Arrhenius Equation

  1) The rate constant for the first-order dehydration of tert-butyl alcohol at 500^oC is 1.20 x 10^-4 s^-1. The rate constant for this process at 600^oC is 6.80 x 10^-3 s^-1. Calculate the activation energy for this reaction.

     (a) -227 kJ/mol

     (b) 227 kJ/mol

     (c) 318 kJ/mol

      (d) 100. kJ/mol

     (e) -100. kJ/mol

  2) Use the graph to the right to calculate the rate constant for the following reaction at 40.0ºC.

CH₃CH₂NO₂(aq) C₂H₂(g) + HNO₂(aq)

     (a) 3.1 x 10^-18 sec^-1

     (b) 9.56 x 10^-15 sec^-1

     (c) -8.3 x 10⁵ sec^-1

     (d) -6.5 x 10⁶ sec^-1

  3) The activation energy for the isomerization of cyclopropane to propene is 274 kJ/mol. By what factor does the rate of reaction increase as the temperature rises from 500^oC to 550^oC?

     (a) 1.0

     (b) 13

     (c) 2.6

      (d) 4.0 x 10²

  4) The rate constant for a certain first-order reaction at 27^oC is 4.9 x 10^-4 s ^-1 and is 0.18 s^-1 at 227^oC. Calculate the activation energy for this reaction.

     (a) 8.55 x 10⁴ kJ/mol

     (b) 9.80 x 10⁴ kJ/mol

     (c) 3.68 x 10⁴ kJ/mol

      (d) -1.50 x 10³ kJ/mol

     (e) 1.50 x 10³ kJ/mol

  5) Use the graph to the right to calculate the rate constant for the following reaction at 40.0ºC.

C₂H₅Cl(aq) C₂H₄(g) + HCl(aq)

     (a) -9.29 x 10⁶ sec^-1

     (b) -1.51 x 10⁶ sec^-1

     (c) -57.0 sec^-1

     (d) 1.70 x 10^-25 sec^-1

 6) The reaction rate triples when the temperature increases from 15 ^oC to 35 ^oC for a particular reaction. What is the activation energy for this reaction?

     (a) 2.39 x 10² J/mol

     (b) 2.06 x 10^-3 J/mol

     (c) 7.92 x 10^-2 J/mol

     (d) 4.05 x 10⁴ J/mol