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

2BrO3- + 12 H+ + 10e- --> Br2 + 6H2O , is an oxidation -reduction (redox) reaction. In which…

Answered: 1. The formation of molecular bromine…

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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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)
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The question is in the image, thanks a lot, have a really good day !!
For each reaction, indicate which elements are oxidized and which are reduced. a. WO2 + 3H2 → W + 3H20 Oxidized: Reduced: b. 2Na + Cl2 → 2NACI Oxidized: Reduced: C. 2 Fe2O3 + 3C 4Fe + 3CO2 Oxidized: Reduced:

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