3.1 Chemical Kinetics
Reaction Rates : - Change in concentration of reactants (or products) as a function of time
3.2 How to Express Reaction Rate
=> Rate = d[A]
dt
change in concentration of A over a period, t when
[A] decrease with time, change of [A] is -ve.
=> Unit : mol/Ls @ M/s
3.3 Differential Rate Equation
aA + bB
* Keep In Mind : 2A
dissappear in each mole B formed.
3.4 Rate Law
- expressing rate as function of reactant
concentration and temperature
- given aA + bB
is :
- also called rate equation
3.5 Rate Equation
- does not change as reaction proceed.
3.6 Reaction Orders
=> Define how the rate affected by reactant
concentration
concentration
=> Always determine by experimentally
=> Order or reaction is no related to stoichiometry
ceofficent of reactant in balance chemical eqn.
ceofficent of reactant in balance chemical eqn.
Example 1 :
Example 2 :
Find the overall order from rate equation below :
ORDERS
OVERALL REACTION ORDERS
KEEP IN MIND =)
3.7 Integrated Rate Law
Function of integrated rate law :
* can estimate the period taken for x mol/L of
compound A to be used up
* we can know the concentration of compound A after
the reaction in specific time RATE = k [A]
KEEP IN MIND =)