a. Explain the difference between order and molecularity in a reaction. b. Expla
ID: 819607 • Letter: A
Question
a. Explain the difference between order and molecularity in a reaction.
b. Explain the difference between a transition state and a reaction intermediate.
c. Explain the difference between branching and propagation steps in a chain reaction.
d. What type of mechanistic steps are needed to get an overall 3/2 order in the reaction:
CO + Cl2 k-1/k1 COCl2
e. Explain the difference in the way the Arrhenius exponential term arises in activated
complex theory and in collision theory.
f. Relaxation kinetics for a simple reaction A?B are expressed as 1/? = k1 + k-1
where ? is the relaxation time. Briefly explain why this is a sum and not a difference.
g. For the reaction 2A + B ???
k
?1 P, the rate = -
Explanation / Answer
ORDER OF A REACTION
MOLECULARITY OF A REACTION
ORDER OF A REACTION
MOLECULARITY OF A REACTION
It is sum of the concentration terms on which the rate of reaction actually depends or it is the sum of the exponents of the concentrations in the rate law equation. It is the number of atoms, ions or molecules that must collide with one another simultaneously so as to result into a chemical reaction. It need not be a whole number i.e. it can be fractional as well as zero. It is always a whole number. It can be determined experimentally only and cannot be calculated. It can be calculated by simply adding the molecules of the slowest step. It is for the overall reaction and no separate steps are written to obtain it. The overall molecularity of a complex reaction has no significance. It is only slowest step whose molecularity has significance for the overall reaction. Even the order of a simple reaction may not be equal to the number of molecules of the reactants as seen from the unbalance equation.For simple reactions, the molecularity can usually be obtained from the Stoichiometry of the equation.
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