Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
![**Chemical Reaction Mechanism Analysis**
**Reaction:**
\[ 2 \text{H}_2\text{O}_2(aq) \longrightarrow 2 \text{H}_2\text{O}(l) + \text{O}_2(g) \]
**Proposed Mechanism in the presence of \(\text{I}^-(aq)\):**
**Step 1 (Slow):**
\[ \text{H}_2\text{O}_2(aq) + \text{I}^-(aq) \longrightarrow \text{H}_2\text{O}(l) + \text{OI}^-(aq) \]
**Step 2 (Fast):**
\[ \text{H}_2\text{O}_2(aq) + \text{OI}^-(aq) \longrightarrow \text{H}_2\text{O}(l) + \text{O}_2(g) + \text{I}^-(aq) \]
**Question:**
Which of the following species is a catalyst?
**Options:**
- A. \(\text{H}_2\text{O}\)
- B. This mechanism has no catalysts.
- C. \(\text{H}_2\text{O}_2\)
- D. \(\text{I}^-\)
- E. \(\text{OI}^-\)
**Explanation:**
In this chemical mechanism, the catalyst is the species that is present at the beginning and is regenerated at the end of the reaction.
To determine the catalyst:
- \(\text{I}^-\) appears in the initial step and is regenerated in the final step.
- \(\text{OI}^-\) is produced in the first step and consumed in the second step, so it is not a catalyst.
Therefore, the correct answer is:
- **D. \(\text{I}^-\)**
Catalysts are essential in chemical reactions as they increase the reaction rate without being consumed in the overall process. This particular example illustrates the role of \(\text{I}^-\) as a catalyst in the decomposition of \(\text{H}_2\text{O}_2\).](https://content.bartleby.com/qna-images/question/6e1a523d-017a-4e32-b964-043b2d7d2f50/560c7e12-3f70-4d7a-b0da-b45e86a9ec7b/yhbybg8.png)
Transcribed Image Text:**Chemical Reaction Mechanism Analysis**
**Reaction:**
\[ 2 \text{H}_2\text{O}_2(aq) \longrightarrow 2 \text{H}_2\text{O}(l) + \text{O}_2(g) \]
**Proposed Mechanism in the presence of \(\text{I}^-(aq)\):**
**Step 1 (Slow):**
\[ \text{H}_2\text{O}_2(aq) + \text{I}^-(aq) \longrightarrow \text{H}_2\text{O}(l) + \text{OI}^-(aq) \]
**Step 2 (Fast):**
\[ \text{H}_2\text{O}_2(aq) + \text{OI}^-(aq) \longrightarrow \text{H}_2\text{O}(l) + \text{O}_2(g) + \text{I}^-(aq) \]
**Question:**
Which of the following species is a catalyst?
**Options:**
- A. \(\text{H}_2\text{O}\)
- B. This mechanism has no catalysts.
- C. \(\text{H}_2\text{O}_2\)
- D. \(\text{I}^-\)
- E. \(\text{OI}^-\)
**Explanation:**
In this chemical mechanism, the catalyst is the species that is present at the beginning and is regenerated at the end of the reaction.
To determine the catalyst:
- \(\text{I}^-\) appears in the initial step and is regenerated in the final step.
- \(\text{OI}^-\) is produced in the first step and consumed in the second step, so it is not a catalyst.
Therefore, the correct answer is:
- **D. \(\text{I}^-\)**
Catalysts are essential in chemical reactions as they increase the reaction rate without being consumed in the overall process. This particular example illustrates the role of \(\text{I}^-\) as a catalyst in the decomposition of \(\text{H}_2\text{O}_2\).
