We know
log(K2/K1)=Ea.(T2-T1)/2.303R.T1.T2
Where K1,K2= rate constant
T1,T2= temperatures
R=8.314
Substituting values. In above equation we can get
Ea=74.6KJ/mol
Calculate the activation energy of a reaction if the rate constant at 555 K is 3.72...
7. Calculate the rate constant at 70°C for the reaction A + 3B-> 2C given that the rate constant of the reaction is equal to 3.5x10 'M's' at 100°C. (Ea=142 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...
How can I do the calculation Calculate the activation energy, E_a, for the reaction 2N_2O_5(g) rightarrow 4NO_2(g) + O_2(g) from the observed rate constants: k = 3.46 times 10^-5 s^-1 at 25 degree C and k = 1.5 times 10^-3 s^-1 at 55 degree C. a. 1437 kJ/mol b. 102 kJ/mol c. 0.101 kJ/mol d. 9.62 kJ/mol e. 1.04 kJ/mol
Calculate the rate constant, k, for a reaction at 70.0 °C that has an activation energy of 90.0 kJ/mol and a frequency factor of 2.26×1011 s−1.
Calculate the rate constant, k, for a reaction at 70.0 °C that has an activation energy of 77.2 kJ/mol and a frequency factor of 1.15 x 1011 s-1
Calculate the rate constant, k , for a reaction at 63.0 °C that has an activation energy of 82.2 kJ/mol and a frequency factor of 7.53 × 10 11 s−1.
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)
The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightarrow 2C_2H_4(g) At 600.0 K the rate constant is 6.1 times 10^-8 s^-1. What is the value of the rate constant at 870.0 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?