Calculate the equilibrium constant, K, at 298 K for the cell: Pb |Pb2+ || Ag+ | Ag The standard reduction potential for the Pb2+/Pb couple is -0.13 V, and it is +0.80 V for the Ag+/Ag couple.
Calculate the equilibrium constant, K, at 298 K for the cell: Pb |Pb2+ || Ag+ |...
Design a voltaic cell with the following two reduction half-reactions: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Pb2+(aq) + 2 e− ⟶ Pb(s) Eo = −0.13 V Calculate Eocell and the equilibrium constant K for the voltaic cell at 298 K. Click here for a copy of Final Exam cover sheet.
Consider the cell. Cu ∣ Cu2+ (0.00534 M)∣∣ Pb2+ (0.00735 M) ∣∣ Pb Calculate the half‑cell reduction potential at 298 K at the cathode. ? cu2+/cu=+0.34V ?cathode=......V Calculate the half‑cell reduction potential at 298 K at the anode. ? pb2+/pb=-0.13V ?anode=....V What is the initial potential needed to provide a current of 0.0800A if the resistance of the cell is 4.13Ω? Assume that ?=298 K. ?applied=......V
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...
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equilibrium with PbI2. The measured avgerage cell potential of Pb-PbI2 is 0.084 V the known [Pb2+] is 0.050 M Eo of Pb2+ (aq) + 2 e- --------> Pb(s) is -0.13 V 0.050 M KI Mixed 9 mL of 0.050 M KI with 3 mL of 0.050 M Pb(NO3)2 .
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.13 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Pb2+/Pb couples are 0.00 and -0.13 V, respectively. voltmeter saltbridge 1+ Pl(s) LPH2 (g) O Pb2+(aq) + H2(g) --> Pb(s) + 2H+(aq) O Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g)
salt bridge Pb2+2 e Eo0.13 V Pb (s) Ag1 e o = 0.80 V Ag (s) What is the voltage, at 298 K, of this voltaic cell starting with the following non-standard concentrations: [Pb2+1 (aq) 0.063 M [Ag (aq) 0.61 M Use the Nernst equation: E=E- (RT/nF) In Q First calculate the value of Q, and enter it into the first answer box. Q is dimensionless. Then calculate E, the non-standard cell potential, and enter its value into the second...
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode. If the voltmeter reading is –0.13 V, match each electrode with its correct name. Given: Standard reduction potential of the H+/H2 and Pb2+/Pb couples are 0.00 and –0.13 V, respectively. Question 2 options: 12 Pb2+|Pb electrode 12 standard hydrogen electrode 1. anode 2. cathode
6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(aq)....
Question 8 (1 point) Calculate the equilibrium constant, K, for the spontaneous galvanic cell between Pb2+/Pb and Cr3+/Cr2+ conducted at standard conditions. 7.9 x102 1.7 x1014 3.1 x109 5.6 x104 Show Report OE PASSW STRAIN605 lenovo
The standard reduction potential of the Pb2+|Pb electrode is –0.13 V and the standard potential of the cell Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s) is +0.63 V. What is the standard reduction potential of the Zn2+|Zn electrode? Question 9 options: –0.76 V –1.52 V +0.76 V –0.50 V +0.50 V