Calculate the activation energy (in kJ/mol) of a reaction if the rate of the reaction increases by a factor of 3.5 when the temperature is increased from 40°C to 60°C. If the temperature is increased raised from 110°C to 130°C, by how much will the rate of the reaction increase?

Isomerization of n-butane to isobutane is a bit difficult to accomplish because it requires breaking C-C bonds. The activation barrier for the transformation is 120 kJ/mol. What fraction of n-butane molecules with an energy equal to or greater than the activation barrier exists at 455 K and 575 K. Also determine the ratio of the two fractions (at 575 K to 455 K).

The rate constant for the first-order decomposition of hydrogen peroxide into water and oxygen is 7.652×10⁻¹² s⁻¹ at 313 K and 2.516×10⁻¹⁰ s⁻¹ at 343 K. What is the value of the frequency factor for this reaction?

The table below shows the results of a kinetics study for the alkaline hydrolysis of ethyl acetate.
CH₃COOC₂H₅ + NaOH → CH₃COONa + C₂H₅OH

The reaction is second-order overall (First order in ethyl acetate and first-order in sodium hydroxide). Calculate the value of the rate constant at 10.0 °C.

In the graph shown below, each line correspond to a different reaction. Arrange the reactions in order of decreasing activation energy.

The activation energy of an uncatalyzed reaction is 95 kJ/mol. The addition of a catalyst lowers the activation energy to 55 kJ/mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25°C

The rate constant (k) for a reaction was measured as a function of temperature. A plot of ln k versus 1/T (in K) is linear and has a slope of −8193 K. Calculate the activation energy for the reaction.