For each of the following galvanic cells (1) write out the conventional (overall) cell reaction and...
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+
Part A Write a balanced equation for the overall cell reaction in the following galvanic cell Pt(s) Br (aq) Br2 () || Cl2 (g) | Cl- (aq) Pt(s) Express your answer as a chemical equation including phases. ΑΣφ ? а а ха х Хъ b b Request Answer Submit 11L
Problem Set #34: Galvanic Cells & Standard Reduction Potential Practice Sheet Directions: (a) Sketch the galvanic cell based on the following overall reaction OR half- reactions. o Show the direction of electron flow o Identify the cathode and anode (b) Give the overall balanced reaction (c) Determine the Evalues for each of the galvanic cells. (d) Give the standard line notation for each cell. (Assume that all concentrations are 1.0M and that all partial pressures are 1.0 atm) 1. 103(aq)...
Show all steps please :) A galvanic cell is prepared using the following two half-cells: (i) MnO4 (0.273 M), Mn2+ (0.167 M), and H+ (1.0 M), and (ii) Fe2+ (0.247 M) and Fe3+ (0.389 M). The standard reduction potentials for the two half cells are: Mnoa + 8H+ + 5e – Mn2+ + 4H20 E° = 1.507 V Fe3+ + e- Fe2+ E° = 0.770 V a) Calculate the voltage for this galvanic cell. b) Write the balanced equation for...
What is the overall cell reaction for the galvanic cell given in shorthand below? Pt(s) i H2(g) | H+(aq) || Cl2(g) CI(aq) Pt(s) A. Pt(s) + H2(g) + CI+(aq) - Pt(s) + 2 H+(aq) + 2 C12(g) B. 2 H+(aq) + 2 C12(g) → 2 HCl(aq) CH2(g) + Cl2() - 2 H+(aq) + 2 CİH(aq) None of these is correct.
17.32. Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balanced equation for the cell reaction, and identify which half-reaction takes place at each anode and cathode. a. Cdº'(aq) + 2 e - Cd(s) Agt(aq) + e - Ag(s) b. AgBr(s) + e - Ag(s) + Br"(aq) MnO2(s) + 4 H*(aq) + 2 e-Mn2(aq) + 2 H2O(0) c. PtCl 2- (aq) + 2 e-Pt(s) + 4 Cl(aq) AgCl(s) + e- Ag(s) + Cl(aq)
Question 4 (1 point) Write the cell diagram for the reaction 2AgCl(s) + H2(g) --> 2Ag(s) + 2H+(aq) + 2C1-(aq) OPt(s) | H2(g)| H+(aq) || CI+(aq)| AgCl(s) | Ag(s) Pt(s) | H2(g)| H+(aq) || CI+(aq) | Ag(s) | Pt(s) O Ag(s) | AgCl(s) || H+(aq), Ci-(aq) | H2(g) | Pt(s) O Ag(s) | AgCl(s) | CI+(aq) || H+(aq)| H2(g) | Pt(s) Pt(s) Cl(aq), H(aq)| H2(g) || AgCl(s) Ag(s)
What is the shorthand notation that represents the following galvanic cell reaction? Sn2+(aq) + Cl2(g) → Sn3+(aq) + 2 Cl-(aq) A) Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) B) Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) C) Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) D) Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
3.Consider a galvanic cell based on the reaction. Assume theses reactions are carried out in acidic media and that all concentrations are 1M and that all partial pressures are 1 atm. a) MnO4 (ag)+ CIO3 (ag) CIO4 (ag) + Mn (aq) b) Cr (aq+ Cl2(ag) Cr O2 +CI (aq) (aq) For each the above overall reactions, answer thee following questions. identify the cathode and anode. b. Give the overall balanced equation. How many electrons are transferred? a. c. d. Calculate...