15. Chemical Kinetics

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?

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.

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.

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 38.0 kJ/mol. If the rate constant for this reaction is 1.60 x 10^2 M^-1s^-1 at 249 K, what is the rate constant at 436 K according to the Arrhenius Equation?

At 298 K, the decomposition of ammonia is catalyzed by tungsten. The activation energy for the catalyzed reaction is 163 kJ/mol. If in the absence of a catalyst, the activation energy is 335 kJ/mol, which of the following statements is true with reference to this reaction?

At 298 K, the decomposition of ammonia is catalyzed by tungsten. The activation energy for the catalyzed reaction is 163 kJ/mol. If in the absence of a catalyst, the activation energy is 335 kJ/mol, which of the following statements is true with reference to this reaction?

Chemists commonly use a rule of thumb that an increase in temperature of 10 K doubles the reaction rate. What must the activation energy be for this statement to be true if the change in temperature is from 25°C to 35°C?

Chemists commonly use a rule of thumb that an increase in temperature of 10 K doubles the reaction rate. What must the activation energy be for this statement to be true if the change in temperature is from 25°C to 35°C?

For two measured rate constants for the same reaction at different temperatures: Temperature / °C | k / s⁻¹ - 199 | 4.50 × 10⁻⁵ - 258 | 3.2 × 10⁻³ What is the activation energy (in kJ mol⁻¹) for this reaction?