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: 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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The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
The Ostwald process for the commercial production of nitric acid involves the Following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(s)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) a. Which reaction in the Ostwald process are oxidation-reduction reactions? b. Identify each oxidizing agent and reducing agent.
Using Table 17.1, calculate E° for the reaction between (a) lead and silver nitrate ion to produce lead(II) nitrate. (b) oxygen and iron(II) ions to produce water and iron(III) ions. (c) sulfur and nitrogen oxide gas in basic solution to form nitrate and sulfide ions.
Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.
. In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a.2Br2O3(s)+6Cl2(g)4BCl3(l)+3O2(g)b.GeH4(g)+O2(g)Ge(s)+2H2O(g)c.C2H4(g)+Cl2(g)C2H4Cl2(l)d.O2(g)+2F2(g)2OF2(g)
Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?
Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen. 4 Au(s) + 8 NaCN(aq) + O2(g) + 2 H2O() 4 NaAu(CN)2(aq) + 4 NaOH(aq) (a) Name the oxidizing and reducing agents in this reaction. What has been oxidized, and what has been reduced? (b) If you have exactly one metric ton (1 metric ton = 1000 kg) of gold-bearing rock, what volume of 0.075 M NaCN, in liters, do you need to extract the gold if the rock is 0.019% gold?
The Toliens test for the presence of reducing sugars (say, in a urine sample) involves treating the sample with silver ions in aqueous ammonia. The result is the formation of a silver mirror within the reaction vessel if a reducing sugar is present. Using glucose, C6H12O6, to illustrate this test, the oxidation-reduction reaction occurring is C6H12O6 (aq) + 2 Ag+(aq) + 2OH(aq) C6H12O7(aq) + 2 Ag(s) + H2O() What has been oxidized, and what has been reduced? What is the oxidizing agent, and what is the reducing agent? Tolien's test. The reaction of silver ions with a sugar such as glucose produces metallic silver. (a) The set-up for the reaction. (b) The silvered test tube
Determine the oxidation number of each element in each of the following compounds: (a) HCN (b) OF2 (c) ASCl3

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