15. Chemical Kinetics

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?

Using the Arrhenius Equation, if the activation energy for a reaction is 80 kJ/mol, at what temperature will the rate be ten times faster than at 0 degrees Celsius?

If an increase in temperature from 25°C to 35°C doubles the reaction rate constant, what is the activation energy of the reaction? Assume the Arrhenius equation applies.

Suppose that a catalyst lowers the activation barrier of a reaction from 122 kJ/mol to 54 kJ/mol. By what factor would you expect the reaction rate to increase at 25.00 °C? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are the same.)

The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower does the activation barrier have to be when sucrose is in the presence of the enzyme?