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Details:

The main difference between molecularity and order of reaction lies in their definition and determination:

Molecularity

It is the number of reactant molecules involved in an elementary step of a reaction.

It is always a whole number (1, 2, or 3) and cannot be fractional or zero.

It is determined by the reaction mechanism and cannot be found from the overall balanced equation.

Example: If a reaction step involves two molecules reacting together, its molecularity is bimolecular.

Order of Reaction

It is the sum of the powers of the concentration terms in the rate law equation.

It can be zero, a whole number, or even a fraction.

It is determined experimentally from the rate equation and does not always correspond to the molecularity.

Example: For a reaction with a rate law Rate = k[A]²[B]¹, the order is 2 + 1 = 3.

Key Distinction:

Molecularity applies to a single step in a reaction mechanism, while order of reaction applies to the overall reaction and is found experimentally.

Molecularity is always an integer, while order can be fractional or zero.

Would you like any specific examples or further clarifications?