The emf of the cell, H-(1 bar)|HCl(0.01 m)|AgClI(s)|Ag is given by E(in volts) = -0.096 +...
For the cell: Ag 's)| H2 (9) (Р %3D 1 bar), HCI (b = 1.00 molal), AgCl (s) | Ag(s) The standard cell potential was measured at different temperatures and the resulting data was fitted to a polynomial expression. The result is: E = 0.22233 - 0.0006477(T - 298.15) - 3.241 x 10-6(T - 298.15)2 Volts With T the Kelvin temperature What is the equilibrium constant for the cell reaction at 280 K?
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell° for this galvanic cell? If a more complete description of the cell is Ag(s)│Ag(NO3)(aq, 0.50 M)││KMnO4(aq, 0.50 M), HCl(aq, 2.5 M), Mn(Cl)2(aq, 0.01 M)│Pt(s), Ag(s) what is Ecell? What is the balanced, spontaneous cell reaction for the cell conditions given in b.?
1--What is E°cell for the following hypothetical reaction exactly as written (in volts), given the standard electrode potential (E°) values below? X(s) + Y2+(aq) → X2+(aq) + Y(s) X2+(aq) + 2 e- → X(s) E° = -0.69 V Y2+(aq) + 2 e- → Y(s) E° = -2.45 V 2--In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Pt(s)|H2(g)|H+(aq)|| Ag(s)|Ag+(aq) Select one...
Corrosion Problem: Electrode Electrode Pb (s) PbCh (s) HCl (aqueous) AgCI (s)Ag (s) The emf of the cell represented in the accompanying diagram is 0.490 V at 25°C and the temperature coefficient is-1.84 × 10-4 VpC. All the compo- nents are present as pure solids in contact with an HCl electrolyte. (a) Write the half-cell reactions. (b) Write the overall cell reaction (c) Calculate the Gibbs free energy change and the entropy change for this reaction.
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AG° at 25° for 12 H2 (g) + AgCl(s) – HCl(aq) + Ag(s) Select one: a.-23.2 kJ/mol b. 21.2 kJ/mol C.-22.2 kJ/mol d. 23.2 kJ/mol e. 22.2 kJ/mol
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 - 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AS° at 25° for 12 H2 (g) + AgCl(s) + HCl(aq) + Ag(s) Select one: a. 27.5 J/mol K b. -47.5 J/mol.k c. 47.6 J/mol K d. 37. e. -37. Ashwaq sent a photo
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
A. Calculate the cell potential that would result in the following electrochemical cell at 25oC: Pt | UO22+(0.10M),U4+(0.22M),H+(0.60M) || Ag+(0.034M) | Ag Line notation is anode || cathode Write Nernst equations for the anode and cathode separately. Then Ecell = Ecathode - E anode B. If the electrochemical cell Ag/AgCl || Zn2+(x M) | Zn(s) develops a potential of -1.039 volts at 25oC, what is the Zn2+ concentration in the solution? (Answer in decimal format) Ag/AgCl reference electrode has E=0.199...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...