The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the reaction at 343 K than at 322 K? (R = 8.314 J/mol • K)
The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the...
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 209 °C? (R = 8.314 J/mol • K)
The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M⁻¹s⁻¹, then what is the value of the rate constant at 121 °C? (R = 8.314 J/mol • K)
If a particular reaction has an activation enery, Ea, of 160 kJ/mol, how much faster is a reaction at 70 ∘C compared to the reaction at 25 ∘C? a. The reaction is approximately 875 times slower at the higher temperature. b. The reaction is approximately 4,800 times faster at the higher temperature c. The reaction is approximately 520 times faster at the higher temperature
What is the activation energy (in kJ/mol) of a reaction whose rate constant increases by a factor of 89 upon increasing the temperature from 307 K to 343 K? R = 8.314 J/(mol • K).
The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 35 × 10⁻⁴ s⁻¹ at 322 K, what is the rate constant at 273 K? An experimental plot of ln(k) vs. 1/T is obtained in lab for a reaction. The slope of the best-fit line for the graph is -3090 K. What is the value of the activation energy for the reaction in kJ/mol?
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...
A particular reaction has an activation energy, Ea, of 108 kJ/mol. If the rate constant for the reaction is 0.00573 s −1 at 498 °C, at what temperature(in°C) would the rate constant be 0.283 s −1?
The activation energy for a particular reaction is Ea =13.10 kJ What percentage of the molecules are at or above the activation energy at 500.0 K?
A certain reaction has an activation energy of 50.49 kJ/mol. At what Kelvin temperature will the reaction proceed 8.00 times faster than it did at 343 K?
For a given reaction, the activation energy is 61.5 kJ/mol. If the reaction rate constant is 5.23E-3 M-1s-1 at 38.0 °C, what is the reaction rate constant at -3.00 °C? (R = 8.314 J/K×mol)