A certain half-reaction has a standard reduction potential E =-1.25 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell thatmust provide at least 0.80 V of electrical power. The cell will operate under standard conditions.Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell.h DataAg+ (aq) + e Ag (s)0.7996Is there a minimum standard reductionpotential that the half-reaction used atthe anode of this cell can have?yes, there is a minimum.Ered= v!!Al3+ (aq) + 3e-- Al (s)-1.676Au+ (aq) + e Au (s)1.692If so, check the "yes" box and calculatethe minimum. Round your answer to 2decimal places. If there is no lowerlimit, check the "no" box.Au3+ (aq) + 3e - Au (s)1.498O no minimumBa2+ (ag) + 2e - Ba (s)-2.912Brz (1) + 2e- 2Br (aq)1.066Ca2+ (ag) + 2e - Ca (s)-2.868Is there a maximum standard reductionpotential that the half-reaction used atthe anode of this cell can have?E= OvCl2 (g) + 2e - 2CI- (aq)Co2+ (aq) + 2e- - Co (s)O yes, there is a maximum.1.35827red-0.28If so, check the "yes" box and calculatethe maximum. Round your answer to 2decimal places. If there is no upperlimit, check the "no" box.Co3+ (aq) + e- Co2+ (aq)1.92O no maximumCr2+ (aq) + 2e→ Cr (s)Cr+ (aq) + 3e - Cr (s)Cr+ (aq) + e - Cr2+ (aq)-0.913-0.744-0.407Cro42- (aq) + 4H20 (1) + 3e -Cr(OH)3 (s) + 5OH (aq)-0.13By using the information in the ALEKSData tab, write a balanced equationdescribing a half reaction that could beused at the anode of this cell.Cu2+ (aq) + 2e - Cu (s)0.3419Cu2+ (ag) + e - Cut (ag)0.153Note: write the half reaction as it wouldactually occur at the anode.Cu* (ag) + e→ Cu (s)0.521F2 (g) + 2e 2F (aq)2.866Fe2+ (aq) + 2e Fe (s)-0.447ExplanationCheckFe3+ (aq) + e-- Fe2+ (aq)0.771Fe+ (aq) + 3e Fe (s)-0.037MacBook Air20esc000000 FA►►F12F8F9F10FIIF1F2F3F5F6F724%&* 2H (aq) + 2e H2 (g)0.0002H20 (1) + 2e → H2 (g) + 20H (aq)-0.8277H202 (aq) + 2H+ (aq) + 2e → 2H20 (1)1.776I2 (s) + 2e 21 (aq)0.53552103 (aq) + 12H+ (aq) + 10e I2 (s) + 6H20 (1)1.195Mg2+ (aq) + 2e Mg (s)-2.372Mn2+ (aq) + 2e Mn (s)-1.185MnO2 () + 4H+ (aq) + 2e-- Mn2+ (aq) + 2H20 (1)1.224MnO4 (aq) + 8H+ (aq) + 5e Mn2+ (aq) + 4H20 (1)1.507MnO4 (aq) + 2H20 (1) + 3e MnO2 (s) + 40H (aq)0.595HNO2 (aq) + H+ (aq) + e- NO (g) + H20 (1)0.983N2 (g) + 4H2O (1) + 4e- → 40H (aq) + N2H4 (aq)-1.16NO3 (aq) + 4H+ (aq) + 3e NO (g) + 2H20 (I)0.957Na+ (aq) + e Na (s)-2.71Ni2+ (ag) + 2e Ni (s)-0.2571.22902 (g) + 4H+ (aq) + 4e- → 2H20 (1)0.40102 (g) + 2H20 (1) + 4e¬ → 40H (aq)0.69502 (g) + 2H+ (aq) + 2e → H2O2 (aq)-0.1262Pb2+ (ag) + 2e → Pb (s)-0.3588PBSO4 (s) + H (aq) + 2e Pb (s) + HSO4 (aq)k Air4)F12F11IIF8F9F10F7%3Ddelete+ II

A certain half-reaction has a standard reduction potential E=-1.25 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that red must provide at least 0.80 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the cathode of the cell. dh Data Ag+ (aq) + e Ag (s) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? O yes, there is a minimum. Ov %3D red Al3+ (aq) + 3e-- Al (s) -1.676 Au+ (aq) + e- Au (s) 1.692 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Au3+ (aq) + 3e Au (s) 1.498 O no minimum Ba2+ (aq) + 2e- Ba (s) -2.912 Brz (1) + 2e - - 2Br (aq) 1.066 Ca2+ (aq) + 2e - Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? = Ov Cl2 (9) + 2e → 2CI- (aq) O yes, there is a maximum. E red 1.35827 %3! Co2+ (aq) + 2e - Co (s) Co3+ (aq) + e Co2+ (aq) Cr2+ (aq) + 2e→ Cr (s) Cr3+ (aq) + 3e Cr (s) Cr+ (aq) + e Cr2+ (aq) Cro42- (aq) + 4H20 (1) + 3e - Cr(OH)3 (s) + 50H (aq) -0.28 If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. 1.92 O no maximum -0.913 -0.744 -0.407 -0.13 By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Cu2+ (aq) + 2e- Cu (s) 0.3419 Cu2+ (ag) + e - Cu* (aq) 0.153 Note: write the half reaction as it would actually occur at the anode. Cu* (ag) + e - Cu (s) 0.521 F2 (9) + 2e 2F (aq) 2.866 Fe2+ (ag) + 2e- Fe (s) -0.447 Explanation Check Fe3+ (aq) + e - Fe2+ (aq) 0.771 1. Fe+ (aq) + 3e Fe (s) -0.037 MacBook Air 20 FI F12 D00 F4 F10 FS F6 F7 F8 F9 FI F2 F3

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...