QUESTION 27 Calculate Ecell under non-standard conditions for the following electrochemical cell: Pt(s)| FeCl2 (aq, 0.150...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
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.?
Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) | Fe3+ (aq)| Pt The cell is constructed by preparing one half-cell with a solution containing 8.33 * 10-3 M FeCl3 and 1.67*10-2 M FeCl2, and preparing the other half-cell with a solution containing 8.33*10-3 M CuCl2 and 0.025 M CuCl. Calculate the cell potential once the half-cells are connected to each other. E°(Cu2+/Cu+) = 0.16 V; E°(Fe2+/Fe3+) = 0.77 V
The following electrochemical cell was set up in the lab Pt│Fe(NO3)2, Fe(NO3)3││Ag(NO3)│Ag What is Ecell°? If a more complete description of the cell is Pt│Fe(NO3)2(0.200 M), Fe(NO3)2(0.150 M)││Ag(NO3)(0.200 M) │Ag what is Ecell? c. What is the spontaneous cell reaction for the cell conditions given in b.?
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq) | Pt,H2 (g) (P=1.00 atm) calculate DG° in kJ calculate Ecell for [H+] = 0.8 M and [Zn2+] = 0.5 M calculate K at 25°C
Calculate Ecell (the reduction potential for the balanced chemical equation under nonstandard conditions) for the electrochemical cell shown below: Pt | Fe2+ (4.25x10-3 M), Fe3+ (1.50x10-3 M) || MnO4 - (6.50x10-3 M), Mn2+ (2.00x10-2 M), H+ (0.100 M) | Pt. Use the following standard reduction potentials for each half reaction. The Eo for Fe3+/Fe2+ = 0.77 V and Eo for MnO4 - /Mn2+ = 1.51 V.
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 an electrochemical cell, starting with standard state conditions, based on the following reaction. 2 H*(aq)+ Cd(s) Cd2+(aq) H2g) Ecell 0.40v Which of the following actions would increase the measured cell potential? Reducing the [H'] in the hydrogen cell O Increasing the mass of the solid Cd electrode Reducing the Cdion concentration O Increasing the pressure of hydrogen gas in the hydrogen cell O None of these
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M)| Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect