Homework Help is Here – Start Your Trial Now!
Science
Chemistry
1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced reduction half-reaction: 10€ + 2BrO3 + 12H+ → Br2 + 6H2O b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced oxidation half-reaction: 2Br → Br2 + 2e- c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) Balanced net ionic redox reaction: 6H* + BrO3 + 5Br→ 3Br2 + 3H2O d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of H+: HBr and CH3COOH) Balanced net molecular redox reaction: KBRO3 + CH3COOH + 5HBr→ 3Br2 + 3H2O + CH3COOK 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations. (Note that Br2 is generated in the redox equation and consumed in the final step, thus it is considered. to be a reaction intermediate and should not appear in the net equation - you will need to scale one or more of the equations before the equations are combined.) NOTE: Equations should be completed using either "line-angle" structures for any organic molecules. Do not use the molecular formulae.

1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced reduction half-reaction: 10€ + 2BrO3 + 12H+ → Br2 + 6H2O b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced oxidation half-reaction: 2Br → Br2 + 2e- c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) Balanced net ionic redox reaction: 6H* + BrO3 + 5Br→ 3Br2 + 3H2O d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of H+: HBr and CH3COOH) Balanced net molecular redox reaction: KBRO3 + CH3COOH + 5HBr→ 3Br2 + 3H2O + CH3COOK 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations. (Note that Br2 is generated in the redox equation and consumed in the final step, thus it is considered. to be a reaction intermediate and should not appear in the net equation - you will need to scale one or more of the equations before the equations are combined.) NOTE: Equations should be completed using either "line-angle" structures for any organic molecules. Do not use the molecular formulae.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.4ACP: The overall reaction for the production of Cu(OH)2 from Cu in oxygenated water can be broken into...
See similar textbooks
icon
Related questions
Question

In this experiment a reactive aromatic compound, acetanilide, will be brominated using molecular bromine (generated in situ from hydrobromic acid and potassium bromate) as the electrophilic reagent. 

Based on this information, please answer questions 2 and 3. 

1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced reduction half-reaction: 10€ + 2BrO3 + 12H+ → Br2 + 6H2O b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced oxidation half-reaction: 2Br → Br2 + 2e- c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) Balanced net ionic redox reaction: 6H* + BrO3 + 5Br→ 3Br2 + 3H2O d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of H+: HBr and CH3COOH) Balanced net molecular redox reaction: KBRO3 + CH3COOH + 5HBr→ 3Br2 + 3H2O + CH3COOK 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations. (Note that Br2 is generated in the redox equation and consumed in the final step, thus it is considered. to be a reaction intermediate and should not appear in the net equation - you will need to scale one or more of the equations before the equations are combined.) NOTE: Equations should be completed using either "line-angle" structures for any organic molecules. Do not use the molecular formulae.
Transcribed Image Text:1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced reduction half-reaction: 10€ + 2BrO3 + 12H+ → Br2 + 6H2O b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. Balanced oxidation half-reaction: 2Br → Br2 + 2e- c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) Balanced net ionic redox reaction: 6H* + BrO3 + 5Br→ 3Br2 + 3H2O d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of H+: HBr and CH3COOH) Balanced net molecular redox reaction: KBRO3 + CH3COOH + 5HBr→ 3Br2 + 3H2O + CH3COOK 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations. (Note that Br2 is generated in the redox equation and consumed in the final step, thus it is considered. to be a reaction intermediate and should not appear in the net equation - you will need to scale one or more of the equations before the equations are combined.) NOTE: Equations should be completed using either "line-angle" structures for any organic molecules. Do not use the molecular formulae.
Expert Solution
steps

Step by step

Solved in 1 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Similar questions
Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS