Ethylene (ethene) is a precursor to many important products including polyethylene. It is produced along with other by- products from ethane in the temperature range 700 K - 900 K, in a reaction that includes the steps below. Note that the order of the steps is jumbled! Reaction 1: CH3 + CH3CH3 CH4 + CH3CH2 Reaction 2: CH3CH2'+ M → CH2CH2 + H'+ M Reaction 3: CH2CH2 + H'+ M → CH3CH2'+ M Reaction 4: H* + CH3CH3 H2 + CH3CH2 Reaction 5: H2 + CH3CH2' H' + CH3CH3 Reaction 6: H' + CH3CH2' CH3CH3 Reaction 7: CH3CH3 + M → 2CH3' + M

Ethylene (ethene) is a precursor to many important products including polyethylene. It is produced along with other by- products from ethane in the temperature range 700 K - 900 K, in a reaction that includes the steps below. Note that the order of the steps is jumbled! Reaction 1: CH3 + CH3CH3 CH4 + CH3CH2 Reaction 2: CH3CH2'+ M → CH2CH2 + H'+ M Reaction 3: CH2CH2 + H'+ M → CH3CH2'+ M Reaction 4: H* + CH3CH3 H2 + CH3CH2 Reaction 5: H2 + CH3CH2' H' + CH3CH3 Reaction 6: H' + CH3CH2' CH3CH3 Reaction 7: CH3CH3 + M → 2CH3' + M

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...

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he rate constant of a chemical reaction increased from 0.100 s−1s−1 to 3.30 s−1s−1 upon raising the temperature from 25.0 ∘C∘C to 43.0 ∘C∘C . Calculate the value of (1T2−1T1)(1�2−1�1) where T1�1 is the initial temperature and T2�2 is the final temperature. Express your answer numerically. View Available Hint(s)for Part ACalculate the value of ln(k2k1) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.Express your answer numerically.View Available Hint(s)for Part What is the activation energy of the reaction?Express your answer numerically in kilojoules per mole.View Available Hint(s)
Q6. Does the Rate Constant for the reaction between Parts B and C have the same value or are they different. Briefly explain your answer. Note: You do not need to carry out a calculation to answer this question
Consider the mechanism shown here:
3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/
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tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (
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