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The rate constant is 2.84×10-3 L mol-1 s-1 at 335.0°C and 3.48×10-2 L mol-1 s-1 at 528.0°C.

Calculate the rate constant k at 413.0°C for this reaction.



Calculate the pre-exponential factor A for this reaction.

Jan 4th, 2015

Use the Arrhenius equation

k = Ae-Ea/RT

k1 = Ae-Ea/RT  ;   k2 = Ae-Ea/RT

In ( k1/k2) = Ea/R ( 1/T1 - 1/T2)

In ( 2.82 X 10-3 Lmol-1 s-1/ 3.48 x 10-2 Lmol-2 s-1) = Ea/8.314 ( 1/608 - `1/801)

In ( 0.081034) = Ea/8.314 ( 0.0016- 0.0012)

-2.512 = Ea/8.314 ( 0.0004)

8.314 X -2.512 = Ea ( 0.0004)

-20.89/ 0.0004 = Ea (0.0004)/0.0004)

Ea = -5.22 X 10^-4

 In K = ( - Ea/ R) ( 1/T) + In A

        = - (-5.22 X 10^-4/ 8.314) ( 1/ 686) + In A

        = 6264.73 X 0.00145 + 1

 In K = 9.13 + 1= 10.13

     K = e^10.13

         = 2.5 X 10^4

and In A =1
so, A = e^1 = 2.7183

Jan 4th, 2015

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