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

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 (

Consider the following equation: H2CO3 (aq)        →        H2O (l)   +    CO2 (g)     Rate = k [HCO3-]2     Rate = - ∆ [CO2]/ 2 ∆t     Rate =k [CO2]n     Rate =  ∆ [H2O]/ ∆t     Rate =  -k (∆[H2CO3]/ (3 ∆t)