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The reaction 5 CI (aq) + CIO3(aq) + 6 H*(aq) → 3 Cl₂(g) + 3 H₂O(l) is expected to obey the following mechanism: CIO3(aq) + H+ (aq): HCIO3(aq) HCIO3(aq) + H+ (aq): H₂CIO3(aq) CIT(aq) + H₂CIO3+ (aq) ₁ (CI-CIO₂)(aq) + H₂O(1) (CI-CIO₂) (aq) + 4 H*(aq) + 4 Cl(aq) - →→→→products What is the rate law for this reaction? 1. rate = k [CI]2 [CIO3]² [H+]² 2. rate = k [CI] [CIO31² [H+]² 3. rate = k [CI]2 [CIO3¹]² [H*] 4. rate = k [CI] [CIO3] [H+]² 5. rate = k [CI]2 [CIO3] [H*] O 4. rate = k [CI-] [CIO3-] [H+]2 O 2. rate = k [CI-] [CIO3-12 [H+]2 O 1. ratek [CI-]2 [CIO3-12 [H+]2 O 5. rate = k [CI-]2 [CIO3-] [H+] O 3. rate = k [CI-12 [CIO3-]2 [H+] wwwwwww Fast equilibrium Fast equilibrium Slow Fastarrow_forwardThe proposed 3-step mechanism for a reaction is Step 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k.1 = reverse rate constant.) %3D Step 2) A(g) + Z(g) Step 3) B(g) B(g) slow (k2 = rate constant) P(g) fast (k3 = rate constant) > a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] Initial [Y] Initial [Z] Initial Rate (M) (M) (M) (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants, products,…arrow_forwardPlease show full work!arrow_forward
- A medication has a first order elimination rate constant of 0.344 h-1. What is its half life?arrow_forwardDetermine the rate law and rate constant for the following reaction. Don't forget the units. Some of the numbers are blurry. (The concentrations for H* are x 10-5 and the rates are x 10-7 with the last value being x10-8) 10, (aq) + 81(aq) + 6 H(aq) → 31 (aq) + 2 H₂O(aq) Trial [103] Initial Rate (M/s) 1 0.0050 2.70 x 10 2 0.0100 5.40 x 10 3 0.0050 6.07 x 10 4 0.0050 6.75 x 10 [I]. 0.030 0.030 0.045 0.030 [H*]. 2.0 x 10 2.0 x 10 2.0 x 10 1.0 x 10arrow_forwardI am taking an online chem class and it’s harder than I thought. I have the answers to my whole study guide but I want to understand the WHY of the answers. Thank you!arrow_forward
- Under dissolving indium chloride (InCℓ) in hydrochloric acid (HCℓ), In+ (aq) undergoes disproportionation reaction according to the following unbalanced equation. In+ (aq) = In (s) + In3+ (aq) This disproportionation follows a first – order kinetics with a half-life of 667 s.(a) What is the concentration of In+(aq) after 1.25 hours if the initial solution of In+ (aq) was prepared by dissolving 2.38 g InCℓ (s) in 5.00 x 102 mL of dilute hydrochloric acid?(b) What mass of In (s) is formed after 1.25 hours? (c) Determine the rate constant k, for this reaction. (d) Sketch a graph of [In+] versus time (sec) over a period of 3 hours.arrow_forward13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium (H+) was studied. The table below summarizes the initial rates in four separate reactions where different initial concentrations of the reactants were used. What is the rate law for this reaction? (5 points) Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O ->>> [Cr₂0]/M [C2H5OH]/M [H+]/M (rate), /Ms-1 0.273 0.404 0.375 3.26 0.819 0.404 0.375 9.77 0.273 0.808 0.375 13.0 0.273 0.404 0.750 6.52 a) rate = = k[C₂H5OH][Cr2O7²¯][H+] b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+] c) rate = k[C₂H5OH][Cr₂07²-]² [H+] d) rate = k[C₂H5OH]² [Cr₂O,²-] e) rate = = k [Cr₂07²¯]² [H+]²arrow_forwardGiven below is a possible three-step mechanism describing the reaction of hydrogen peroxide with iodide ion in an acidic solution. Step 1: (slow) H2O2(aq) + I-(aq) ---> OH-(aq) + HOI(aq) Step 2: (very fast) OH-(aq) + H+(aq) ---> H2O(liq) Step 3: (fast) HOI(aq) + H+(aq) + I-(aq) ---> I2(aq) + H2O(liq) Assuming that the above reaction mechanism is correct, write the expected rate law expression. Is your experimental data consistent with the proposed mechanism? Explain your answer.arrow_forward
- 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 I (aq) + 1+ (aq) → 12 (aq) fast steparrow_forwardHNO3 + H₂C(OH)2 → HNO₂ + HCOOH + H₂O has a rate law: rate = k [H₂C(OH)₂] [HNO₂] -1 -3 Given a rate constant of 0.0664 dm³ mol¯¹ s¯¹ and initial concentrations [HNO3]0= 6.0 mol dm¯³, [H₂C(OH)₂]0= 166 mmol dm¯ , [HNO₂]0= 6.1 mmol dm³, how long will it take for the methanediol concentration to fall to 37 mmol dm-³?arrow_forward2. The proposed reaction mechanism is as follows: BrO₂ (aq) + H* (aq) → HBrO3 (aq) HBrO3 (aq) + H+ (aq) → H₂BrO₂+ (aq) H₂BrO3+ (aq) + Br (aq) → Br₂O₂ (aq) + H₂O (l) Br₂O₂ (aq) + 4H*(aq) + 4Br(aq) → 3Br₂ (l) + H₂O (l) Evaluate the validity of this proposed reaction. Justify your answer. i. ii. iii. iv. [Fast] [Medium] [Slow] [Fast]arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY