Which one of the following statements is false? In order for a reaction to occur

Question

Which one of the following statements is false? In order for a reaction to occur, reactant molecules must collide with each other. A catalyst alters the rate of a reaction and is neither a product nor a reactant in the overall equation. According to collision theory a three-body collision is less likely than a two-body collision. In reactions that are second order in one reactant and first order in another, the slow step generally involves a three-body collision of these reactants. The transition state is a short-lived, high energy state, intermediate between reactants and products. The decomposition of dimethylether at 504 degree C is first order with a half-life of 1570 seconds. What fraction of an initial amount of dimethylether remains after 4710 seconds? 1/3

Explanation / Answer

The answer is : In reactions that are second order in one reactant and first order in another, the slow step generally involves a three-body collision of the reactants.

The molecularity of reaction is not necessarily equal to order of reaction. Molecularity of reaction is given by number of molecules collide with one another to form a product in slowest step.

2A+B -------->C

Rate = K [A]2[B]

the mechanism for this reaction

A + B ----------> I (Intermediate)

I + A ----------> C

As we can deduce from mechanism A will collide with B forming I ( an intermediate), thus molecularity for this reaction is 2

Rate = K [A]2[B]

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