SIMULATION Voltaic Cells Under Standard ConditionsOxidizingReducingElectrodeE° cathodeEOanode = EºcellAgentAgentPotential (V)Au3+(aq) + 3 eAu(s)+1.50Br2(t) + 2 e2 Br (aq)+1.08CathodeAnodeHg2 (aq) + 2 eHg(t)+0.855Ag (aq) + eAg(s)+0.80Hg2 (aq) + 2 e2 Hg(t)+0,789Cu2*(aq) + 2 eCu(s)+0.337Sn1+(aq) + 2 eSn²*(s)+0.152 H30 (aq) + 2 e H2(g) + 2 H20(s)0.00Sn2"(aq) + 2 eSn(s)-0.14Ni2*(aq) + 2 eNi(s)-0.25Cd2+(ag) + 2 eCd(s)-0.40Al3+(aq) + 3 eAl(s)-1.66Mg2 (aq) + 2 eMg(s)-2.37Li"(aq) + eLi(s)-3.045Click on an Oxidizing Aget and a Reducing Agent.Choose Au3+ as the oxidizing agent and Ni as the reducing agent. What is the value of E° cell?VGibbsFreeEnergy

In this question, we want to determine the value of standard potential for cell between Au3+ and Ni.…

Oxidizing Reducing Electrode E°cathode EO anode = E°cell Agent Agent Potential (V) Au (aq) + 3 e Au(s) +1.50 Br2(t) + 2 e 2 Br (aq) +1.08 Cathode Anode Hg2+(aq) + 2 e Hg(t) +0.855 Ag (aq) + e Ag(s) +0.80 Hg22 (aq) + 2 e 2 Hg(t) +0.789 Cu2*(aq) + 2 e Cu(s) +0.337 Sn+(aq) + 2 e Sn2+(s) +0.15 2 H30 (aq) + 2 e H2(g) + 2 H20(s) 0.00 Sn2*(aq) + 2 e Sn(s) -0.14 Ni(s) -0.25 Ni2* (aq) + 2 e Cd2+(ag) + 2 e Cd(s) -0.40 Al3*(aq) + 3 e Al(s) -1.66 Mg2 (aq) + 2 e Mg(s) -2.37 Li (aq) + e Li(s) -3.045 Click on an Oxidizing Ageat and a Reducing Agent. Choose Aut as the oxidizing agent and Ni as the reducing agent. What is the value of E°cell? V. 1 1 1 Gibbs Free Energy

Oxidizing Reducing Electrode E°cathode EO anode = E°cell Agent Agent Potential (V) Au (aq) + 3 e Au(s) +1.50 Br2(t) + 2 e 2 Br (aq) +1.08 Cathode Anode Hg2+(aq) + 2 e Hg(t) +0.855 Ag (aq) + e Ag(s) +0.80 Hg22 (aq) + 2 e 2 Hg(t) +0.789 Cu2(aq) + 2 e Cu(s) +0.337 Sn+(aq) + 2 e Sn2+(s) +0.15 2 H30 (aq) + 2 e H2(g) + 2 H20(s) 0.00 Sn2(aq) + 2 e Sn(s) -0.14 Ni(s) -0.25 Ni2* (aq) + 2 e Cd2+(ag) + 2 e Cd(s) -0.40 Al3*(aq) + 3 e Al(s) -1.66 Mg2 (aq) + 2 e Mg(s) -2.37 Li (aq) + e Li(s) -3.045 Click on an Oxidizing Ageat and a Reducing Agent. Choose Aut as the oxidizing agent and Ni as the reducing agent. What is the value of E°cell? V. 1 1 1 Gibbs Free Energy

Chemistry

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...

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Give the standard line notation for each cell. (a) 2 IO3(aq) + 10 Fe²+ (aq) + 10 H+ (aq) 10 Fe³+ (aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Fe³+ (aq), I₂ (aq) || Fe²+ (aq), IO3¯(aq), H+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), Fe³+ (aq) || IO3(aq), H+ (aq), I₂ (aq) | Pt(s) Pt(s) | IO3(aq), H+ (aq), I₂ (aq) || Fe²+ (aq), Fe³+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), IO3¯¯(aq), H+ (aq) || Fe³+ (aq), I₂ (aq) | Pt(s) (b) (c) (d) Zn(s) + 2 Ag+ (aq) = Zn²+ (aq) + 2 Ag(s) Ag(s) | Zn²+ (aq) || Ag+ (aq) | Zn(s) Zn(s) | Zn²+ (aq) || Ag+ (aq) | Ag(s) Ag(s) | Ag+ (aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag+ (aq) || Zn²+ (aq) | Ag(s) H₂O₂ (aq) + 2 H+ (aq) + 2e → 2 H₂O(l) O2(g) + 2 H+ (aq) + 2 e¯ → H₂O₂ (aq) Pt(s) | H₂O₂ (aq) | Pt(s) ○ Pt(s) | O₂(g) | H₂O₂ (aq), H+ (aq) || H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq), H+ (aq) || O₂(g) | H₂O₂ (aq), H+ (aq) | Pt(s) ○ Pt(s) | H₂O₂ (aq) | O₂(g) || H+ (aq) | Pt(s) Mn²+ (aq) + 2 e → Mn(s) Fe³+ (aq) + 3e → Fe(s) Fe(s) | Mn²+ (aq) || Fe³+ (aq) | Mn(s) Mn(s) | Mn²+ (aq) || Fe³+ (aq) | Fe(s)…
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Oxidizing Reducing Electrode Agent Agent Potential (V) Au³+ (aq) + 3 e Au(s) +1.50 Br₂(!) + 2 e 2 Br (aq) +1.08 Hg(t) +0.855 Hg²+ (aq) + 2 e Ag+ (aq) + e Hg₂²+ (aq) + 2 e Ag(s) +0.80 2 Hg(1) +0.789 Cu²+ (aq) + 2 e Cu(s) +0.337 Sn4+ (aq) + 2 e Sn²+(s) +0.15 2 H30+ (aq) + 2 e H₂(g) + 2 H₂O(s) 0.00 Sn²+ (aq) + 2 e Sn(s) -0.14 Ni²+ (aq) + 2 e Ni(s) -0.25 Cd²+ (aq) + 2 e Cd(s) -0.40 Al³+ (aq) + 3 e Al(s) -1.66 Mg²+ (aq) + 2 e Mg(s) -2.37 Li+ (aq) + e Li(s) -3.045 Click on an Oxidizing Agent and a Reducing Agent. Choose Au³+ as the oxidizing agent and Ni as the reducing agent. What is the value of Eºcell? 0.70 X V → → → → ↑ Eº cathode Gibbs Free Energy Eº anode = Eºcell = Cathode Anode
Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
Fe (s) +3 Au (aq) ^ + Fe log ^ 3+ +3 Au (s) For the first part, identify the oxidation half-reaction , identify the reduction half- reaction, identify the oxidizing agent, and identify the reducing agent under standard conditions. Next, calculate the standard cell potential, E for the reaction . cell E^ red +1.69 V Half-reaction Au^ + (aq) + e^ - Au (s) Fe^ 3+ (aq) + 3 e^ - Fe (s) -0.040 V Now , calculate the non- standard cell potential , when [Au^ + ]=0.0015 M and the [Fe^ 3+ ]= 0.033 M. After finding the cell potential , calculate the Gibb's free energy , AG Finally, calculate the equilibrium constant , K. Express your answers in two significant digits . Show your work for partial credit . Under non -standard conditions , is this reaction spontaneous or nonspontaneous ? Are reactants or products favored at equilibrium under non -standard conditions ?
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