InterviewSolution
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InterviewSolution
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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/molB. 150 kJ/molC. 130 kJ/molD. 120 kJ/mol |
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Answer» Correct Answer - A `Ae^(-E_(a)//RT)=[(Ae^(-E_(a_(1))//RT)xxAe^(-E_(a_(2))//RT))/(Ae^(-E_(a_(3))//RT))]^(2//3)` `=[Ae^((-E_(a_(1))-E_(a_(2))+E_(a_(3)))//RT)]^(2//3)` `E_(a)=(2)/(3)[E_(a_(1))+E_(a_(2))-E_(a_(3))]` `=(2)/(3)[180+80-50]=140 ` kJ/mol |
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