Homework • Unanswered To double the rate of a reaction at T-25°C with an activation energy...
A reaction has an activation energy, Ea = 41.6 kJ mol-1 at 25 °C. By how many degrees must the temperature be raised in order to increase the reaction rate by a factor of 30. A) 2.0 B) 374 C) 29 D) 76 E) 6.0
A reaction has an activation energy, Ea = 41.6 kJ mol-1 at 25 °C. By how many degrees must the temperature be raised in order to increase the reaction rate by a factor of 30. A. 2.0 B. 6.0 C. 29 D. 374 E. 76 The following reaction takes place in an acidic solution As4O6(s) + MnO4-(aq) → AsO43-(aq) + Mn2+(aq) In the simplest balanced equation, the coefficients for each listed species are As4O6 MnO4- H+ A. 1,3,12 B. 3,5,36...
Part A: The activation energy of a certain reaction is 44.9 kJ/mol. At 25 ∘C, the rate constant is 0.0120s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Part B: Given that the initial rate constant is 0.0120s−1 at an initial temperature of 25 ∘C, what would the rate constant be at a temperature of 120. ∘C for the same reaction described in Part A?
The rate constant of a reaction is 0.049 1/s at 25.°C, and the activation energy is 39.041 kJ/mol. What is k at 76.4°C?
_13) The activation energy of a reaction is 100 kJ/mole. The increase in the rate constant when its temperature is raised from 295 to 300 K is approximately: A) 50% B) 100% C) 10% D) 25%
The activation energy of a particular reaction is 83.1 kJ/mol. By what factor will the rate constant increase when the temperature is increased from 50 °C to 60 °C?
a. A reaction has the following activation energy and reaction rate k constant at 20 °C 10,000 cal/mo k2 1.42 h Calculate: a. reaction rate constants for 10, 15, 20, 25, 30, 35 and 40 oC b.construct the Arrhenius plot (x-1/T versus y - log k) using the reaction rate constants calculated in a. calculate Qio for each pair of temperatures with the difference od 10°C, such as between 10 and 20°C., 15 and 25 °C, etc. (you will have...
The energy of activation for a particular reaction is 11.1 kJ/mol. At 18.9 °C the rate constant of the reaction is 1.67 × 102s.-1 Calculate the temperature (in °C) when the rate constant, k = 4.99 × 103s.-1 R = 8.314472 J⋅mol-1⋅K-1. Report your answer to THREE significant figures.
The activation energy of a certain reaction is 33.6 kJ/mol . At 23 ∘C , the rate constant is 0.0150s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Given that the initial rate constant is 0.0150s−1 at an initial temperature of 23 ∘C , what would the rate constant be at a temperature of 120. ∘C for the same reaction described in Part A?
A reaction that has a very high activation energy A reaction that has a very high activation energy gives a curved Arrhenius plot. has a rate that does not change much with temperature. must be first-order. must have a small activation energy for the reverse reaction. has a rate that is very sensitive to temperature.