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Consider two reactions having same Arrhenius factor A, but different energy of activation. (i) A → B ; E a 1 = 20 kJ (ii) C → D ; E a 2 = 30 kJ Both are at temperature 25 ° C If temperature in both reaction is increased slightly in such a way that change in temperature in both case is same than choose the correct options.

Options

  1. AThe second reaction is faster
  2. BThe second reaction is more sensitive towards temperature variation
  3. CIf temperature increases, rate of first reaction increase more sharply
  4. DAll the above are correct

Correct answer

B. The second reaction is more sensitive towards temperature variation

Step-by-step solution

Arrhenius equation; d l n k = E a R T 2 d T Here, T and dT same and positive d l n k α E a l n k 2 - l n k 1 α E a l n K 2 K 1 α E a So, if temperature increases, then rate of reaction having more E a increases more sharply.

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