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?

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?

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.