Use an Arrhenius plot to determine the activation barrier forthe reaction. Kj/mo
ID: 690334 • Letter: U
Question
Use an Arrhenius plot to determine the activation barrier forthe reaction. Kj/mol Use an Arrhenius plot to determine frequency factor for thereaction.s^-1 Any help appreciated Temperature Rate Constant 300 3.13×102 310 9.51×102 320 0.270 330 0.719 340 1.81 The following data show the rate constant of a reaction measured atseveral different temperatures. Use an Arrhenius plot to determine the activation barrier forthe reaction. Kj/mol Use an Arrhenius plot to determine frequency factor for thereaction.s^-1 Any help appreciatedExplanation / Answer
According to Arrehenius Equation , rate constant , K = A e-( Ea /RT ) ------(1) For two cases log ( K' / K ) = ( Ea / 2.303R ) [ ( T' - T )/ T' ] Ea = [ (2.303RT'T) / ( T' - T ) ] * log ( K'/K ) Consider the first two cases in the given table & plug thecorresponding values we get Ea =[ (2.303RT'T) / ( T' - T ) ] * log ( K'/K ) = [ (2.303* 8.314 * 310 * 300 ) / ( 310 -300 ) ] * log ( 9.51 * 10^-2 / 3.13*10^-2 ) = 85942.26 J = 85.942 KJ So , activation energy , Ea = 85.942 KJ From Equation (1) frequency factor ,A = K / e-( Ea /RT ) = 3.13 * 10^-2 / ( e - 85.942 * 1000 / ( 8.314 * 300) ) Considering thefirst case = 2.8837 * 10^13 s^-1 = 3.13 * 10^-2 / ( e - 85.942 * 1000 / ( 8.314 * 300) ) Considering thefirst case = 2.8837 * 10^13 s^-1Related Questions
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