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Which one of the following statements for the order of a reaction is incorrect?
A
Order of reaction is always whole number
B
Order can be determined only experimentally
C
Order is not influenced by stoichiometric coefficient of the reactants
D
Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction
Detailed Solution
Order of a reaction is the sum of the powers of the concentration terms of the reactants in the experimentally determined rate law (true).
It is an experimental quantity and cannot be predicted from the balanced equation, so it does not depend on the stoichiometric coefficients (both true).
Order can be zero, a whole number or a fraction; for example, the decomposition of acetaldehyde has order 1.5.
It is molecularity, not order, that is always a whole number.
Hence the incorrect statement is that the order of a reaction is always a whole number.
It is an experimental quantity and cannot be predicted from the balanced equation, so it does not depend on the stoichiometric coefficients (both true).
Order can be zero, a whole number or a fraction; for example, the decomposition of acetaldehyde has order 1.5.
It is molecularity, not order, that is always a whole number.
Hence the incorrect statement is that the order of a reaction is always a whole number.