Multiple Choice
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.
15. Chemical Kinetics
Arrhenius Equation
Back15. Chemical Kinetics
Arrhenius Equation
- Multiple ChoiceAt 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?
- Multiple Choice
The following data shows the rate constant of a reaction measured at numerous temperatures. Use the Arrhenius plot to determine the frequency factor for the reaction.
1views - Multiple ChoiceUsing 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?
- Multiple ChoiceSuppose 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.)
- Multiple ChoiceUsing 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?
- Multiple Choice
The rate constant of a reaction at 32°C is 0.060/s. If the frequency factor is 3.1 × 1015 s–1, what is the activation barrier?
1views - Multiple ChoiceA certain first-order reaction has a rate constant of 2.63 x 10^-2 s^-1 at 22.0°C. What is the value of the rate constant k at 75.0°C if the activation energy Ea is 76.9 kJ/mol?
- Multiple ChoiceThe 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.
- Multiple ChoiceAt 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?
- Multiple ChoiceA 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?
- Multiple ChoiceA 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?
- Multiple ChoiceIf 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.
- Multiple ChoiceA 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?
- Multiple ChoiceThe 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?