7. Which of the following mechanisms is compatible with the rate law obtained in this experiment? Give an explanation for your choice. a) 2 1- (aq) + S₂082 (aq) → 12(aq) + 2 SO42- (aq) one-step reaction b) I- (aq) + S₂082-(aq) → 1+ (aq) + 2 SO42 (aq) slow step (aq) + 1+ (aq) → 12 (aq) fast step

7. Which of the following mechanisms is compatible with the rate law obtained in this experiment? Give an explanation for your choice. a) 2 1- (aq) + S₂082 (aq) → 12(aq) + 2 SO42- (aq) one-step reaction b) I- (aq) + S₂082-(aq) → 1+ (aq) + 2 SO42 (aq) slow step (aq) + 1+ (aq) → 12 (aq) fast step

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.89E: Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation,...

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List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
The reaction described by the following equation: 21-(aq) + H;O2(aq) + 2H*(aq) → I:(aq) + 2H;O(aq) has an experimental rate law (v) = k[I][H2O2]. Suggest a plausible mechanism for this reaction, and identify the rate-determining step.
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The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.
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
The equation for the iodination of acetone in acidic solution isCH3 COCH3(aq) + I2(aq) → CH3 COCH2(aq) + H+(aq) + I- (aq) The rate of the reaction is found to be dependent not only on the concentration of the reactants but also on the hydrogen ion centration. Hence the rate expression of this reaction is: rate = k [CH3COCH3]m [I2 ]n [H+]p The rate is obtained by the following the disappearance of iodine using starch as an indicator. The following data are obtained: [CH3COCH3] [H+] [I2] Initial Rate (mol/L.s) 0.80 0.20 0.001 4.2 x 10-6 1.6 0.20 0.001 8.2 x 10-6 0.80 0.40 0.001 8.7 x 10-6 0.80 0.20 0.0005 4.3 x 10-6 1. What is the order of the reaction with respect to each reactant? 2. Write the rate expression for the reaction.3. Calculate, K4. What is the rate of the reaction when [H+]= 0.933 M and [CH3COCH3]= 3[H+]= 10[I-] ?
Write the net ionic equation and rate law for the equation? 6Hl(aq) + 6Na₂S₂O3(aq) + KBrO3(aq) →6Nal(aq) + 3Na₂S4O6(aq) + KBr(aq) + 3H₂O(l)
1-Bromobutane reacts with water to form 1-butanol according to the following equation. C4H,Br(aq) + 2 H20(1) → C¿H,OH(aq) + H30*(aq) + Br¯(aq) The following is a proposed mechanism for the reaction. C4H9B1(aq) → C4H,*(aq) + Br¯(aq) C4H,*(aq) + H,0(1) → C4H3OH,*(aq) C,H,OH,*(aq) + H,0() – CH,OH(aq) + H30*(aq) slow fast fast Determine the overall rate law for this proposed mechanism. (Rate expressions take the general form: rate = k. [A]ª . [B]°.) chemPad Help Greek - Rate=k[C4H9B1][H2o²] Rate=k[C_4H_9Br][H_2O^2] Remember that answers are case-sensitive. Your answer contains an incorrect or incomplete chemical formula.
The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in the presence of I (aq) is proposed to be: Step 1: Н202(аq) + Г(аq) > H20() + ОГ(аq) slow Step 2: H2O2(aq) + OI (aq) → H20(1) + O2(g) +I (aq) fast Which of the following species is an intermediate? A. This mechanism has no intermediates. B. H20 O C. H202 O D- O E. O
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