please answer this question?? 7:29 *4 72% < Question 27 of 28 Submit For the galvanic...
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)...
Question 10 of 11 For the galvanic (voltaic) cell Cd2+ (aq) + Fe(s) — Cd(s) + Fe2(aq) (E° = 0.0400 V), what is the ratio [Fe2+1/[Cd2+] when E = 0.002 V? Assume T is 298 K (1 2 3
For the galvanic (voltaic) cell Cd2+ (aq) + Fe(s) Cd(s) + Fe2+(aq) (E° = 0.0400 V), what is the ratio [Fe2+1/[Cd2+] when E = 0.001 V? Assume T is 298 K 1 2. 3 Х 4 5 6 C 7 8 9 + +/- 0 x 100
the question is on the the bottom of the image! please answer the question is : using the measured potentials give the cell notations of at least 10 possible galvanic cells that do not use zinc in them. Eºcell (V) Cell +0.62 Anode: Zn(s) in ZnSO4(29) Cathode: Ca(s) in CuSO4(20) -0.51 Anode: Zn(s) in ZnSO4(29) Cathode: Ni(s) in NiSO4(aq) - 1.61 Anode Zn(s) in ZnSO4(29) Cathode: Mg(s) in MgSO4(aq) Anode Zn(s) in ZnSO4(0) Cathode: Mn() in MnSO4(aq) -0.42 Anode: Zn(s)...
please show work and how they got the answer 13. If [Cu2+] = 0.30 M for the same cell described below, then what concentration of Fe2+ is needed to result in Ecell = 0.76 V? You will need to use the standard reduction potential table. Cu2+/ Cu → E = +0.34 V Fe2+/ Fe → E = -0.45 Cu?* (aq) + Fe(s) - Fe* (aq) + Cu(s) Eºcell = +0.78 V, Q = x/ 0.30, X = [Fe2+], Using Nernst,...
Answer all question (a-d) thank you Consider a galvanic cell which has an Iron electrode submerged in a Fe(NO3)2 soln. and a Gold electrode submerged in a Au(NO3)3 soln. a) Find the Ecell of this cell under standard conditions: (2pts) Ans: Au3+ (aq) + 3e = Aus) ER 1.50 V + 2e = Fe(s) Er = -0.44 V Fe2+ (aq) b) Write out the balanced net reaction of this cell? (3pts) c) What is the cell potential if the concentration...
pleaae do all, please please please QUESTION 3 Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2+(aq) + 2 e <-> Mn(s) E = -1.18 V Cr3+ (aq) + 3 e <-> Cris) - 0.41 V A Mn (s) | Mn 2+(aq, 1.0 M) 1 Cr3+(aq. 1.0 M) | Cris) B. Mn (s) Mn 2+(aq, 1.0 M) || Cris) | Cr3+(99, 1.0 M)...
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)...
help with these please LU 101 is question. Consider the following half-reactions: JE° (V) Half-reaction Hg2+ (aq) + 2e → Hg(0.855V Ca2+(aq) + 2e —— C 0.403V Fe2+ (aq) + 2e -> Fe(s) 0.440V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Fe2+(aq) oxidize Hg() to Hg2+ (aq)? O y (6) Which species can be oxidized by Cd²+ (aq)? If...
a b and c please 7. Consider a galvanic cell which has an Iron electrode submerged in a Fe(NOsha olm. and Goldlectrode submerged in a Au(NO3), soln. a) Find the Eceu of this cell under standard conditions: (2pts) Ans Aut(aq) + 3 = Au ER - 1.50 V Fe? (0) +2e=Fe( ER=-0.44 V b) Write out the balanced net reaction of this cell? (3pts) c) What is the cell potential if the concentration of the Iron ions is 1.50 M...