Plz answer 1-6!! Thank you :) [Review Topics]2req[References]Use the References to access important values if needed for this question.2reqConsider the following half-reactions:2reqHalf-reactionE° (V)(s) +2e21°(aq)0.535VS 2reqCu*(aq) + 2eCu(s) 0.337VS 2reqFe*(aq) + 2eFe(s) -0.440V(1) The weakest oxidizing agent is:enter formulaM(2) The strongest reducing agent is:2reqs 2req(3) The strongest oxidizing agent is:Is 2reg(4) The weakest reducing agent is:(5) Will I'(aq) reduce Fe2"(aq) to Fe(s)?(6) Which species can be oxidized by Cu2"(aq)?If none, leave box blank.PreRetry Entire Group8 more group attempts remainingSubmit Answer

Answered: Image /qna-images/answer/d0685b26-24d6-40c9-a238-c3c042846e45.jpg

Half-reaction E° (V) 1(s) + 2e 21'(aq) 0.535V Cu*(aq) + 2e → Cu(s) 0.337V Fe (aq) + 2e Fe(s) -0.440V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will I'(aq) reduce Fe2"(aq) to Fe(s)? (6) Which species can be oxidized by Cu2"(aq)? If none, leave box blank.

Half-reaction E° (V) 1(s) + 2e 21'(aq) 0.535V Cu*(aq) + 2e → Cu(s) 0.337V Fe (aq) + 2e Fe(s) -0.440V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will I'(aq) reduce Fe2"(aq) to Fe(s)? (6) Which species can be oxidized by Cu2"(aq)? If none, leave box blank.

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 26QAP: For the following half-reactions, answer the questions below....

See similar textbooks

Similar questions

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.
Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is H+(aq) capable of oxidizing Cu(s) to Cu2+(aq)? b. Is Fe3+ (aq) capable of oxidizing I (aq)? c. Is H2(g) capable of reducing Ag+(aq)?
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, 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 PbC2O4(s)+2ePb(s)+C2O42(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/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
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)?
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
For the following half-reactions, answer these questions. Ce4+(aq)+eCe3+(aq)E=+1.61VAg+(aq)+eAg(s)E=+0.80VHg22+(aq)+2e2Hg(l)E=+0.80VSn2+(aq)+2eSn(s)E=0.14VNi2+(aq)+2eNi(s)E=0.24VAl3+(aq)+3eAl(s)E=1.68V (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg(l) reduce Sn2+(aq) to Sn(s)? (g) Which ion(s) can be reduced by Sn(s)? (h) Which metal(s) can be oxidized by Ag+(aq)?
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
For the following half-reactions, answer the questions below. Co3+(aq)+eCo2+(aq)E=+1.953VFe3+(aq)+eFe2+(aq)E=+0.769VI2(aq)+2e2I(aq)E=+0.534VPb2+(aq)+2ePb(s)E=0.127VCd2+(aq)+2eCd(s)E=0.402VMn2+(aq)+2eMn(s)E=1.182V (a) Which is the weakest reducing agent? (b) Which is the strongest reducing agent? (c) Which is the strongest oxidizing agent? (d) Which is the weakest oxidizing agent? (e) Will Pb(s) reduce Fe3+(aq) to Fe2+(aq)? (f) Will I-(aq) reduce Pb2+(aq) to Pb(s)? (g) Which ion(s) can be reduced by Pb(s)? (h) Which if any metal(s) can be oxidized by Fe3+(aq)?
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?
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?