I DO NOT GET THIS SO PLEASE EXPLAIN WHEN ANSWERING. Explain how did they figure out the slope, how did they find the y-intercep, I thought the equation is k=Ae^-Ea/RT why did they make it so that slope = -Ea/R and intercept = lnA.
This book asumes alot of these without explaining or teaching, so please help. ALSO SOLVE 14.7!!!!
The decomposition of ozone shown here is important to many atmospheric reactions 03(g)02(g) +O(g) A study of the kinetics of the reaction results in the following data Rate Constant (M-1 s-1 3.37 Ã 103 4.85 Ã 104 3.58 Ã 105 1.70 Ã 106 5.90 Ã 106 1.63 Ã 10 3.81 Ã 107 Temperature (K) 1300 1400 1500 1600 1700 1800 1900 Rate Constant (M-1.s-1) 7.83 Ã 107 1.45 Ã 108 246 Ã 108 3.93 Ã 108 5.93 Ã 108 8.55 Ã 108 1.19 Ã 109 Temperature (K) 600 700 800 900 1000 1100 1200 Determine the value of the frequency factor and activation energy for the reaction SOLUTION To determine the frequency factor and activation energy, prepare a graph of the natural log of the rate constant (In k) versus the inverse of the temperature (1/T) 25 20 15 The plot is linear, as expected for Arrhenius behavior. The line that fits best has a slope of-1.12 Ã 104 K and a y-intercept of 26.8. Calculate the activation energy from the slope by setting the slope equal to -Ea/R and solving for Ea: ë 10 Slope y-intercept y=-1.12 Ã 104x + 26.8 1.12 Ã 104 K = 0 0 0.0005 0.001 0.0015 0.002 Ea = 1.12 Ã 104 K( 8.314 1/T (K) mol K = 9.31 Ã 104 J / mol 93.1 Ljmol Calculate the frequency factor (A) by setting the intercept equal to In A 26.8 In A 8 = 4.36 Ã 1011 Since the rate constants are measured in units ofM-1 - s1, the frequency factor is in the same units. Consequently, you can conclude that the reaction has an activation energy of 93. 1 W/mol and a frequency factor of 4.36 Ã 1011 M-1 . S-1 FOR PRACTICE 14.7 For the decomposition of ozone reaction in Example 14.7, use the results of the Arrhenius analysis to predict the rate constant at 298 K.