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The rate constant for the decomposition of hydrocarbons is `2.418xx10^(-5)s^(-1)` at `546K`. If the energy of activation is `179.9kJ mol^(-1)`, what w

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The rate constant for the decomposition of hydrocarbons is 2.418×10-5s-1 at 546K . If the energy of activation is 179.9kJmol-1 , what will be the value of pre- exponential factor? Select the correct answer from above options

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Correct Answer - 3.9×1012s-10 k=2.418×10-5s-1,Ea=179.9kJmol-1,T=546K, Using Arrhenius equation, k=Ae-Ea/RT lnk=lnA- Ea RT orlogk=logA- Ea 2.303RT orlogA=logk+ Ea 2.303RT =log(2.418×10-5s-1)+ 179kJmol-1 2.303×8.314×10-3kJmol-1×546K orA=Antilog(12.5924)s)-1)=3.912×1012s-1

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