15. Chemical Kinetics

The activation energy for a first-order reaction is 26.5 kJ/mol. At 10.0°C, the rate constant is 0.020 s⁻¹. Calculate the temperature at which the rate constant is 0.040 s⁻¹ using the Arrhenius Equation.

The activation energy for the decomposition of HI(g) to H2(g) and I2(g) is 186 kJ/mol. The rate constant at 555 K is 3.52 × 10^-7 L/mol-s. What is the rate constant at 645 K?

Using the Arrhenius Equation, what is the rate constant at 40°C for the reaction: Fe(phen)3 2+ + 3 H3O+ + 3 H2O → Fe(H2O)6 2+ + 3 phenH+, given that the activation energy, Ea, is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10^-3 s^-1?

Using the Arrhenius Equation, what is the rate constant (k) for the reaction of NO with F2 at a temperature of 298 K, given that the activation energy (Ea) is 6.30 kJ/mol and the frequency factor (A) is 6.00 × 10^8 M⁻¹·s⁻¹?

Using the Arrhenius Equation, what is the rate constant (k) for the reaction of NO with F2 at a temperature of 298 K?

The rate constant for a reaction is 1 × 10⁻³ M sec⁻¹ at 27°C and the Arrhenius frequency factor is 3500 sec⁻¹. What is the activation energy?

Using the Arrhenius Equation, calculate the activation energy for the decomposition of acetaldehyde, CH3CHO, given that the rate constant is 1.1 × 10⁻² L mol⁻¹ s⁻¹ at 703 K and 4.95 L mol⁻¹ s⁻¹ at 865 K.

The rate constant of a chemical reaction increased from 0.100 s⁻¹ to 3.20 s⁻¹ upon raising the temperature from 25.0 °C to 55.0 °C. Calculate the value of (1/T1 - 1/T2) in Kelvin⁻¹, where T1 is the initial temperature and T2 is the final temperature.

The reaction N2 + O2 → 2NO takes place in the gas phase. The rate constant at 250 K is 4.32 × 10^13 M⁻¹s⁻¹, and at 275 K the rate constant is 8.19 × 10^13 M⁻¹s⁻¹. Calculate the frequency factor (A) for the reaction using the Arrhenius equation.

Using the Arrhenius Equation, what is the activation energy (Ea) for the reaction between nitrogen dioxide and carbon monoxide, given that the rate constant at 701 K is 2.57 M⁻¹·s⁻¹ and at 895 K is 567 M⁻¹·s⁻¹?

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?