a. Pb(s) ---------------> Pb^2+ (aq) + 2e^- E0 = 0.13v
2Ag^+ (aq) + 2e^- --------> 2Ag(s) E0 = 0.80v
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Pb(s) + 2Ag^+ (aq) ----------> Pb^2+ (aq) + 2Ag(s) E0cell = 0.93v
b.
2I^- ---------------> I2(s) + 2e^- E0 = -0.54v
2ClO2(g) + 2e^- ------> 2ClO2^- E0 = 0.95v
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2ClO2(g) + 2I^- (aq) ------------> 2ClO2^- (aq) + I2(s) E0cell = 0.41v
C.
2Zn(s) ---------------------> 2Zn^2+ (aq) + 4e^- E0 = 0.76v
O2(g) + 4H^+ (aq) --------> 2H2O(l) E0 = 1.23v
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2Zn(s) + O2(g) + 4H^+ (aq) ---------> 2Zn^2+ (aq0 + 2H2O(l) E0cell = 1.99v
4. Determine the standard cell potential for each of the electrochemical cells. 2Ag(s) + Pb2+(aa) 2"...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Calculate the standard cell potential for each of the electrochemical cells.2Ag+(aq)+ Pb(s)---> 2Ag(s) +Pb^2+(aq)Express your answer using two significant figures.Ecell=? V2ClO2(g)+2I-(aq)--->2ClO2-(aq)+I2(s)Express your answer using two significant figures.Ecell=?VO2(g)+4H+(aq)+2Zn(s)--> 2H20(l) + 2Zn2+(aq)Ecell=?V
- Write the reactions below in cell notation. a. 2Ag+ + Pb(s) + 2Ag(s) + Pb2+(aq) b. 20102(g) + 21 (aq) → 2C102 (aq) + 12(s) C. O2(g) + 4H+(aq) + 2Zn(s) → 2H2O(l) + 2Zn2+(aq)
Exercise 19.49 Use line notation to represent the electrochemical cells for each of the following overall redox reactions. Part A 2Ag+ (aq) + Pb(s) +2Ag(s) + PbP (o) O Ag(s) Ag+ (aq)||Pb2+ (aq) Pb(6) O Ag+ (aq) Ag(0) Pb(s)[Pb (4) O Pb2+ (aq)|Pb()||Ag()|Ag (og) O Pb(s)|Pb2+ (aq)||Ag+ (aq)|A6(*) Submit Request Answer Part B 2010 (8) +21 (aq) +2010, (4) +10) O Pt()CIO; () CIO,()||()T()Ps) Pt(s) C10(e) C10, (w) (0) (0) Pt(s) O POT" (aq) (||C10(e)C10; ()Pt(s) OPt()LOT ()||CO, (w) CIO,()PC)...
When the Pb2+ concentration is 1.17 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.356V. What is the Mg2+ concentration? Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq) Answer: _____M
14. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at 298.15 K. a) Hg(l) + S2-(ag, 0.10 M) + 2Ag+(ag, 0.25 M) → 2Ag(s) + HgS(s) \ (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half-cell consisting of a nickel electrode in 0.25 M...
Use line notation to represent the electrochemical cells for each of the following overall redox reactions. 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s) O2(g)+4H+(aq)+2Zn(s)→2H2O(l)+2Zn2+(aq) please help! thank you!!
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Please explain, thank you! (4) Consider a cell at 298 K in which the reaction is Pb (s)+2H (aa-Pb2+ (ag) +H2 (g) (a) Cr ions are added to the Pb|Pb2+ half-cell to precipitate PbCh. The cell voltage is then measured to be +0.210 V. If [H]-1.0 M and the partial pressure of hydrogen is 1.0 atm, what is [Pb2*]? (answer: 1.57 x 103 M) (b) Calculate the Kp of PbCh if [Cl]-0.10 M in the PblPb2 half-cell. (answer: 1.57 x...
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as written). Identify each oxidizing agent and reducing agent. Ni (s) + Zn2+(aq) ----> Ni2+(aq) + Zn (s) Ni (s) + Pb2+(aq) -------> Ni2+(aq) + Pb (s) Al (s) + 3 Ag+(aq) ---------> Al3+(aq) + Ag (s) Pb (s) + Mn2+(aq) ----------> Pb2+(aq) + Mn (s)