EQUATIONS 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 under acidic conditions. Label the half reaction as either oxidation or reduction. 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. c. 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 Ht: 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.)
EQUATIONS 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 under acidic conditions. Label the half reaction as either oxidation or reduction. 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. c. 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 Ht: 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.)
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter19: Redox Reactions
Section: Chapter Questions
Problem 89A
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Transcribed Image Text:EQUATIONS
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.
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.
c. 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 Ht: 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.)
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