In the following reaction which occurs from left to right: 3 Cu2*(aq) + 2 Fe(s) → 2 Fe3*(aq) + 3 Cu(s) the Cu(s) is the oxidizing agent and Fe*(aq) is the reducing agent the Cu2*(aq) is the reducing agent and Fe(s) is the oxidizing agent the Cu2*(aq) is the oxidizing agent and Fe(s) is the reducing agent O the Fe(s) is the oxidizing agent and Cu²*(aq) is the reducing agent

In the following reaction which occurs from left to right: 3 Cu2(aq) + 2 Fe(s) → 2 Fe3(aq) + 3 Cu(s) the Cu(s) is the oxidizing agent and Fe(aq) is the reducing agent the Cu2(aq) is the reducing agent and Fe(s) is the oxidizing agent the Cu2(aq) is the oxidizing agent and Fe(s) is the reducing agent O the Fe(s) is the oxidizing agent and Cu²(aq) is the reducing agent

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 20RORR: The Ostwald process for the commercial production of nitric acid involves the Following three steps:...

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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.
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 blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium di-chromate solution, resulting in the production of Cr3+ (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr2O72) is orange in solution, and the Cr3+ ion is green. The balanced equations is 16H+(aq) + 2Cr2O72(aq) + C2H5OH(aq) 4Cr4+(aq) + 2CO2(g) + 11H2O(l) This reaction is an oxidationreduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?
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?
Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?
Xenon trioxide, XeO3, reacts with aqueous base to form the xenate anion, HXeO4. This ion reacts further with OH to form the perxenate anion, XeO64, in the following reaction: 2HXeO4(aq)+2OH(aq)XeO64(aq)+Xe(g)+O2(g)+2H2O(l) Identify the elements that are oxidized and reduced in this reaction. You will note that the equation is balanced with respect to the number of atoms on either side. Verify that the redox part of this equation is also balanced, that is, that the extents of oxidation and reduction are also equal.
The mass of a solid piece of iron Fe(s) should be determined by allowing it to react with a solution of 0.500 L potassium dichromate K2Cr2O7 (aq) in a redox reaction in acidic solution, so that all iron is oxidized into iron (II) ions, Fe2+(aq). Concomitant chromium(III) ions, Cr3+(aq), after the reduction equation: Cr2O7 2−(aq) + 14H +(aq) + 6e − → 2Cr3+(aq) + 7H2O(l) a) Write the complete and balanced reaction equation for the redox reaction where the piece of iron is oxidized into iron (II) ions by the dithromations in the solution. b) A sample of the reaction solution after the oxidation of iron is completed shows that the molar concentration of Cr3+ ions is 0.0162 M. What is the calculated mass of the piece of iron Fe(s) in grams? c) What is the amount of electrons e − in moles transmitted in this specific reaction? Calculate the electrical work wel the oxidation of the piece of iron has created in kilojoules (kJ), using the enclosed electrode potentials E 0 and the…
In the following chemical reaction, which element is the reducing agent? 3 Sn(NO₃)₂(aq) + 2 Fe(s) → 2 Fe(NO₃)₃(aq) + 3 Sn(s)
The quantity of antimony in a sample can be determined by an oxidation–reduction titration with an oxidizing agent. A 7.05 gsample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+(aq).The Sb3+(aq) is completely oxidized by 34.8 mL of a 0.115 M aqueous solution of KBrO3(aq).The unbalanced equation for the reaction is BrO−3(aq)+Sb3+(aq)⟶Br−(aq)+Sb5+(aq)(unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: g percentage of antimony: %
Balance the following redox reaction: CuS(s) + NO3` (aq) à Cu2+(aq) + S(s) + NO (g) (in acid)