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1. The formation of molecular bromine (Br2) from HBr and KBгO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 b. C. under acidic conditions. Label the half reaction as either oxidation or reduction. 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. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) 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) 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.) a) Balanced reduction half-reaction:10e¯ + 2BrО¸¯ + 12H+ → Br₂ + 6H₂O b) Balanced oxidation half-reaction: 2Br¯ → Br₂ + 2e- c) Balanced net ionic redox reaction: 6H+ + BrO3¯ +5Br¯ →3Br₂ + 3H2O d) Balanced net molecular redox reaction: KBrO3 + CH3COOH + 5HBr → 3Br2 + 3H2O + CH3COOK

1. The formation of molecular bromine (Br2) from HBr and KBгO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 b. C. under acidic conditions. Label the half reaction as either oxidation or reduction. 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. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) 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) 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.) a) Balanced reduction half-reaction:10e¯ + 2BrО¸¯ + 12H+ → Br₂ + 6H₂O b) Balanced oxidation half-reaction: 2Br¯ → Br₂ + 2e- c) Balanced net ionic redox reaction: 6H+ + BrO3¯ +5Br¯ →3Br₂ + 3H2O d) Balanced net molecular redox reaction: KBrO3 + CH3COOH + 5HBr → 3Br2 + 3H2O + CH3COOK

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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answer question 2 & 3. NOTE: question 1 is already answered in the image provided below 

1. The formation of molecular bromine (Br2) from HBr and KBгO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 b. C. under acidic conditions. Label the half reaction as either oxidation or reduction. 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. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) 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) 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.)
Transcribed Image Text:1. The formation of molecular bromine (Br2) from HBr and KBгO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 b. C. under acidic conditions. Label the half reaction as either oxidation or reduction. 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. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) 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) 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.)
a) Balanced reduction half-reaction:10e¯ + 2BrО¸¯ + 12H+ → Br₂ + 6H₂O b) Balanced oxidation half-reaction: 2Br¯ → Br₂ + 2e- c) Balanced net ionic redox reaction: 6H+ + BrO3¯ +5Br¯ →3Br₂ + 3H2O d) Balanced net molecular redox reaction: KBrO3 + CH3COOH + 5HBr → 3Br2 + 3H2O + CH3COOK
Transcribed Image Text:a) Balanced reduction half-reaction:10e¯ + 2BrО¸¯ + 12H+ → Br₂ + 6H₂O b) Balanced oxidation half-reaction: 2Br¯ → Br₂ + 2e- c) Balanced net ionic redox reaction: 6H+ + BrO3¯ +5Br¯ →3Br₂ + 3H2O d) Balanced net molecular redox reaction: KBrO3 + CH3COOH + 5HBr → 3Br2 + 3H2O + CH3COOK
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