Chemical Reaction Engineering
For a heterogeneous catalytic reaction

The surface of the catalyst does not play an important role during reaction
Free energy of activation is lowered in the presence of catalyst, which remains unchanged at the end of reaction
The catalyst does not form an intermediate complex with the reactant
A relatively small amount of catalyst can cause the conversion of large amount of reactants which does not mean that catalyst concentration is important

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Chemical Reaction Engineering
The rate expression for a heterogenous catalytic reaction is given by, - rA = K.KA PA(1 + KA.PA + Kr.PR), where K is surface reaction rate constant and KA and KR are absorption equilibrium constants of A and R respectively. If KR PR >> (1 + KA PA), the apparent activation energy EA is equal to (given E is the activation energy for the reaction and ΔHR and ΔHA are the activation energies of adsorption of R and A)

ΔHA + ΔHR
E + ΔHA
E + ΔHA - ΔHR
E

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