for decomposition reaction the value of RAR constant K at two different temperature are given below-

K1=2.15*10Lmol s at 650K

k2=2.39*10Lmol s at 700K

calculate the value of activation energy for this reaction(R=8.314)

Asked by Shomyajit Misra Misra | 6th May, 2014, 09:07: PM

Expert Answer:

Solution:

The Arrhenius equation is:

 

log k2/k1 = Ea [ T2 - T1/T1T2]

               2.303R

k 1 = 2.15 x10-8molL-1s-1

k 2 = 2.39 x 10-9molL-1s-1

T1 = 650 K

T2 = 700K

Substititing the values,

 

log (2.39 x 10-9/2.15 x10-8=   Ea                    [ 700 - 650/650x700]

                                             2.303 x 8.314

1.046 = Ea           [700 - 650/650x700]

            2.303 x 8.314

Ea = 1.046 x 2.303 x 8.314 x 650 x 700   =  182254Jmol-1 = 182.254kJmol-1

               50

 

Answered by Vaibhav Chavan | 7th May, 2014, 09:17: AM

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