Given the following pair of half-reactions, fill in the line notation for a standard cell using...

Given the following pair of half-reactions, fill in the line notation for a standard cell using these two half-reactions. Since it is a standard cell, all concentrations will be 1 M, so do not enter concentrations. You have solid platinum (Pt) electrodes to use, where necessary. Do not include the physical state of the components, i.e., solid platinum would just be Pt. For subscript and superscripts use the model: Ag+ would be Ag^+ and SO42- would be entered as SO4^2-, with the "^" character indicating a superscript. Leave a space between components.

I3- (aq) + 2e- → 3 I- (aq) ξo = 0.55

Tl3+ (aq) + 2e- → Tl+ (aq) ξo = 1.24

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Write the Standard Cell Notation and Half Reactions of the following voltaic cell combinations. 1. Zinc...

Write the Standard Cell Notation and Half Reactions of the following voltaic cell combinations. 1. Zinc Nitrate (0.20 M) and Copper Nitrate (0.30 M); Copper – Anode, Zinc – Cathode 2. Lead Sulfate (0.25 M) and Zinc Sulfate (0.50 M); Lead – Cathode, Zinc – Anode 3. Copper Sulfate (0.65 M) and Lead Sulfate (0.20 M); Copper – Anode, Zinc – Cathode 4. Silver Nitrate (0.15 M) and Lead Nitrate (0.40 M); Silver – Anode, Lead – Cathode 5. Aluminum...

7. Given the standard reduction potential for the following two half-cell reactions (in the presence of...

7. Given the standard reduction potential for the following two half-cell reactions (in the presence of 1.00 M HCl): Fe3+ + e <==> Fe2+, E0 = + 0.68 V AsO4 - + 2H+ + 2e <==> AsO3 - + H2O, Eo = +0.559 V. Please calculate the system potential at the equivalence point when Fe3+ was used to titrate AsO3 - in the presence of 1.00 M HCl. Answer: 0.60 V

Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the...

Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the proper coefficient for each of the species involved in the overall reaction. Water molecules and protons are not shown in the half-reactions, but may be needed in the overall reaction. MnO4- (aq) ? MnO2 (s) ?o = 0.59 V NO3- (aq) ? NO (g) ?o = 0.96 V NO3- (aq) MnO4- (aq) NO (g) MnO2 (s) H+ (aq) H2O (l)

Write the balanced, net-ionic equations for the cell reactions for the following half-cell combinations at standard...

Write the balanced, net-ionic equations for the cell reactions for the following half-cell combinations at standard conditions. Be sure to consider direction of spontaneity. A. Cu/Cu2+, Zn/Zn2+ B. Ag/Ag+, Mg/Mg2+ C. Zn/Zn2+, Pb/Pb2+ D. Ni/Ni2+, Ag/Ag+ E. Cu/Cu2+, Mg/Mg2+

Consider a galvanic cell based on the following line notation at standard conditions and 298K: Sn...

Consider a galvanic cell based on the following line notation at standard conditions and 298K: Sn | Sn2+ || Fe3+ | Fe Which of the following changes WILL NOT change the potential of the cell? Add equal amounts of water to each half cell Replace the Fe electrode with a Pt electrode Increase the concentration of Sn2+ Decrease the concentration of Fe3+ Replace the Sn electrode with a Pt electrod

A concentration cell is built based on the following half reactions by using two pieces of...

A concentration cell is built based on the following half reactions by using two pieces of gold as electrodes, two Au3+ solutions, 0.101 M and 0.423 M, and all other materials needed for a galvanic cell. What will the potential of this cell be when the cathode concentration of Au3+ has changed by 0.035 M at 307 K? Au3+ + 3 e- → Au Eo = 1.50 V

A concentration cell is built based on the following half reactions by using two pieces of...

A concentration cell is built based on the following half reactions by using two pieces of copper as electrodes, two Cu2+ solutions, 0.145 M and 0.405 M, and all other materials needed for a galvanic cell. What will the potential of this cell be when the cathode concentration of Cu2+ has changed by 0.031 M at 279 K? Cu2+ + 2 e- → Cu Eo = 0.341 V

Calculate the cell potential for a reaction in a electrolytic cell with the following half-reactions if:...

Calculate the cell potential for a reaction in a electrolytic cell with the following half-reactions if: [U 3+] = 0.10 M, [MnO4 - ] = 0.20M, [Mn2+], and [H+ ] = 0.20 M U 3+ + 3e -> U o Ecell = - 1.642 V MnO4 - + 8H+ + 5e- -> Mn2+ + 4H2O Ecell = +1.51 V

Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair...

Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair of two half-reactions: a) H2= 2H+ + 2e- Fe2+= à Fe3+ + e- b) 1/4O2(g) + H++ e- == ½ H2OH2 =à 2H++ 2e- C) 2IO3-+ 12H++ 10e-== I2+ 6H2O 2I-= I2+ 2e-

Write the cell reaction and electrode half-reactions and calculate the standard potential of each of the...

Write the cell reaction and electrode half-reactions and calculate the standard potential of each of the following cells: a) Zn/ZnSO4(aq)//AgNO3(aq)/Ag b) Pt/K3[Fe(CN)6](aq), K4[Fe(CN)6](aq)//CrCl3 (aq)/Cr Please show all steps and clear writing. Thanks

Subjects