The two main theories of catalysis are:
Intermediate compound theory for heterogenous catalysis and the adsorption theory for homogenous catalysis.
Intermediate compound theory for autocatalysis and the adsorption theory for heterogenous catalysis.
Collision theory for homogenous catalysis and the transition state theory for heterogenous catalysis.
Intermediate compound theory for homogenous catalysis and the adsorption theory for heterogenous catalysis.
For any chemical reaction to occur:
Collision energy must be equal to the activation energy for the reaction.
Collision energy must be greater than the activation energy for the reaction.
Collision energy must be greater than or equal the activation energy for the reaction.
Collision energy must be less than or equal the activation energy for the reaction.
Compound A (represented by circles) converts to compound B (represented by squares) in a first-order process, as represented by the scenes:
The half-life, t1/2, of the reaction is:
t1/2 = 30s.
t1/2 = 45s.
t1/2 = 60s.
t1/2 = 90s.
The two most important theories of kinetics are:
Collision theory and transition state theory.
Intermediate state theory and transition state theory.
Catalysis theory and transition state theory.
Collision theory and catalysis theory.
