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A reaction occurs in three steps . The r...

A reaction occurs in three steps . The rate constants of the first , second and third steps of the reaction are `k_(1), k_(2) and k_(3)` respectively and the overall rate constant of the reaction is `k=k_(1)k_(2)//k_(3)` . If the activation energies of the first , second and third step of the reaction are 30, 44 and `56"kJ.mol"^(-1)` respectively , then the overall activation energy of the reaction `("in kJ.mol")` is -

A

23

B

37

C

18

D

42

Text Solution

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The correct Answer is:
C
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A reaction takes place in three steps will activation energy Ea_1 = 180 kJ/mol , Ea_2 = 80 kJ/mol & Ea_3 = 50kJ/mol respectively.Overall rate constant of the reaction is k = [(k_1k_2)/k_3]^(2/3) Calculate activation energy of the reaction.

The activation energy of the exothermic reaction ArarrB " is "40"kJ."mol"^(-1) . The heat of reaction is 15"kj.mol"^(-1) . What is the activation energy for the backward reaction ?

Knowledge Check

  • At 300K , frequency factor (A) of a first order reaction is 1000 times its rate constant . The activation energy of the reaction ("in kJ. Mol"^(-1)) is -

    A
    `12.56`
    B
    `7.48`
    C
    `15.69`
    D
    `17.22`

  • For a reaction, ArarrB , DeltaH = +xkJ .mol^(-1) and activation energy is "ykj.mol"^(-1) . If activation energy of the reaction , BrarrA " is z kJ.mol"^(-1) , then -

    A
    `zgty`
    B
    z = y - x
    C
    `z=y+x`
    D
    `z=-y+x`

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