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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(7.4) Describe in shorthand notation a galvanic cell for which the cell has the following reaction. Chose the BEST option by writing the CAPITAL LETTER of the best answer. Cu(s) + 2 Fe*3(aq) - Cu*?(aq) + 2 (be). Fe2 (aq) CHOICES: (A) Cu Cu*2||Fe*3|Fe*2 (B) Cu*2|Cu||Fe*3| Fe*2 (C) Cu|Cu*2||Fe*2 |Fe*3 (C) Cu*2|Cu||Fe*2| Fe*3 Answer:
(5). Please don't write on a paper. I can't understand handwritten. Sketch a voltaic cell in which the cell reaction is:
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:
A concentration cell running at 25°C consists of two Al(s)/Al3+(aq) cells. If the concentration of Al3+ at the anode is 4.12 x 10-8 M and the concentration of Al3+ at the cathode is 1.27 M, what is the value of Ecell? (Two decimal places)
B through D please. Thanks!
2. (5) 8 Question b6 of / Complete and balance the following half-reaction in acidic solution MnO,(aq) → Mno,(s) -> 3. 02+03+ 4- 4+ 3 4 7 9. 0. 1 03 4 6. (s) (1) (g) (aq) e H* OH H. Mn H,O* H.O Reset • x H,O Delete
(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
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 =
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19. The following unbalanced redox reaction occurs in basic aqueous solution. Upon balancing, the reaction has side of the reaction. H2O(1) included on the a. 3 H20(1), product side b. 6 H20(I), reactant side c. 4 H2O(1), reactant side NO; (aq) + Cr(OH)3(s) → CrO4²(aq) + NO2 (aq) d. 5 H20(1), product side e. 2 H20(1), reactant side