Kinetics Flashcards
What is the rate equation
rate = -d [A] / dt = k [A] ^n
A is disappearing and then B is appearing delta a / by the change in time (dt)rate constant (small k always, written in italics, multipied by conc of A to the power of
n is the order of the reaction
What is zero order
N=0 so same equation
The reaction is independent of [A] and occurs at a constant rate
Zero order example
First order
the rate is dependent on one reacting species
k x [A]
Second order
depends on the concentration of two reactants
A +B —> C
rate = k [A] [B]
Catalysis
Reactants are transformed to products via a transition state that only lasts briefly and cannot be isolated.
Catalysts make the product through a different mechanism with a lower activation energy so it is faster (but not always)
Homogenous catalysis:
catalyst in same phase as reactants (e.g. all liquid or all gases)
Heterogeneous catalysis:
catalyst in different phase to reactants (e.g. solid catalyst in liquid reactant)
Arrhenius Equation
If we know the rate constant at several temperatures you can determine the activation energy (Ea).
A plot of lnk vs. 1/T is a straight line with slope = -Ea/R
Autocatalysis
One of the products of the reaction acts as a catalyst. Initially reaction is slow then dramatically speeds up.