Given the half-reactions and their respective standard reduction potentials1.Cu³+ + 2 e-+ Cu+E; = +1.28 VCu²+ + eE; = +0.15 VE; == +0.52 V2.+ Cu+3.Cu²+ + 2 e-→ Cu(s)= +0.34 V4.Cu* + e-Cu(s)Ecalculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II).Cu³+ + eCu2+E° =V

Answered: Image /qna-images/answer/abbda739-1d2b-4160-ae88-f8965d9fc79a.jpg

Given the half-reactions and their respective standard reduction potentials Cu³+ + 2 e- – Cu+ E; = +1.28 V E; = +0.15 V = +0.34 V 1. 2. Cu2+ + e – Cu* Cu²+ + 2e¯ E; = E; = 3. Cu(s) 4. Cu+ + e- Cu(s) +0.52 V calculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II). Cu³+ + e- Cu2+ E° =

Given the half-reactions and their respective standard reduction potentials Cu³+ + 2 e- – Cu+ E; = +1.28 V E; = +0.15 V = +0.34 V 1. 2. Cu2+ + e – Cu* Cu²+ + 2e¯ E; = E; = 3. Cu(s) 4. Cu+ + e- Cu(s) +0.52 V calculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II). Cu³+ + e- Cu2+ E° =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 61QAP

See similar textbooks

Similar questions

The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
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)?
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)?
The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard conditions. Write out the Nernst equation. What are nonstandard conditions? What do , n, and Q stand for in the Nernst equation? What does the Nernst equation reduce to when a redox reaction is at equilibrium? What are the signs of G and when K 1? When K 1? When K = 1? Explain the following statement: determines spontaneity, while determines the equilibrium position. Under what conditions can you use to predict spontaneity?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.00 M separated by a porous disk from a compartment with a copper metal electrode immersed in a solution of 10.00 M NH3 that also contains 2.4 103 M Cu(NH3)42+. The equilibrium between Cu2+ and NH3 is: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 and the two cell half-reactions are: Assuming Ag+ is reduced, what is the cell potential at 25C?