Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s)...
Consider the following cell diagram:
Pt(s) | Fe3+(aq) , Fe2+(aq) ||
Cl–(aq) | Cl2(g) | Pt(s)
The reaction utilized by this cell is
Question 8 options:
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Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) |
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Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) |
|
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2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) |
|
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Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) |
|
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2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq) |
Homework Answers
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Consider the following cell diagram:
Pt(s) | Fe3+(aq) , Fe2+(aq) ||
Cl–(aq) | Cl2(g) | Pt(s)...
For the following electrochemical cell: Fe(s)| Fe3+(aq) || Cl(aq) | Cl2(g)|| Pt(s) a) Write the Cell...
For the following electrochemical cell: Fe(s)| Fe3+(aq) || Cl(aq) | Cl2(g)|| Pt(s) a) Write the Cell Reaction for this Cell. b) Identify the Anode and Cathode.
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the...
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V
Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential...
Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential is 0.683 V, what is the ratio of Fe2+(aq) to Fe3+(aq)? What is the ratio of these concentrations if the cell potential is 0.807 V?
Given the cell reaction: 2Cl–(aq) + Fe3+(aq) → Cl2(aq) + Fe2+(aq): (unbalanced) a) As written, is...
Given the cell reaction: 2Cl–(aq) + Fe3+(aq) → Cl2(aq) + Fe2+(aq): (unbalanced) a) As written, is the cell galvanic or electrolytic? b) Calculate ε°cell. c) Calculate ΔG°.
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+(aq) — 2CH(aq)...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+(aq) — 2CH(aq) + 2Fe3+(aq) O Fe2+ O Cl2 OCH O Fe3+
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq)...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq) + 2Fe 3+ (aq) Fe2+ Cl2 OCH Fe3+
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+...
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+ (aq) + 2 C1 (aq) Write a cell diagram for this reaction In this reaction, calculate Eºcell under standard conditions Calculate AGº from the cell potential B. C. D. Calculate K from the cell potential. E. Predict the value of Ecell for this reaction in if the concentration of is 0.150 M, is 0.100 M and the concentration of Cl- is 0.010 M. Fe2+...
QUESTION 8 Based on the following cell notation, write a balanced and complete redox reaction: Ca),...
QUESTION 8 Based on the following cell notation, write a balanced and complete redox reaction: Ca), sat. KCI Fe, Fe2 |Pt Ag) AgCl O A. Ag(s) +CI-(aq)Fe2+ AgCI (s) +Fe3+ = O B. AgCl (s)+ Fe2+ = Ag(s) +CI-(aq) Fe3+ CAg(s) +CI-(aq) + Fe2+ = AgCl(s) + Fe3+ D.Ag(s)CI-(aq) + Fe3+ AgCl(s)+ Fe2+ E. Ag(s)+CI-(aq)+2Fe2+= AgCI(s) +2FE3+
Write the shorthand cell notation for each of the following reactions: a. Cu(s) + 2Fe3+(aq) →...
Write the shorthand cell notation for each of the following reactions: a. Cu(s) + 2Fe3+(aq) → Cu2+(aq) + 2Fe2+(aq) b. 2Cl- (aq) + 2Fe3+(aq) → Cl2(g) + 2Fe2+(aq)
4. a) Determine Eº for the cell Pt (s) | Cl2 (g) | Cl− (aq) ||...
4. a) Determine Eº for the cell Pt (s) | Cl2 (g) | Cl− (aq) || Pb2+ (aq), H+ (aq) | PbO2 (s). b) What is the Standard Gibbs free energy of this reaction?
For the following electrochemical cell: Fe(s)| Fe3+(aq) || Cl(aq) | Cl2(g)|| Pt(s) a) Write the Cell Reaction for this Cell. b) Identify the Anode and Cathode.
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+(aq) — 2CH(aq) + 2Fe3+(aq) O Fe2+ O Cl2 OCH O Fe3+
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq) + 2Fe 3+ (aq) Fe2+ Cl2 OCH Fe3+
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+ (aq) + 2 C1 (aq) Write a cell diagram for this reaction In this reaction, calculate Eºcell under standard conditions Calculate AGº from the cell potential B. C. D. Calculate K from the cell potential. E. Predict the value of Ecell for this reaction in if the concentration of is 0.150 M, is 0.100 M and the concentration of Cl- is 0.010 M. Fe2+...
QUESTION 8 Based on the following cell notation, write a balanced and complete redox reaction: Ca), sat. KCI Fe, Fe2 |Pt Ag) AgCl O A. Ag(s) +CI-(aq)Fe2+ AgCI (s) +Fe3+ = O B. AgCl (s)+ Fe2+ = Ag(s) +CI-(aq) Fe3+ CAg(s) +CI-(aq) + Fe2+ = AgCl(s) + Fe3+ D.Ag(s)CI-(aq) + Fe3+ AgCl(s)+ Fe2+ E. Ag(s)+CI-(aq)+2Fe2+= AgCI(s) +2FE3+
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