A galvanic cell has the following reaction. Zn(s) + 2 Fe(aq) → 2 Fe(aq) + Zn(aq)...
A galvanic cell has the following reaction. Zn(s) + 2
Fe
(aq)
→ 2 Fe
(aq)
+ Zn
(aq)
E° = 0.72 V
What is the maximum electrical work that can be obtained from this
cell per mole of iron (III) ion?
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A galvanic cell has the following reaction. Zn(s) + 2
Fe(aq)
→ 2 Fe(aq)
+ Zn(aq)...
A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate the...
A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate the Gibbs free energy change at 25 °C when 2.61 g of iron is deposited. Assume the concentrations in the cell remain at the standard state values of 1 M through the entire deposition process. Calculate the maximum amount of work done by the cell on its surroundings.
Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl2(aq) → ZnCl2(aq)+Fe(s) Write...
Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl2(aq) → ZnCl2(aq)+Fe(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? Explanation Check © 2020 McGraw-Hill Education. All...
Suppose the galvanic cell sketched below is powered by the following reaction: 4 Fe(s)+2 Fe(NO3)2(aq) —...
Suppose the galvanic cell sketched below is powered by the following reaction: 4 Fe(s)+2 Fe(NO3)2(aq) — 3 Fe(NO3),(aq)+3 Fe(s) S1 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2:...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at...
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at 25 ∘C , given that [Fe3+]=0.00150 M and [Au3+]=0.795 M . Refer to the table of standard reduction potentials. E= V
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...
1)What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2(s) +...
1)What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2(s) + 2H2O + 2e- ⇄ Ni(OH)2(s) + 2OH-(aq), E°NiO2= 0.49 V; Fe(OH)2(s) + 2e- ⇄ Fe(s) + 2OH-(aq), E°Fe(OH)2= − 0.88 V. A)NiO2(s) + 2Fe(s) + 2H2O → Ni(OH)2(s) + 2Fe(OH)2(s) B)NiO2(s) + Fe(s) + 2H2O → Ni(OH)2(aq) + Fe(OH)2(aq) C)NiO2(s) + Fe(s) + 2H2O → Ni(OH)2(s) + Fe(OH)2(s) D)Ni(OH)2(s) + Fe(OH)2(s) → NiO2(s) + Fe(s) + 2H2O 2)What is the standard cell potential of...
A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2VO+2(aq)+4H+(aq)+Fe(s)->2VO+2(aq)+2H2O(l)+Fe+2(aq)...
A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2VO+2(aq)+4H+(aq)+Fe(s)->2VO+2(aq)+2H2O(l)+Fe+2(aq) Suppose the cell is prepared with 3.82 M VO+2 and 1.96 M H+ in one half-cell and 4.70 M VO+2 and 6.88 M Fe+2 in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
1) A particular voltaic cell operates on the reaction Zn(s) + Cl2(g) → Zn2+ (aq) +...
1) A particular voltaic cell operates on the reaction Zn(s) + Cl2(g) → Zn2+ (aq) + 2C1- has a cell potential of 0.853 V. Calculate the maximum electrical work generated when 15.0 g of zinc metal is consumed.
QUESTION 5 The following reaction takes place in the galvanic cell below: Zn(s) + Sn2+(aq) +...
QUESTION 5 The following reaction takes place in the galvanic cell below: Zn(s) + Sn2+(aq) + Zn2+(aq) + Sn(s) IT Select all statements that are true. A. Zn is the anode. B. Electrons flow from the zinc electrode to the tin electrode. Anions flow from the salt bridge toward the zinc electrode. UD. The mass of zinc electrode decreases while the mass of the tin electrode increases as the reaction progresses,
Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl2(aq) → ZnCl2(aq)+Fe(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? Explanation Check © 2020 McGraw-Hill Education. All...
Suppose the galvanic cell sketched below is powered by the following reaction: 4 Fe(s)+2 Fe(NO3)2(aq) — 3 Fe(NO3),(aq)+3 Fe(s) S1 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
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...
1) A particular voltaic cell operates on the reaction Zn(s) + Cl2(g) → Zn2+ (aq) + 2C1- has a cell potential of 0.853 V. Calculate the maximum electrical work generated when 15.0 g of zinc metal is consumed.
QUESTION 5 The following reaction takes place in the galvanic cell below: Zn(s) + Sn2+(aq) + Zn2+(aq) + Sn(s) IT Select all statements that are true. A. Zn is the anode. B. Electrons flow from the zinc electrode to the tin electrode. Anions flow from the salt bridge toward the zinc electrode. UD. The mass of zinc electrode decreases while the mass of the tin electrode increases as the reaction progresses,
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