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.
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.
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.
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.
Definition Definition Organic compounds with a planar cyclic ring of atoms bonded through alternated single and double bonds. Aromatic organic compounds, also called arenes, are an important class of hydrocarbons under the branch of organic chemistry.
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