1. The gas-phase reaction between methane and diatomic sulfur is given by the equation CH₂(g) + 2 S₂(g) → CS₂(g) + 2 H₂S(g) At 550°C the rate constant for this reaction is 1.1 L/mol. s, and at 625°C the rate constant is 6.4 L/mol. s. Calculate the activation energy for this reaction in J/mol A. 24.9 B. 1.4x105 C. 6.4x103 D. 22.6 E. 53.8

1. The gas-phase reaction between methane and diatomic sulfur is given by the equation CH₂(g) + 2 S₂(g) → CS₂(g) + 2 H₂S(g) At 550°C the rate constant for this reaction is 1.1 L/mol. s, and at 625°C the rate constant is 6.4 L/mol. s. Calculate the activation energy for this reaction in J/mol A. 24.9 B. 1.4x105 C. 6.4x103 D. 22.6 E. 53.8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

One mechanism for the destruction of ozone in the upper atmosphere is Os (9) + NO(g) → NO₂(g) + O2(g) Slow NO₂(g) + 0(g) → NO(g) + O₂(g) Fast Overall reaction O3(g) + O(g) → 20₂ (g) a. Which species is a catalyst? ONO 003 002 O NO2 b. Which species is an intermediate? ONO 003 002 O NO₂ c. E₂ for the uncatalyzed reaction 03 (g) + 0(g) → 20₂ (g) is 14.0 kj. E for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 85°C? Assume the frequency factor A is the same for each reaction. Ratio = [References) Submit Answer Try Another Version frem atempt remaning (Pr Previous
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning The reaction C,H, (g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 750.0 K? k = 1.34 x103 Incorrect
4. A certain chemical reaction has a rate constant of 1.50 L/mol·min at 45.0°C with an activation energy of 108.0 kJ/mol. Calculate the value of the rate constant for the reaction at 60.0°C.
Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,O,(aq) 2 H₂O(1) + O₂(g) The activation energy for this reaction is 75 kJ.mol-¹. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ.mol-¹. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K
16. The decomposition of hydrogen bromide is 2 HBr(g) → H2(g) + Br2(g) The reaction has rate constants of 7.23 x 10-8 M-1 s-1 at 5.00 x 102 K and 9.14 x 10-6 M-1 s-1 at 6.00 x 102 K. What is the activation energy in kJ/mol? Group of answer choices 136 kJ/mol none of the answers are correct 145 kJ/mol 107 kJ/mol 121 kJ/mol
A certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% V
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol
The activation energy for the following reaction is 125 kJ/mol, and AE for the reaction is -216 kJ/mol. NO₂(g) + CO(g) → NO(g) + CO₂(g) What is the activation energy for the reverse reaction NO(g) + CO₂(g) → NO₂(g) + CO(g) Please enter your answer as a real number only. (The units should be kJ/mol, but leave that off. Just enter a number like 420.3. But don't enter 420.3. Enter the correct answer.)
A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104
If the rate constant for a reaction triples when the temperature rises from 3.00 × 10² K to 3.19 × 102 K, what is the activation energy of the reaction? The gas constant Ris 8.3145 x 10³ kJ/mol. K. Activation energy = kJ/mol
The activation energy of a certain reaction is 41.8 kJ/mol . At 29∘C , the rate constant is 0.0180s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Solve the following equation for T2: ln ⁡(k2/k1) = Ea/R (1/T1−1/T2) The temperatures must be in kelvins and the activation energy must be in J/mol. Use the following value for the gas constant: R=8.314 J/mol⋅K.
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 258.0 °C 3.9 x 1010 153.0 °C 1.5 × 1010 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E х10 a mol