I need help please Sapling Learning he cell Pt (s)HXg, 0.833 atm)H'(aq, 7 M)Cd (aq, 1.00 M)ICd (s) values, E", are as follows E-0.00 V E-0403 v 2H(a)+eH Tools Sapling Learning he cell...
For the cell shown, the measured cell potential, ?cell, is −0.3629 V at 25 °C. Pt(s) | H2(g,0.899 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, ?o, are 2H+(aq)+2e−⟶H2(g)?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)?o=−0.403 V Calculate the H+ concentration. [H+]=
For the cell shown, the measured cell potential, Ecell, is -0.3689 V at 25 °C. Pt(s)H,(g, 0.789 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) + 24 H, (g) E° = 0.00 V Cd²+ (aq) + 2e - Cd(s) E = -0.403 V Calculate the H+ concentration. [H+] =
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.
For the cell shown, the measured cell potential, Ecell, is −0.3587 V at 25 °C.Pt(s) | H2(g,0.849 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, E⁰, are2H+(aq)+2e−⟶H2(g) E⁰=0.00 VCd2+(aq)+2e−⟶Cd(s) E⁰=−0.403 VCalculate the H+ concentration.
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!
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s) | H, (8,0.873 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, (g) E° = 0.00 v Cd2+ (aq) + 2e- Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+) = .0588 M Incorrect
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
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 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. [HT] = M
Given the measured cell potential, E_cell, is -0.3657 V at 25 degree C in the following cell, calculate the H^+ concentration Pt (s)|H_2(g, 0.801 atm)|H^+ (aq, ? M)||Cd^2+ (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E degree, are as follows. 2H^+ (aq) + 2e^- rightarrow H_2 (g) E degree = 0.00 V Cd^2+ (aq) + 2e^- rightarrow Cd (s) E degree = -0.403 V [H^+] =
For the cell shown, the measured cell potential, Ecell, is -0.3711 V at 25 °C Pt(s) H2(g, 0.865 atm) | Ht (aq,? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H"(aq) + 2е — H2(g) Eo = 0.00 V Cd2+(aq)2 e - Cd(s) Eo =-0.403 V Calculate the Ht concentration М