Consider the mechanism shown here: 2 NO N202 N202 + H2 → N20 + H20 (slow step) N20 + H2→N2 + H2O What is the molecularity of the 2nd step? Oa. termolecular Ob. unimolecular Oc C. amolecular Od. bimolecular
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Q: Number 2
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- Determine the molecularity of the rate limiting step in this mechanism: S1 (fast): C6H6 + Br2 + FeBr3 --> C6H5Br+ + FeBr4 - S2 (slow): C6H5Br+ + FeBr4 - --> C6H5Br + HBr + FeBr3 a.) unimolecular b.) bimolecular c.) trimolecular d.) can't be determinedIs the proposed mechanism below valid or invalid? Justify your answer.Overall reaction: 2NO2(g) + F2(g) → 2NO2F(g) ________________________________________________Step 1: NO2(g) + F2(g) →NO2F(g) + F(g) slow Step 2: F(g) + NO2(g) → NO2F(g) fastThe acid-catalyzed hydrolysis of sucrose occurs by the fol-lowing overall reaction whose kinetic data are given below:C₁₂H₂₂O₁₁(s) H₂O(l) →C₆H₁₂O₆(aq) C₆H₁₂O₆(aq) (a) Determine the rate constant and the half-life of the reaction.(b) How long does it take to hydrolyze 75% of the sucrose?(c) Other studies have shown that this reaction is actually sec-ond order overall but appears to follow first-order kinetics.(Such a reaction is called a pseudo–first-order reaction.) Sug-gest a reason for this apparent first-order behavior.
- Consider a reaction is of second order with respect to one of the reactants. How will the rate of reaction be affected if the concentration of this reactant is (i) tripled, and (ii) reduced to half?The 4 molecules are reacting with CH3S- in acetone. Which transition state numbered 1-4 represents A, B, C, and D? Why?The reaction A → C proceeds by a stepwise mechanism: A → B, overall ΔE = 73 kJ/mol; Ea = 97 kJ/mol B → C, overall Δ E = -103 kJ/mol; Ea = 132 kJ/mol Which step is rate-determining?
- Helppppppp meeeeeee Catalyzed reaction how many stepppss??Consider the following energy profile. (a) How many elementary reactions are in the reactionmechanism? (b) How many intermediates are formed inthe reaction? (c) Which step is rate limiting? (d) For theoverall reaction, is ΔE positive, negative, or zero?The mechanisms shown below have been proposed to explain the kinetics of the reaction2 NO (g) + 2 H2 (g) ⇄ N2 (g) + 2 H2O (g)Mechanism IH2 (g) + 2 NO (g) ⇄ N2O (g) + H2O (g) (fast)H2 (g) + N2O (g) H2O (g) + N2 (g) (slow)Mechanism IIH2 (g) + 2 NO (g) N2O (g) + H2O (g) (slow)H2 (g) + N2O (g) ⇄ H2O (g) + N2 (g) (fast)Mechanism IIIH2 (g) + NO (g) 2 H2O (g) + N (g) (slow)N (g) + NO (g) ⇄ N2 (g) + O (g) (fast)H2 (g) + O (g) H2O (g) (fast)Which is consistent with the following experimental data?
- The following mechanism is proposed: C6H5COOH ⇌ C6H5CO2H2+ (fast) C6H5CO2H2+ ⇌ C6H5CO+ + H2O (fast) C6H5CO+ + HX + H2O ⟶ C6H6NH2 + N2 + CO2 (slow) The overall rate constant for this reaction is 0.200x 10-3L mol-1 s-1. Is this value consistent with rate law r = kobs*[C6H5COOH]*[HX] ?Chemistry pls help figure out this mechanismTable 1 with temperature and rate constants Temperature (oC) Rate constants KH (min-1) 61.0 7.13*10-6 71.2 2.77*10-5 Mark and Anthony have considered the following reaction for urea NH2CONH2 in 0.1M HCl: NH2CONH2 + 2H2O --> 2NH+2 + CO2-3 and the rate constant for the reaction is k1. Stephan and Kurt have been in the laboratory and measured rate constants for the reaction at two different temperatures. The measurement results are given in Table 1. 1) You must write down expressions for the changes in time for the concentrations of the reactants and products. That is, determine d[X]/dt, where [X] is the concentration of either reactants or products and write this down using concentrations and the rate constant. 2) You must use the Arrhenius expression to determine the activation energy for the reaction. 3) You must use the Arrhenius expression to determine the pre-exponential factor in the Arrhenius expression.