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

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 :

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 :

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

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).

A reaction takes place in three steps. The rate constant are k_(1), k_(2) and k_(3) . The overall rate constant k=(k_(1)k_(3))/(k_(2)) . If E_(1), E_(2) and E_(3) (energy of activation) are 60, 30 and 10 kJ, respectively, the overall energy. Of activation is

A reaction takes place in theee steps: the rate constant are k_(1), k_(2), and k_(3) . The overall rate constant k=(k_(1)k_(3))/(k_(2)) . If E_(1), E_(2) , and E_(3) (energy of activation) are 60, 30 and 10kJ , respectively, the overall energy of activation is