Using the Arrhenius Equation, what is the activation energy (Ea) in kJ/mol for a reaction with a rate constant of 0.000122 s⁻¹ at 27 °C and 0.228 s⁻¹ at 77 °C?

A particular first-order reaction has a rate constant of 1.35 × 10^2 s⁻¹ at 25.0°C. What is the magnitude of the rate constant k at 95.0°C if the activation energy Ea is 55.5 kJ/mol?

A particular first-order reaction has a rate constant of 1.35 × 10² s⁻¹ at 25.0°C. Using the Arrhenius equation, what is the rate constant (k) at 95.0°C if the activation energy (Ea) is 55.5 kJ/mol?

A particular first-order reaction has a rate constant of 1.35 x 10^0 s^-1 at 25°C. What is the magnitude of the rate constant k at 75.0°C if the activation energy Ea is 55.3 kJ/mol?

Using the Arrhenius Equation, calculate the activation energy (Ea) in kilojoules per mole for a reaction with rate constants of 0.000116 s⁻¹ at 25 °C and 0.305 s⁻¹ at 85 °C. Express your answer to three significant figures.

A reaction has a rate constant of 0.0117 s⁻¹ at 400.0 K and 0.689 s⁻¹ at 450.0 K. Using the Arrhenius equation, what is the value of the rate constant at 425 K?

A reaction has a rate constant of 1.21×10⁻⁴ s⁻¹ at 25 °C and 0.225 s⁻¹ at 75 °C. What is the value of the rate constant at 17 °C when the activation energy (Ea) is 130 kJ/mol? Express your answer in units of inverse seconds (s⁻¹) and with 3 significant figures.

A reaction is followed and found to have a rate constant of 3.36 x 10^4 M^-1 s^-1 at 344 K and a rate constant of 7.69 M^-1 s^-1 at 219 K. Determine the activation energy for this reaction.

A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60 × 10⁻⁶ s⁻¹ at 275 K, what is the rate constant at 366 K according to the Arrhenius Equation?