15. Chemical Kinetics

Using the Arrhenius Equation, calculate the activation energy (Ea) for the reaction between nitrogen dioxide and carbon monoxide given the rate constants at 701 K and 895 K are 2.57 M⁻¹s⁻¹ and 567 M⁻¹s⁻¹, respectively.

Using the Arrhenius Equation, what is the predicted rate constant for the reaction NO2(g) + CO(g) → NO(g) + CO2(g) at 525 K, given that the rate constant at 701 K is 2.57 M⁻¹·s⁻¹ and the activation energy is 1.5 × 10² kJ/mol?

Using the Arrhenius Equation, calculate the frequency factor (A) for the reaction NO2(g) + CO(g) → NO(g) + CO2(g) given the activation energy Ea = 1.50 × 10² kJ/mol, and rate constants k1 = 2.57 M⁻¹·s⁻¹ at 701 K and k2 = 567 M⁻¹·s⁻¹ at 895 K.

You wish to determine the activation energy for the following first-order reaction: A → B + C. How would you use the Arrhenius equation to determine the activation energy?