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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

SIMULATION Voltaic Cells Under Standard Conditions
Oxidizing
Reducing
Electrode
E° cathode
EO
anode = Eºcell
Agent
Agent
Potential (V)
Au3+(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
Hg2 (aq) + 2 e
2 Hg(t)
+0,789
Cu2*(aq) + 2 e
Cu(s)
+0.337
Sn1+(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
Ni2*(aq) + 2 e
Ni(s)
-0.25
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 Aget and a Reducing Agent.
Choose Au3+ as the oxidizing agent and Ni as the reducing agent. What is the value of E° cell?
V
Gibbs
Free
Energy

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Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.049 M at 25 °C. 2 Fe2*(aq) + H2O2(aq) + 2 H*(aq) → 2 Fe³*(aq) + 2 H2O(t) Acidic Solution Standard Electrode Potential, E(volts) H2O2(aq) + 2 H*(aq) + 2 e 2 H2O(t) +1.77 → Au(s) Aus (aq) + 3 e → Au(s) Br2(e) + 2 e –→ 2 Br(aq) NO: (aq) + 4 H*(aq) + 3 e" Au*(aq) + e - +1.68 > +1.50 +1.08 NO(g) + 2 H20 +0.96 Ag*(aq) + e → Ag(s) +0.80 Hg2 (aq) + 2 e Fe"(aq) + e- →2 Hg(t) Fe"(aq) > +0.789 > +0.77 Cu2*(aq) + 2 e Cu(s) +0.337 > Hg2Clz(s) + 2 e →2 Hg(t) + 2 Cr(aq) Sn**(aq) + 2e → 2 H*(aq) + 2 e Pb2"(aq) + 2 e +0.27 Sn2"(aq) +0.15 » H2(g) 0.00 -0.126 → Pb(s) Sn(s) Sn2*(aq) + 2 e Ni"(aq) + 2 e Cd2"(aq) + 2 e → Cd(s) Cr**(aq) + e -0.14 > Ni(s) -0.25 -0.40 » Cr**(aq) -0.408 Fe2"(aq) + 2 e Zn2*(aq) + 2 e → Cr2*( aq) + 2 e A* (aq) + 3 e - » Fe(s) -0.44 Zn(s) -0.763 → Cr(s) Al(s) > -0.91 > -1.66 Mg2"(aq) + 2 e - → Mg(s) -2.37 >
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