8 8) Use the standard half-cell potentials listed below to calculate the standard cell potential for thefollowing reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)Pb(s) + Br2(1) – Pb2+(aq)+ 2 Br´(aq)Pb2+(aq) + 2 e¯ - Pb(s)Br2(1) + 2 e -2 Br(aq)E° = -0.13 VE° = +1.07 VA) -0.94 VB) +1.20 VC) -0.60 VD) +0.94 VE) -1.20 Veaboga ierlW (Iat the dawn of( (a()1(Alo irsinoo nori arT (Sbas ()nori of (I)nori srityd baninnsisanoitonor-llerl owt orh yidnoblI noitsbixo (AUnderstandingnoibson-lisd noitebixo (8()E (n)+)nothssn-tierl noitabixo (Onoitbson-liarl noitebio (aai terW (ISBN 1-4116-733po noibrn-llad no bns noitoes2o oitocar-llsrd noiabixoobonr arlssnolbubon (8bas noibn-id ooubo (O9 "781411 67336

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8) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Pb(s) + Br2(1) – Pb2+(aq) +2 Br°(aq) Pb2+(aq) + 2 e" - Pb(s) Br2(1) + 2 e -2 Br(aq) E° = -0.13 V E° = +1.07 V A) -0.94 V B) +1.20 V C) -0.60 V D) +0.94 V E) -1.20 V Ui

8) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Pb(s) + Br2(1) – Pb2+(aq) +2 Br°(aq) Pb2+(aq) + 2 e" - Pb(s) Br2(1) + 2 e -2 Br(aq) E° = -0.13 V E° = +1.07 V A) -0.94 V B) +1.20 V C) -0.60 V D) +0.94 V E) -1.20 V Ui

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 92QRT

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