Please explain how to fill in table given provided information thanks CELL POTENTIALElectrode system usedin cellZn (s) | Zn²+ (aq) || Cu²+(aq) | Cu (s)Zn (s) | Zn²+ (aq) || Fe³+(aq) | Fe²+ (s) | graphiteCu (s) | Cu²+ (aq) || Ag+(aq) | Ag (s)Zn (s) | Zn²+ (aq) || Ag+(aq) | Ag (s)Zn (s) | Zn²+ (aq) || 12 (s) |1- (aq) | graphiteFe2+ (s) | Fe³+ (aq) || Br₂(1) | Br- (aq) | graphiteCI- (aq) | Cl₂ (g, 1 atm) || |Br2 (1) Br- (aq) | graphiteCellNegativePotential (V) Electrode0.825 Zn0.407 Zn0.413 Cu1.250 Zn1.025 Zn0.408 Fe0.103 CIOxidationReactionZn (s)->Zn²+ + 2eZn (s) ->Zn²+ + 2eCu (s) ->Cu²+ (aq) +2eZn (s)->Zn²+ + 2e->Zn (s)Zn²+ + 2eFe²+ (s)->Fe³+ + eCl- (aq) ->Cl₂ (g, 1 atm)Eº Reduction EºOxida Reactiontion(M)1.25Cu²+ (aq)+ 2e ->Cu (s)1.25 Fe³+ (aq)-> Fe²+(s)0.413 Ag+ (aq) +e -> Ag(s)1.25 Ag+ (aq) +e> Ag(s)1.25 12 (s) + e0.538-> 1- (aq)0.843 Br2 (1) + e-> Br-(aq)Br2 (1) –>Br- (aq) +eReduction(M)-0.425-0.8430.000.00-0.225-0.435-0.435 264 Experiment 32 Voltaic Cell MeasurementsA.2. Table of Electrode PotentialsIn Table A.1, you should have a value for Ed or Exid for each of the electrode systems you have studied.Remembering that for any electrode system, Ered =-E0Eoxid, you can find the value for Ered for each system. Listthose potentials in the left column of the table below, in order of decreasing (more negative) value.EreductionAg+,Ag= 0.00 V)Electrode reactionin reduction(Eº=EreductionH+,H₂= 0.00 V)The electrode potentials you have determined are based on setting Egt.Ag 0.00 V. The usual convention inelectrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions EAg+,Ag red= +0.80 V. Convert fromone base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enterthese values in the third column of the table.Why are the values of Ed on the two bases related to each other in such a simple way?

The standard cell potential is calculated using the standard reduction potential of the cathode and…

A.2. Table of Electrode Potentials In Table A.1, you should have a value for Eed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ed=-Exid, you can find the value for Ed for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. EO reduction (Eº Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº E reduction H.H₂ = 0.00 V) The electrode potentials you have determined are based on setting E = 0.00 V. The usual convention in Agt.Ag electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E "Ag, Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?

A.2. Table of Electrode Potentials In Table A.1, you should have a value for Eed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ed=-Exid, you can find the value for Ed for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. EO reduction (Eº Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº E reduction H.H₂ = 0.00 V) The electrode potentials you have determined are based on setting E = 0.00 V. The usual convention in Agt.Ag electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E "Ag, Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

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