Which of the following statements about order of reaction is incorrect?
Correct answer: D. It is always equal to molecularity
- A. It does not determines the mechanism of reaction
- B. It is determined experimentally
- C. It is associated with the rate equation
- D. It is always equal to molecularity
Explanation
The statement that the order of a reaction is always equal to its molecularity is incorrect. Molecularity refers to the number of molecules participating in a single elementary step of a reaction, and it is always an integer. Reaction order, however, is the sum of the exponents of reactant concentrations in the rate equation, which is determined experimentally and can be fractional or differ from molecularity.Option A is incorrect because the reaction order does not determine the mechanism, though it provides information about the kinetics. Option B is incorrect because the reaction order is indeed determined experimentally. Option C is incorrect because the order of a reaction is associated with the rate equation, indicating how reactant concentrations affect the rate.
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About Reaction Kinetics
Reaction kinetics relates reaction rate to concentration, temperature, surface area and catalysts. Questions cover rate laws, reaction order, rate constants, activation energy and the activated complex, including how a catalyst lowers the activation energy without changing the overall energy change or equilibrium position.
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