Consider the following mechanism for the formation of tert-butanol: (CH3) CBr(aq) (CH3), C+ (aq) (CH₂)₂C¹ (aq) + OH¯(aq) → (CH₂)¸COH(aq) 1 Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. 0 + Br (aq) yes no (1) (2) ローロ 0.0. X e

Propose a reaction pathway consisting of only a unimolecular or bimolecular steps for the 2A+B-->C+D that is consistent with the rate law rate=k(A)(B). Make sure you label which step is the rate determining step and prove that your proposed mechanism gives both the overall reaction and overall rate law. Explain the assumptions you must make in order for your mechanism to be consistent with the actual rate law.

Consider the following proposed reaction mechanism: (1) CIO (aq) + H,O(1)= HCIO(aq) + OH (aq) [fast] (2)I (aq) + HCIO(aq) → HIO(aq) + Cl¯(aq) [slow] (3) OH (aq) + HIO(aq) → H,O() + 10 (aq) [fast] Ignoring water, how many reaction intermediates are present? O 3 O 1 O 2

A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow

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 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}

Consider the following mechanism for the formation of nitrogen dioxide: 2 NO(g) N2O2(g) (1) N,O2(9) + O2(9) → 2 NO2(g) (2) Write the chemical equation of the overall reaction: yes 0,0,.. Are there any intermediates in this mechanism? no ? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one.