The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.

The decomposition of hydrocarbon follows the equation

k = (4.5 × 10¹¹s^–1) e^-28000K/T. Calculate E_a.

The rate constant for the first order decomposition of H₂O₂ is given by the following equation: log k = 14.34 – 1.25 × 10⁴K/T

Calculate E_a for this reaction and at what temperature will its half-period be 256 minutes?

The decomposition of A into product has value of k as 4.5 × 10³ s^–1 at 10°C and energy of activation 60 kJ mol^–1. At what temperature would k be 1.5 × 10⁴s^–1?

The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of A is 4 × 10¹⁰s^–1. Calculate k at 318K and E_a.