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Correct statements regarding Arrhenius equation among the following are : A. Factor e^ -E a / R T corresponds to fraction of molecules having kinetic energy less than Ea. B. At a given temperature, lower the Ea, faster is the reaction. C. Increase in temperature by about 10^ C doubles the rate of reaction. D. Plot of k vs 1 ~T gives a straight line with slope =- E a R . Choose the correct answer from the options give

Options

  1. AB and D Only
  2. BA and B Only
  3. CB and C Only
  4. DA and C Only

Correct answer

C. B and C Only

Step-by-step solution

The Arrhenius equation is given by k = A e^ -E_a/RT . Statement A: The factor e^ -E_a/RT represents the fraction of molecules having kinetic energy equal to or greater than the activation energy E_a . Thus, statement A is incorrect. Statement B: From the equation, as E_a decreases, the value of k increases, leading to a faster reaction rate. Thus, statement B is correct. Statement C: For many reactions, the temperature coefficient is approximately 2, meaning the rate of reaction doubles for every 10^ C rise in temp

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