A suggested mechanism for the decomposition of peroxide (H2O2) is H2O2(aq) -> 2OH(aq) H2O2(aq) + OH(aq) ->> H2O()+ HO2(g) HO2(g) + OH(aq))→ H2O() + O2(g) Based on the mechanism which statement is true? O (1) The rate law is rate = k[H202] (2) the molecularity of the slow reaction is 4 (4) OH2 is an intermediate (3) OH is a catalyst A Moving to the next question prevents changes to this answer. fast slow fast

Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast) Cl2(g) = 2 CI(g) (2 - slow) CI(g) + CHCI3(g) HCI(g) + CCI3(g) --> (3 - fast) CI(g) + CCI3(g) --> A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect? %3D (Choose the best answer.) The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3). Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove reaction equation may be in the reaction rate law.

Consider the following mechanism for the formation of tert-butanol: 3 (CH3) CBr(aq) → (CH₂)₂C²(aq) + Br(aq) 3 (CH₂)₂C² (aq) + OH¯(aq) → (CH3) COH(aq) 3 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 0 yes no (1) (2) 0-0 00 0,0.... X 'a S

The 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.

The formation of tert-butanol is described by the following chemical equation: (CH3)₂CBr (aq) + OH(aq) → Br¨¯ (aq) + (CH3)₂COH(aq) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: (CH³)¸CBr (aq) → (CH3)¸₂C² (aq) +Br¯(aq) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 0 ロ→ロ Ś

??

Choose which mechanism(s) – just state the mechanism(s) that are most likely HO. OH OH2 "OH Br OH2 "OH Br

Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 CH33CBr (aq)  →   CH33C+ (aq)  +   Br− (aq) k1 2 CH33C+ (aq)  +   OH− (aq)  →   CH33COH (aq) k2 Suppose also  k1 ≫ k2 . That is, the first step is much faster than the second.

The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reactionNO (g) + Cl2 (g) ⇄ NOCl2 (g)NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)(2b) What is the reaction intermediate in this mechanism?

The decomposition of nitramide in aqueous solution at 25 °c NH2NO2(aq)N½O(g) + H20(1) is first order in NH2NO2. During one experiment it was found that when the initial concentration of NH2NO2 was 0.402 M, the concentration of NH2NO2 dropped to 7.40x10-2 M after 25187 s had passed. Based on this experiment, the rate constant for the reaction is s-1.