The following data show the rate constant of a reactionmeasured at several diffe

Question

The following data show the rate constant of a reactionmeasured at several different temperatures: Temp (K) Rate constant (1/s) lnk 1/T 310 .00434 -5.44 .003 320 .0140 -4.27 .00313 330 .0421 -3.17 .00303 340 .118 -2.14 .00294 350 .316 -1.15 .00286 I graphed the ln(k) vs 1/T and got Ea = 95.7 kJ/molwhich is correct I need to use an Arrhenius plot to determine the frequencyfactor for the reaction: A=         s-1 from my graphing calculator I got a y-intercept =31.73 then used A = e31.73 =6.03x1013 but this was wrong. Any help would be great.Promise to rate. K8 The following data show the rate constant of a reactionmeasured at several different temperatures: Temp (K) Rate constant (1/s) lnk 1/T 310 .00434 -5.44 .003 320 .0140 -4.27 .00313 330 .0421 -3.17 .00303 340 .118 -2.14 .00294 350 .316 -1.15 .00286 I graphed the ln(k) vs 1/T and got Ea = 95.7 kJ/molwhich is correct I need to use an Arrhenius plot to determine the frequencyfactor for the reaction: A=         s-1 from my graphing calculator I got a y-intercept =31.73 then used A = e31.73 =6.03x1013 but this was wrong. Any help would be great.Promise to rate. K8 from my graphing calculator I got a y-intercept =31.73 then used A = e31.73 =6.03x1013 but this was wrong. Any help would be great.Promise to rate. K8 Temp (K) Rate constant (1/s) lnk 1/T 310 .00434 -5.44 .003 320 .0140 -4.27 .00313 330 .0421 -3.17 .00303 340 .118 -2.14 .00294 350 .316 -1.15 .00286

Explanation / Answer

We Know that :     According to Arrehenius equation :         K = Ae-Ea/ RT                                      K - Rate Constant                                                                               Ea - Activation Energy                                          R - Gas Constant                                           T - Temperature of the Reaction                                             A - Frequency factor        A =  K / e -Ea / RT             = 0.00434 s-1 / e - 95.7 x 1000 J / mol   / ( 8.314 J / mole - K x 310 K )                  =   5.7593 x 1013 s-1 .             = 0.00434 s-1 / e - 95.7 x 1000 J / mol   / ( 8.314 J / mole - K x 310 K )                  =   5.7593 x 1013 s-1 .

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