The calculation of activation energy is given bellow
1. Consider the following reaction: 2N2Os(g) → 4NO2(g) + O2(g), with the rate constant (k (s'))...
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
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9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the first order kinetics with rate constant of 4.8 x 10's. (a) if the initial 165 x 10-2M what is the concentration at 825 s? (b) How long it will take for concentration is 1.65 x 10-2M what is the concentrat the concentration of N2Os to decrease to 1.00 x 10-2M? t 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
#14 Rate Constant and Temperature 1. The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T (in K) is linear and has a slope of -1.01 x 104 K. Calculate the activation energy for this reaction. 2. The rate constant of a reaction at 32.0oC is 0.0550 s-1. If the frequency factor is 1.20 x 1013 s-1, what is the activation energy? 3. A reaction has a rate constant of...
Variation of the rate constant with temperature for the first-order reaction 2N2(g) + O(g) → 2N2O4(g) is given in the following table. Determine the activation energy and pre-exponential factor for the reaction. What would be the rate constant at 350 K? Temperature / K Rate Constant / s-1 273 7.87 x 103 298 3.46 x 105 318 4.98 x 106 338 4.87 x 107 What is the activation energy in kJ/mol? Do not enter the units with your answer. What...
20. Consider the reaction 2N2O5(g)4NO2(g) + O2(g) at 25 C for which the following data are relevant: Дн 13.30 kJ/mol 355.7 J/K mol N205 33.15 kJ/mol 239.9 J/K mol NO2 0 kJ/mol 204.8 J/K mol О2 Calculate AG° for the reaction at 25°C a. 1.35 x 105 kJ b. 94.7 kJ c. -29.0 kJ d. 135 kJ е. O kJ
7) The rate constant for the reaction 2N2O5(g) 25°C 4NO2(g) +O2(g) is k = 3.38x10-5/s at a) Enter the half-life of N20s in seconds. Use two significant figures and do not enter units b) Enter the total pressure in kPa 10 seconds after initiation of the reaction if initially there was 88.3kPa of pure N2O5 vapor. Use two significant figures and do not enter the units c) Enter the total pressure in kPa 10 minutes after initiation of the reaction...
Consider the rate of decomposition: 2 N2O5(g) → 4NO2(g) + O2(g). The rate of reaction will be dependent on: A. [N2O5] B. [NO2] C. [O2] D. [NO2] and [O2]
12) The rate of the elementary reaction CS2 + O2 ---> CS + SO2 has been studied as a function of temperature between 1500 and 2100 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 1500 2.18×104 1620 4.82×104 1740 9.57×104 1860 1.74×105 (a) Calculate the activation energy of this reaction. ___ kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. ___...
The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T(in K) is linear and has a slope of −1.12×104 K . Calculate the activation energy for the reaction. Express your answer using three significant figures with the appropriate units.
The Arrhenius equation for the dependence of the rate constant, k, on temperature is given by In k = + In A, where A is the frequency factor, R is the ideal gas constant, and EA is the activation energy. The rate of conversion of cyclo-propane to propene in gas phase was measured over the temperature range 750-900 K, and the rate constants that were found are reported below. Hint: think about what the following equation means In = (1,...