Reaction A
$$O3(g)+Cl(g)ClO(g)+O2(g)
$$A=2.93×10−11 cm3molecule • s and
Ea=2.16 kJmol
Reaction B
$$O3(g)+NO(g)NO2(g)+O2(g)
$$A=2.34×10−12 cm3molecule •
s Ea=11.6 kJmol
On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction A at 298 K.
On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction B at 298 K.
using Arrhenius equation we can calculate rate constant
Reaction A $$O3(g)+Cl(g)ClO(g)+O2(g) $$A=2.93×10−11 cm3molecule • s and Ea=2.16 kJmol...
Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g) ΔG° = - 34.5 kJ Please explain how you enter it into the calculator I get 1.23*10^-14. Which is incorrect the answer is 1.12*10^-6.
1. Consider the following reaction: O3(g)→O2(g)+O(g) Using the results of the Arrhenius analysis (Ea=93.1kJ/mol and A=4.36×1011M⋅s−1), predict the rate constant at 298 K . Express the rate constant in liters per mole-second to three significant figures. 2. Why is knowledge of reaction rates important (both practically and theoretically)?
Consider the following reaction: O3(g)→O2(g)+O(g) Using the results of the Arrhenius analysis (Ea=93.1kJ/mol and A=4.36×1011M⋅s−1), predict the rate constant at 308 K . Express the rate constant in liters per mole-second to three significant figures.
Ozone decomposes to form oxygen molecules and oxygen atoms, O3(g) ? O2(g) + O(g), in the upper atmosphere. The energy of activation for this reaction is 93.1 kJ/mol. At 600 K, the rate constant for this reaction is 3.37
5. The decomposition of ozone is important to many atmospheric reactions: O3(g) à O2(g) + O(g) A study of the kinetics of the reaction resulted in the following data: Temperature (K) Rate Constant (M-1·s-1) Temperature (K) Rate Constant (M-1·s-1) 600 3.37 x 103 1300 7.83 x 107 700 4.85 x 104 1400 1.45 x 108 800 3.58 x 105 1500 2.46 x 108 900 1.70 x 106 1600 3.93 x 108 1000 5.90 x 106 1700 5.93 x 108 1100...
2Ca(s)+O2(g)→2CaO(s) ΔrH∘= -1269.8 kJmol−1; ΔrS∘= -364.6 JK−1mol−1 Calculate the Gibbs energy change for the reaction at 24 ∘C. Express your answer using four significant figures. 2Ca(s) + O2 (g) → 2CaO(s) Δ,Ho =-1269.8 kJ mol 1: Δ,S":-3646 J K 1 mol 1 Part A Calculate the Gibbs energy change for the reaction at 24 °C. Express your answer using four significant figures. kJ mol 1 Submit Previous Answers Request Answer
The first order elementary reaction: A + B + C was carried out in a constant volume batch reactor isothermally at 328 K. The concentrations of species A, CA, were recorded as a function of time, as given in the following table. The activation energy Ea=120 kJ/mol. 0.9 6 t (min) CA (mol/dm) 0 20 0.5 17.4 1.5 12.9 2.2 10.5 4 6.2 15.5 8.3 3.5 Based on integral method: b) Process the data using the above table and the...
The reaction 2 NO2(g) → 2 NO (g) + O2(g) has rate constants of 2.70 x 10-2 M-1s-1 at 227 oC and 0.240 M-1s-1 at 277oC. What is the activation energy of this reaction? (Given: Arrhenius equation, k = Ae-Ea/RT ) A) 99.6 kJ/mol B) 22.8 kJ/mol C) 49.8 kJ/mol D) -22.8 kJ/mol E) 65.3 kJ/mol I'm unsure on how to do it since you're not given the frequency factor
Consider the reaction 2HI(g)→H2(g)+I2(g). At 585 K, the rate constant is 9.64×10−5Lmol s. At 690. K, the rate constant is 2.83×10−3Lmol s. Use the Arrhenius equation to calculate the activation energy for the reaction. Ea=−R[lnk2−lnk1(1T2)−(1T1)] Provide your answer below:
1. Consider the following reaction: 2N2Os(g) → 4NO2(g) + O2(g), with the rate constant (k (s')) determined as a function of temperature: T(°C) k 2.0 x 105 7.3 x 103 2.7 x 10+ 9.1 x 104 2.9 x 10 50 60 What is the activation energy for this reaction? HINT: You will need to make a plot of these data.