givin the answer for 1 & 2 below, provide an answer for 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.) 1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redoxreactions.a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2under acidic conditions. Label the half reaction as either oxidation or reduction.10e + 2Br03 + 12H* → Br₂ + 6H₂O (Reduction)b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 underacidic conditions. Label the half reaction as either oxidation or reduction.2Br → Br₂ + 2e¯ (Oxidation)C.Write the balanced net (ionic) redox reaction (reduced to the lowest wholenumber coefficients)6H + BrO3 + 5Br¯ → 3Br2 + 3H20d. Rewrite the balanced net redox equation in complete (molecular) form usingKBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bitof manipulation as there are two sources of H+ HBr and CH3COOH)KBгO3 + CH3COOH + 5HBr → 3Br2 + 3H2O + CH3COOK2. Write the equation for the reaction of acetanilide with molecular bromine (for the organiccompounds, draw the full structures, not condensed formulae). уго-Zare tanilideBr. FebrzHВо4P-bromo acetanilide

The question aims to write the balanced equation by adding the given redox equation and the equation…

Answered: reactions. a. Write the balanced…

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Chapter1: Chemical Foundations

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Question

givin the answer for 1 & 2 below,

provide an answer for 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.)

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.
10e + 2Br03 + 12H* → Br₂ + 6H₂O (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.
2Br → Br₂ + 2e¯ (Oxidation)
C.
Write the balanced net (ionic) redox reaction (reduced to the lowest whole
number coefficients)
6H + BrO3 + 5Br¯ → 3Br2 + 3H20
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)
KBгO3 + 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).

уго
-Z
are tanilide
Br. Febrz
H
Во
4
P-bromo acetanilide

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