3. The decomposition of di-tert-butyl peroxide (DTBP) is a first order reaction with a half- life of 320. minutes at 135 °C and 100. min at 145 °C. Calculate the activation energy for this reaction. (C4H9)2O2(g) → 2 (CH3)2CO(g) + C₂H6(g)

3. The decomposition of di-tert-butyl peroxide (DTBP) is a first order reaction with a half- life of 320. minutes at 135 °C and 100. min at 145 °C. Calculate the activation energy for this reaction. (C4H9)2O2(g) → 2 (CH3)2CO(g) + C₂H6(g)

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

At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.0770M NH₂OH(aq) → NH3(aq) + H₂O (aq) Suppose a vessel contains NH4OH at a concentration of 0.500M. Calculate how long it takes for the concentration of NH4OH to decrease by 77.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 : x10
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 617 K.
Sucrose (C12H22O11) hydrolyzes into glucose and fructose. The hydrolysis is a first-order reaction. The half-life for the hydrolysis of sucrose is 64.2 min at 25°C. How many grams of sucrose in 1.25 L of a 0.217 M solution are hydrolyzed in 1.73 hours?
The light-stimulated conversion of 11-cis-retinal to 11-trans-retinal is central to the vision process in humans. This reaction also occurs (more slowly) in the absence of light. At 80.0 ∘C in heptane solution, the reaction is first order with a rate constant of 1.02×10−5/s .Its initial concentration is 3.3×10−3 M. How many hours does it take for the concentration of 11-trans-retinal to reach 3.13×10−3 M ?
The thermal decomposition of sulfuryl chloride to sulfur dioxide and chlorineSOCl(g) SO(g) + Cl(g)is a first order reaction with a half-life of 2.3010 seconds. For this reaction what is the numerical value of k, the rate constant, in s?
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0039 M²s¯¹: 2N₂O(g) 2 N₂(g) + O₂(g) Suppose a 4.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 6.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 00 X 3
4) The decomposition of phosphorus pentachloride (PCIS) into phosphorus trichloride (PCI3) and chlorine gas (Cl2) is a first order process with a rate constant of 0.0842 s at a certain temperature. If 40.4 s after the reaction begins, the concentration of PCIs is 0.0203 M, what was the initial concentration of PCI3? (A) 6.76 x 104 M (B) 0.609 M (C) 3.42 M (D) (E) 0.495 M ES 0.820 Mt (D)
b Sulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s1). So,Cl2(g) → SO2(g) + Cl2(g) If the initial pressure of S02CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of SO2CI, remain after 11.7 h? molecules SO2CI2
Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 2 NO2(g) → 2 NO(g) + O2(g). When 0.665 M NO2 is allowed to react for 50.0 seconds, its concentration falls to 0.0954 M. What is the rate constant for the reaction? (in M1s-1)
The following chemical reaction: A → products shows second order kinetics with respect to A; rate = K[A]². If k = 11.99 x 10-³ mol-¹ L s¯¹ and the initial concentration of A is 1.45 mol L-1, what is the half life of this reaction in minutes? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
The reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) is 2nd order in NO and 1st order in Cl2. 5 mol of nitric oxide and 2 mol of chlorine were brought together in a volume of 2 dm3 and the initial rate was 2.4× 10–3 mol dm3 s–1. What will be the rate when half of the chlorine has reacted?
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.