(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Pb(s) Pb2+(aq) + 2e oxidation 2H+(aq) + 2e->H2(g) reduction (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. + + When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? Cr3++ ☐ Cr₂07² + Cu - Cr³* + Water appears in the balanced equation as a with a coefficient of (Enter 0 for neither.) Cu2+ How many electrons are transferred in this reaction? (reactant, product, neither)

(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Pb(s) Pb2+(aq) + 2e oxidation 2H+(aq) + 2e->H2(g) reduction (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. + + When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? Cr3++ ☐ Cr₂07² + Cu - Cr³* + Water appears in the balanced equation as a with a coefficient of (Enter 0 for neither.) Cu2+ How many electrons are transferred in this reaction? (reactant, product, neither)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 74AP: . To obtain useful electrical energy from an oxidation-reduction process, we must set up the...

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Similar questions

Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
A solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
Consider three metals, X, Y, and Z, and their salts, XA, YA, and ZA. Three experiments take place with the following results: • X+hotH2Obubbles • X+YAnoreaction • X+ZAXdiscolored+Z Rank metals X, Y, and Z, in order of decreasing strength as reducing agents.
Why is it not possible for hydroxide ion (OH-) to appear in either of the half-reactions or the overall equation when balancing oxidation—reduction reactions in acidic solution?
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
. To obtain useful electrical energy from an oxidation-reduction process, we must set up the reaction in such a way that the Oxidation half-reaction and the reduction half-reaction are physically one _____another.
If a 2.5 A current is run through a circuit for 35 minutes, how many coulombs of charge moved through the circuit?
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 following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25V
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.

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