I am not sure how to answer this question
I am not sure how to answer this question Consider the cell described below at 285...
HHelp ASAP Consider the cell described below at 283 K: Sn | Sn2+ (0.871 M) || Pb2+ (0.927 M) | Pb Given E°Pb2+>Pb = -0.131 V, E°şn2+-Sn = -0.143 V. Calculate the cell potential after the reaction has operated long enough for the Sn2+ to have changed by 0.355 mol/L. -2780 V Incorrect. Tries 6/45 Previous Tries Submit Answer
Consider the cell described below at 253 K: Sn | Sn2+ (0.979 M) || Pb2+ (0.943 M) | Pb Given E°pb2+_Pb = -0.131 V, Eºsn2+_Sn = -0.143 V. Calculate the cell potential after the reaction has operated long enough for the Sn2+ to have changed 0.355 mol/L. .00893 V Submit Answer You have entered that answer before Incorrect. Tries 5/45 Previous Tries
I am not sure how to answer this question A concentration cell is built based on the reaction: 2H+ + 2 + H2 The pH in one of the half cells is -0.2945, while the pH in the other is 2.924. If the temperature of the overall cell is 287 K, what is the potential? (Faraday's constant is 96,485 C/mol e) Submit Answer Tries 0/45
Please show all work step by step and final answer. Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. Pb2+ + 2e - Pb Fe2+ + 2e...
Please show all work step by step and final answer. Selective Reduction The standard reduction potential for the half-reaction: Sn4+ + 2e + Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. Sn- Sn2+ + 2e Sn2+ Sn4+ +...
Question 30 (6 points) What is the equilibrium constant (K) at 25°C for the following cell reaction? Sn(s) + Pb2+ (aq) → Sn2+ (aq) + Pb(s); Eºcell = 0.014 V (Please submit your detail solution work to the dropbox, which can be found in the assignments.) A/
Consider the cell described below at 253 K: Fe | Fe2+ (0.867 M) || Cd2+ (0.945 M) | Cd Given EoCd2+Cd -0.403 V, E°Fe2+_Fe = -0.441 V. Calculate the cell potential after the reaction has operated long enough for the Fe2+ to have changed by 0.311 mol/L. Tries 0/45 Submit Answer
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. 2H+ + 2e - H2 Fe3+ + 3e + Fe Sn2+ + 2e Fe2+ + 2e →...
A concentration cell is set up using the following reaction: Sn4+ (aq) + 2e – Sn2+ (aq) ° = 0.150 V The standard line notation, including initial concentrations, for this cell is shown below: (Please note that concentration of ions shown in the anode compartment are in the same order as in the cathode compartment.) Pt (s)[Sn4+] (0.645 M), [Sn2+ ](1.39 M) || (Sn4+] (1.37 M), [Sn2+] (0.611 M) |Pt (s) The initial potential of this concentration cell, at 298...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...