Ethylene oxide is a reagent important in many chemical processes and also a major component in explosives. It is formed through the partial oxidation of ethylene: C2H4 + 1/2 O2 → C2H4C k1 = 6943 s-1 However, ethylene can also undergo a combustion reaction: C,H4 + 3/2 02 → co, + H,C kɔ = ? s- Assuming both reactions obey first order kinetics with excess oxygen and that after 1.1 minutes [C2H4O]/[CO2] = 7.2, what is the rate constant k2? %3D

Ethylene oxide is a reagent important in many chemical processes and also a major component in explosives. It is formed through the partial oxidation of ethylene: C2H4 + 1/2 O2 → C2H4C k1 = 6943 s-1 However, ethylene can also undergo a combustion reaction: C,H4 + 3/2 02 → co, + H,C kɔ = ? s- Assuming both reactions obey first order kinetics with excess oxygen and that after 1.1 minutes [C2H4O]/[CO2] = 7.2, what is the rate constant k2? %3D

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

Part B
The rate constant for this first‑order reaction is 0.0240 s−1 at 400 ∘C. A⟶products After how many seconds will 21.7% of the reactant remain? t=
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 hh at 25 ∘C∘C. If a 1.7 −L−L reaction vessel initially contains 760 torrtorr of N2O5N2O5 at 25 ∘C∘C, what partial pressure of O2O2 will be present in the vessel after 230 minutes?
For the reaction: 3 Ag + NO3– + 4 H+ –––> NO + 2 H2O + 3 Ag+ If the rate of disappearance of Ag is 0.0017 mol L–1 s–1, what is the rate of the appearance of water? For the 1st order reaction: A ––> products, assume the concentration of A falls to one-third of its original value after 150 seconds. Calculate the rate constant and the half-life.
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 rate constant for the decomposition of gaseous azomethane, CH3N=NCH3 → N2 + C₂H6 is 40.8 min¹ at 425 °C. Calculate the number of moles of CH3N=NCH3 and N₂ in a 1.00 L flask 0.0500 min after 2.00 g of CH3N=NCH3 is introduced.
The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.11 M, what is its concentration after exactly 11 minutes have passed? Round your answer to 2 decimal places.
The rate for the reaction H2 (g) + Br2 (g) 2 HBr (g)is first order in both H2 and Br2 concentrations, and the rate constant k at 287 \deg C is 5.87\times 10-4 L mol-1 s-1. Suppose 1.00 L of H2 (g) at a concentration of 6.60\times 10-2 M is rapidly mixed with the same volume of Br2 (g) also at a concentration of 6.60\times 10-2 M. Calculate the time (in seconds) required for the H2 concentration to decrease to a value of 2.55\times 10-2 M. (Enter your answer to three significant figures.)
Ibuprofen is an over the counter medicine used to alleviate pain. The metabolism of ibuprofen in the body follows first-order kinetics. For ibuprofen to be effective, the concentration within the body’s blood must stay above 5.3x10-5 M. A typical dose of ibuprofen is around 600 mg, which gives a concentration of 6.5x10-4 M. How long, in hours, will it take for a dose of 600 mg to reach the point where the ibuprofen is no longer effective? The rate constant for the metabolism of Ibuprofen if 0.0104 1/M min.
A certain first order reaction is 45.0% complete in 65 s. Determine the rate constant and the half-life for this process. K= t = S S -1