A student ran several experiments for this reaction: 5 CH3COOH(aq) + 8 MnO4 (aq) + 24 H*(aq) → 8 Mn2 (aq) + 10 CO₂(g) + 22 H₂O(l) One of the experiments gave this data: Experiment # [CH3COOH) (M) 0.269 3 [MnO4] (M) 0.395 The student determined the rate law to be: ratek [CH3COOH)² [MnO4)² [H*] Calculate k for this reaction. I [H*] (M) 0.245 initial rate (M/s) 0.228

Be sure to answer all parts. The rate law for 2 NO(g) + O2(g)→ 2 NO2(g) is rate = k[NO]°[O2l. %3D The following mechanisms have been proposed: I. 2 NO(g) + O2(g)→ 2 NO2(g) II. 2 NO(g) = N½O2(g) [fast] N,O2(g) + O2(g) → 2 NO,(g) [slow] III. 2 NO(g) = N,(g) + O2(g) [fast] N2(g) + 2 O2(g) → 2 NO2(g) [slow] (a) Which of these mechanisms is consistent with the rate law? Check all that apply. I. II. III. None of the above (b) Which of these mechanisms is most reasonable? I. II. III.

Questions 2A 2B and 2C please

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Suggest a mechanism behind the reaction    NO(g) + Cl2(g)  à  NOCl(g)  + Cl(g) with the rate law    rate = k [NO]2 [Cl2]   This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2                 (slow)       2NO   +   Cl2    à   ……….                  (fast).                                à  …………                                NO     +     Cl2.     à    NOCl    +    Cl

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]

Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104

Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245

The chemical reaction A(aq) + B(aq) à C(aq) + D(aq) + E(aq) has an experimentally determined rate law of rate = k[A][B]. An experiment using the method of isolation was used to determine the order with respect to CH3I. This experiment yielded the following Rate law: rate = k’[A]. What is true of this experiment and its findings? the experiment illustrated that the reaction pseudo 2nd order     [A]>>>[B]                  [A] = [B]                    [A]<<<[B}