15. Chemical Kinetics

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?

The activation energy Ea for a particular reaction is 50.0 kJ/mol. How much faster is the reaction at 313 K than at 310.0 K? (R = 8.314 J/mol • K)

The activation energy for a first-order reaction is 26.5 kJ/mol. At 10.0°C, the rate constant is 0.020 s⁻¹. Calculate the temperature at which the rate constant is 0.040 s⁻¹ using the Arrhenius Equation.

The 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?

Using 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?

Using 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?

Using the Arrhenius Equation, what is the rate constant (k) for the reaction of NO with F2 at a temperature of 298 K?

The rate constant for a reaction is 1 × 10⁻³ M sec⁻¹ at 27°C and the Arrhenius frequency factor is 3500 sec⁻¹. What is the activation energy?

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.

The rate constant of a chemical reaction increased from 0.100 s⁻¹ to 3.20 s⁻¹ upon raising the temperature from 25.0 °C to 55.0 °C. Calculate the value of (1/T1 - 1/T2) in Kelvin⁻¹, where T1 is the initial temperature and T2 is the final temperature.

The 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.

Using the Arrhenius Equation, what is the activation energy (Ea) for the reaction between nitrogen dioxide and carbon monoxide, given that the rate constant at 701 K is 2.57 M⁻¹·s⁻¹ and at 895 K is 567 M⁻¹·s⁻¹?