5.2 Design a system for electrolytically forming Ag/AgCl electrodes. Give the chemical reactions that occur at both electrodes. 5.2 Use Figure 5.2. Put two Ag electrodes in NaCl solution, drive with 1.5 V battery between them s shown in Figure P5.2. 1.5V Battery Energy Source Ag Cathode Chemical Reaction 2H+ + 2e => H₂T R (H+) + (Na+) + (Cl-) Electrolyte Also Explain how this process work ? what is Ag Anode Chemical Reaction Figure P5.2 System for electrolytically forming Ag/AgCl electrodes. the disadvatges of using silver only AgC] Ag (Ag+)+(e-) (Ag+)+(Cl-)→ AgCl electrode ?

5.2 Design a system for electrolytically forming Ag/AgCl electrodes. Give the chemical reactions that occur at both electrodes. 5.2 Use Figure 5.2. Put two Ag electrodes in NaCl solution, drive with 1.5 V battery between them s shown in Figure P5.2. 1.5V Battery Energy Source Ag Cathode Chemical Reaction 2H+ + 2e => H₂T R (H+) + (Na+) + (Cl-) Electrolyte Also Explain how this process work ? what is Ag Anode Chemical Reaction Figure P5.2 System for electrolytically forming Ag/AgCl electrodes. the disadvatges of using silver only AgC] Ag (Ag+)+(e-) (Ag+)+(Cl-)→ AgCl electrode ?

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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both questions go together... thanks! Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e- 2 Br-(aq) 1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l) 0.96 2 Hg2+(aq) + 2 e- Hg22+(aq) 0.920 Hg2+(aq) + 2 e- Hg(l) 0.855 Ag+(aq) + e- Ag(s) 0.799 Hg22+(aq) + 2 e- 2 Hg(l) 0.789 Fe3+(aq) + e- Fe2+(aq) 0.771 I2(s) + 2 e- 2 I-(aq) 0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq) 0.48 Cu2+(aq) + 2 e- Cu(s) 0.337 Cu2+(aq) + e- Cu+(aq) 0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq) 0.14 2 H+(aq) + 2 e- H2(g) 0.0000 Pb2+(aq) + 2 e- Pb(s) -0.126 Sn2+(aq) + 2 e- Sn(s) -0.14 Ni2+(aq) + 2 e- Ni(s) -0.25…
(9). Please don't write on a paper. I can't understand handwritten. Sketch a voltaic cell in which the cell reaction is:
Determine Eº for a galvanic (voltaic) cell if AG = -4.9 kJ/mol and n = 3. (F = 96,500 J/ (V.mol))
(Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction that occurs in an electrochemical cell at 25°C? Fe3+ (aq) + Cu* (aq) ---> Fe²+ (aq) + Cu2+ (aq) The reduction potentials for the two half-reactions involved are: Fe3+ + e- --> Fe2+ (E°RED) = 0.77 V Cu2+ + e- --> Cu* (E°RED) = 0.16 V %3D
2.5
C. d. b. e. f. 1. a. Consider the following reduction potential: Ag+ + le ----→ Ag E° = 0.34 V Zn+2 +2e ------- → Zn Eº= -0.76 V Balance the Redox reaction occurring in the cell What is the sum of the coefficients in the balanced equation and what is the number of electrons transferred? Identify the oxidizing agent in the reactions: Identify the specie/s found at the anode Determine the standard cell potential for the reaction Determine the value of the Gibbs free Energy for the reaction shal
The answer is circled.
4. Mg|Mg* (0.10 M)I |Zn²"(0.10 M)|Zn Reaction at anode: Reaction at cathode: Overall reaction: Standard E (using table) = (show calculation) The %difference =
Using a table of standard electrode potentials, decide which of the following statements is completely true. Multiple Choice cu2" can oxidize H2, and Fe can reduce Mn2". H* can oxidize Fe. and NI can reduce Br2. Ni2" can oxidize Cu?", and Fe2* can reduce H". Fe?" can oxidize H2, and Fe2“ can reduce Au3". Br2 can oxidize NI, and H2 can reduce Mn*.
Gg.183. I need all parts please ....
3. Consider the following galvanic cell: Fe(s) Cr(s) Salt bridge containing KNO3(aq) IM Fet IM Cr+ e. What happens to the mass of the Fe electrode as the redox reaction progresses? f. What happens the concentration of The Fe3+ ion as the reaction progresses? g. Which chamber will the nitrate ion flow into? (anode or cathode)
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