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The reaction takes place in three steps ...

The reaction takes place in three steps with activation energy `E_(A_(1))=x (kJ)/(mol), E_(A_(2))=y(kJ)/(mol) and E_(A_(3))=z(kJ)/(mol) `respectively. Overall rate constant of the reaction is k=`((k_(1)k_(2))/(k_(3)))^(1//5)` .The activation energy of the reaction will be

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Step by step text solution for The reaction takes place in three steps with activation energy E_(A_(1))=x (kJ)/(mol), E_(A_(2))=y(kJ)/(mol) and E_(A_(3))=z(kJ)/(mol) respectively. Overall rate constant of the reaction is k=((k_(1)k_(2))/(k_(3)))^(1//5) .The activation energy of the reaction will be by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 12 exams.

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The decomposition of ethane follows the rate law (-d[CH_(3)CH_(3)])/(dt)=K[C_(2)H_(6)] with overall K= ((K_(1)K_(2)K_(3)K_(4))/(K_(5))) , where K_(1),K_(2),K_(3),K_(4),K_(5) are the rate constants of various elementary steps.The values of E_(a) of elementary reactions were found to be E_(a_(1))=350(kJ)/(mol ) E_(a_(2))=2 (kJ)/(mol) E_(a_(3))=160(kJ)/(mol) E_(a_(4))=30(kJ)/(mol) , E_(a_(5))=10(kJ)/(mol) The activation energy of the overall reaction is xkJ/mol. The value of (x)/(5) is

A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are k1, k2, k3 and k5 respectively. The overall rate constant is is given by: k = k_(2)/k_(1) (k_(1)/k_(2))^(1/2) activation energy are 40,60, 50 and 10 kJ/mol respectively, find the overall energy of activation (kJ/mol).

Knowledge Check

  • A reacation takes place in three steps with actiation energy E_(a_(1)) =180 KJ/mol , E_(a_(2)) =80 KJ/mol , E_(a_(3)) =50 KJ/mol respectively overall rate constant of the reaction is k=[(k_(1)k_(2))/(k_(3))]^(2//3) the overall activation energy of reaction will be (Here k_(1),k_(2) a"and k_(3) are rate constant of first, second and third step respectively.):

    A
    140 KJ/mol
    B
    150 KJ/mol
    C
    43.44 KJ/mol
    D
    100 KJ/mol

  • A reaction takes place in three steps with individual rate constant and activation energy, {:(,"Rate constant","Activation energy"),("Step 1",k_(1),E_(a_(1))=180kJ //"mol"),("Step2", k_(2),E_(a_(2))=180kJ //"mol"),("Step3",k_(3),E_(a_(3))=180kJ //"mol"):} oveall rate constant, k=((k_(1)k_(2))/(k_(3)))^(2//3) overall activation energy of the reaction will be :

    A
    140 kJ/mol
    B
    150 kJ/mol
    C
    130 kJ/mol
    D
    120 kJ/mol

  • For a complex reaction A overset(k) rarr products E_(a1)=180kJ //mol e,E_(a2)=80kJ//mol ,E_(a3)=50kJ//mol Overall rate constant k is related to individual rate constant by the equation k=((k_(1)k_(2))/(k_(3)))^(2//3) . Activation energy ( kJ//mol ) for the overall reaction is :

    A
    100
    B
    43.44
    C
    150
    D
    140

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