The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E by the equation Standard reduction potentials In K Reduction half-reaction E° (V) where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 06 500 C mol, R (the gas constant) is equal to 8.314 JK'mol, and Tis the Kelvin temperature. Ag' (aq) +e+Ag(a) Cu" (ag) + 2e Cu(s) Sn* (ag) + de-+Sn(s) 0.80 0.34 0.15 2H' (ag) + 2e-H3(9) N (ag) + 20-Ni(a) -0.26 Fe (ag) + 2eFe(a) -0.45 Zn" (ag) + 20-»Zn(s) -0.76 AB (ag) + 30 -+Al(s) -1.00 Mg* (aq) + 20 –→Mg(s) -2.37 • Part A Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + N* (ag)-→F¢²*(aq) + Ni(o) Express your answer numerically. View Available Hint(s) Templates Symbol undo redo feset keyboard shortcuts Help

For the cell shown, the measured cell potential, Ecell, is –0.3521 V at 25 °C. Pt(s) | H,(g, 0.785 atm) | H* (aq, ? M) || Cd²*(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H* (aq) + 2e- - H, (g) E° = 0.00 V Cd²* (aq) + 2e" - Cd(s) E° = -0.403 V Calculate the H* concentration. [H*] = M

The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2 H2O(I) + 2 NO2(g). Thestandard cell potential at 25 °C is -0.04 V. Calculate the electricalwork that can be done by the cell.

An aqueous ScCl3 solution is electrolyzed under 1 bar pressure using platinum electrodes.(a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Cl2(g) + 2 e-  2 Cl-(aq) 1.360 O2(g) + 4 H3O+(aq) + 4 e-  6 H2O(l) 1.229 2 H2O(l) + 2 e-  H2(g) + 2 OH-(aq) -0.828 Sc3+(aq) + 3 e-  Sc(s) -2.080 Half-reaction at anode:     +       +       -->       +       +     Half-reaction at cathode:     +       +       -->       +       +     (b) What is the expected decomposition potential?  ________V

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Consider the following table of standard electrode potentials Standard Electrode Potentials at 25 °C Reduction Half-Reaction E" (V) Au" (ag) + Зе Ag"(aq) + Fe* (aq) + 3e Sn²(aq) v*(aq) + 3e In"(ag) + 3e Eu" (ag) + 3e Cr* (aq) Тa" (ag) + Зе Zn*(aq) Nb* (aq) » Au(s) 1.50 e Ag(s) 0.80 » Fe(s) -0.04 + 2e » Sn(s) -0.14 » V(s) -0.26 » In(s) -0.34 » Eu(s) -0.35 + 3e » Cr(s) -0.42 » Ta(s) -0.60 » Zn(s) » Nb(s) → Ti(s) → Al(s) » Be(s) + 2e -0.76 + 3e -1.10 Ti (aq) + 2e Al" (aq) + 3e Ве (ag) + 2е Am* (ag) + 2e -1.63 -1.66 -1.85 » Am(s) -1.90 Pr* (ag) + 2e" » Pr(s) -2.00 Mg* (aq) + 20 - Mg(s) » Na(s) » Ca(s) -2.37 Na (aq) + Ca*(aq) Sr* (aq) + 2e Ba (aq) e -2.71 2e - 2.87 » Sr(s) -2.90 + 2e + Ba(s) -2.91

A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M

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A much-studied cell in electrochemistry has the following cell notation: Ag(s) | AgCI(s) || HCl(aq) | H2(g) | Pt(s) Bearing in mind that HCl(aq) consists of H*(aq) and Cl'(aq), and that this solution is in contact with both electrodes (there is no salt bridge), write down balanced equations for 3. a) the anode half-reaction. b) the cathode half-reaction. c) the cell reaction.

For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7