A certain reaction has an activation energy of 70.0 kJ/mol and a frequency factor of A = 2.60 × 10^12 M⁻¹·s⁻¹. Using the Arrhenius equation, what is the rate constant, k, of this reaction at 30.0 °C?

A common rule of thumb in organic chemistry is that increasing the temperature of a reaction at room temperature by 10°C doubles the rate. Calculate the activation energy (Ea) for a reaction that follows this rule of thumb. Assume room temperature is 25°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?

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.

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 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.