1. Statement-I : Fractional order reactions are not elementary reactions.
Statement-II : For an elementary reaction, order must be same as molecularity.
are these statements true? give reason.
To determine the truth of these statements, we need to examine each one individually and evaluate its accuracy.
Statement-I: "Fractional order reactions are not elementary reactions."
This statement is true. Fractional order reactions are those in which the reaction rate is dependent on a fractional power of the reactant concentrations. These reactions are not considered elementary reactions because they do not follow the simple rate laws observed in elementary reactions. In elementary reactions, the reaction rate depends on the concentration of reactants raised to a whole number power.
Statement-II: "For an elementary reaction, order must be the same as molecularity."
This statement is false. Molecularity refers to the number of molecules or particles involved in an elementary reaction's rate-determining step. On the other hand, the order of a reaction is determined experimentally and represents the power to which the concentration terms are raised in the rate law equation.
In elementary reactions, the two concepts (order and molecularity) may or may not be the same. The order of an elementary reaction could be the same as, different from, or even fractional in relation to its molecularity. It is only in certain cases where the order is equal to the molecularity, such as in some simple unimolecular or bimolecular elementary reactions.
In summary, Statement-I is true, while Statement-II is false. Fractional order reactions are not elementary reactions, and the order of an elementary reaction does not necessarily have to be the same as its molecularity.