinetics Flashcards
Where is kinetics used in dentistry
- kinetics of resin composites and how fast they set
- degradation kinetics of API in drugs (how they store)
- enzyme suppression treatment designed to reduce pocket depth
What does kinetics refer to
How fast a reaction proceeds
what is rate constant k (lowercase)
- indicated how fast a reaction is e.g. k=10^5
- indicates the time to get to equilibrium
What is Kc
Equilibrium constant - ratio of the concentrations of the products and reactants - can only be measured at equilibrium
What is the units for the rate (k)
mol/Ls
Moles per liter seconds
What are elementary steps
In chemical reactions the ‘real process’ occurs in elementary steps, where the sum of the elementary steps to give the balanced equation.
What does RDS stand for
Rate determining step
What is the RDS
The the elementary step in a chemical reaction which requires the highest amount of energy (has the larger energy barrier for it to react) and it determines the rate law.
The slowest step, which determines the overall rate and molecularity of the reaction.
The rate determining step is the slowest elementary step of a chemical reaction it determines the overall rate and molecularity. The RDS is the elementary step with the largest energy barrier (activation energy). It is also used to determine the rate law as it is the slowest elementary step in the reaction
What is the Molecularity of a step
The number of reactants in an elementary step
E.g.
A –> B = unimolecular
C + B –> D = Bimolecular RDS
What is an intermediate
Species which is produced in the middle of a multi step reaction.
It is the lowest point in energy between two consecutive elementary steps. The reaction intermediate is located as the ‘dip’ between two elementary steps within the reaction and is a species which appears in the mechanism of a reaction but not in the final balanced equatio
What are reaction orders
The coefficient of the reactants determines reaction order. E.g. [A]^1 = first order with respect to A
What is a first order reaction
when the rate changes proportionally with the concentration of the reagent (1 for 1)
What is the overall reaction order/ overall molecularity
the sum of all of the individual orders
Reactants
Transition state
Products
What is the effects of temperature on the rate of reaction
Temp Increase
- Increases the number of particles with sufficient activation energy
- Increases the kinetic energy of the particles hence increasing the number of successful collisions
- increases overall rate of reaction
What is this equation and what do the letters stand for
ArrheniT = temperature in kelvin
R = Gas constant
Ea = activation energy (J/mol)
e = exponential
k = reaction constant
A = frequency factor us Equation
What are the units for activation energy
J/mol
Impact of high activation on rate
High Ea = small k (by Arrhenius equation = slow rate of reaction
What is the rough rule for change of temperature on rate
For reactions happening at room temperature the rate of reaction doubles for ever 10 degrees rise in temperature
What is the initial rate
rate of reactions at the very beginning of the reaction
What is the instantaneous rate
rate of reaction at any specific point in time hence it will always be different depending on what time you measure it - changes all the time until equilibrium
What is the average rate
the average rate of reaction over the whole reaction