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2. (5 pts) Calculate the Ecell of the following galvanic battery configuration. Als e flow e...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
Part A through H 1. [60 pts) A galvanic cell is a type of battery where...
Part A through H
1. [60 pts) A galvanic cell is a type of battery where the electrodes are immersed in different electrolyte solutions, which are connected by an ion-conducting bridge. Consider a galvanic cell with Al and Cu electrodes. The Al electrode is immersed in a solution containing a standard concentration of Al3+ ions and the Cu electrode is immersed in a solution containing a standard concentration of Cu* ions. External Circuit The standard reduction potentials for the half...
4. Consider a Galvanic cell constructed from the following half cells, linked by an external circuit...
4. Consider a Galvanic cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. - an Al(s) electrode in 1.0 M AI(NO3)3 solution - a Pb(s) electrode in 1.0 M Pb(NO3)2 solution The balanced overall (net) cell reaction is 5. Calculate the value of Eºcell for the following reaction: 2Au(s) + 3 Ca2+(aq) → AU3+ (aq) + 3 Ca(s) 6. Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br (aq)...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode B) Cathode C) Salt Bridge D) Show the direction of electron flow through the wire Equations and Constants: AG --FE E-Eº - (RT/nF)InQ R-8.3145 J/mol K F-96485 J/V mole (7 pts) 3) For the galvanic cell represented by Zn(s)Zn²+ (aq)|| Ag (aq)| Ag(s) Voltmeter A) Write the anode half reaction Zn(s) JAg(s) B) Write the cathode half reaction C) Write the net reduction-oxidation reaction...
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell°...
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell° for this galvanic cell? If a more complete description of the cell is Ag(s)│Ag(NO3)(aq, 0.50 M)││KMnO4(aq, 0.50 M), HCl(aq, 2.5 M), Mn(Cl)2(aq, 0.01 M)│Pt(s), Ag(s) what is Ecell? What is the balanced, spontaneous cell reaction for the cell conditions given in b.?
What is the standard emf of a galvanic cell made of a Co electrode in a 1.0 M Co(NO32 solution and a Al electrode in a 1.0 M AI(NO3)3 solution at 25°C?
What is the standard emf of a galvanic cell made of a Co electrode in a 1.0 M Co(NO32 solution and a Al electrode in a 1.0 M AI(NO3)3 solution at 25°C? 0 cell Standard Reduction Potentials at 25°C Half-Reaction E(V +2.87 +2.07 +1.82 O,(g) 2H (aq)2e0(g)+HO Co3+(aq) + e-_? Co2+(aq) H,02(aq) + 2H"(aq) + 2e-_ 2H20 Cu2+(aq) + 2e-? Cu(s) AgCIs) + Ag(s) + CI(a) S02-(aq) + 4H'(aq) + 2e S02(g) + 2H20 Cu2+(aq) + e-_ Cu+(aq) Sn (aq)...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) +...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
Sketch the galvanic cell based on a half-cell containing 0.1 M Cu(NO3)2 with a Cu(s) electrode...
Sketch the galvanic cell based on a half-cell containing 0.1 M Cu(NO3)2 with a Cu(s) electrode and a half-cell containing 0.001 M Fe(NO3)2 with an Fe(s) electrode. Show the direction of electron flow and identify the cathode and the anode. Calculate Ecell and ∆G at 25 ◦C.
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M...
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
Part A through H
1. [60 pts) A galvanic cell is a type of battery where the electrodes are immersed in different electrolyte solutions, which are connected by an ion-conducting bridge. Consider a galvanic cell with Al and Cu electrodes. The Al electrode is immersed in a solution containing a standard concentration of Al3+ ions and the Cu electrode is immersed in a solution containing a standard concentration of Cu* ions. External Circuit The standard reduction potentials for the half...
4. Consider a Galvanic cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. - an Al(s) electrode in 1.0 M AI(NO3)3 solution - a Pb(s) electrode in 1.0 M Pb(NO3)2 solution The balanced overall (net) cell reaction is 5. Calculate the value of Eºcell for the following reaction: 2Au(s) + 3 Ca2+(aq) → AU3+ (aq) + 3 Ca(s) 6. Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br (aq)...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode B) Cathode C) Salt Bridge D) Show the direction of electron flow through the wire Equations and Constants: AG --FE E-Eº - (RT/nF)InQ R-8.3145 J/mol K F-96485 J/V mole (7 pts) 3) For the galvanic cell represented by Zn(s)Zn²+ (aq)|| Ag (aq)| Ag(s) Voltmeter A) Write the anode half reaction Zn(s) JAg(s) B) Write the cathode half reaction C) Write the net reduction-oxidation reaction...
What is the standard emf of a galvanic cell made of a Co electrode in a 1.0 M Co(NO32 solution and a Al electrode in a 1.0 M AI(NO3)3 solution at 25°C? 0 cell Standard Reduction Potentials at 25°C Half-Reaction E(V +2.87 +2.07 +1.82 O,(g) 2H (aq)2e0(g)+HO Co3+(aq) + e-_? Co2+(aq) H,02(aq) + 2H"(aq) + 2e-_ 2H20 Cu2+(aq) + 2e-? Cu(s) AgCIs) + Ag(s) + CI(a) S02-(aq) + 4H'(aq) + 2e S02(g) + 2H20 Cu2+(aq) + e-_ Cu+(aq) Sn (aq)...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
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