Determine the AG in KJ for a voltaic cell made of a Zn strip and a Pb strip immersed in 1.0 M aqueous Zn(NO3)2 and Pb(NO3) 2 solutions, respectively, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.)

6) Calculate the potential of a cell, Eºcell, made with a standard bromine electrode as the anode and a standard chlorine electrode as the cathode. Write the shorthand cell notation.

A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. V 'cell II

Determine the ΔG° in KJ for a voltaic cell made of a Ag strip and a Pb strip immersed in 1.0 M aqueous AgNO3 and Pb(NO3)2 solutions, respectively, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.)   Determine the thermodynamic equilibrium constant K for a voltaic cell made of a Zn strip and a Pb strip immersed in 1.0 M aqueous Zn(NO3)2 and Pb(NO3)2 solutions, respectively, at 25.00°C, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.)

Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   NO3-     +      H+        +      Zn        ->         Zn2+     +       NO2     +       H2O

What is the cell potential for a voltaic cell having one electrode composed of a Zn strip dipped in a 0.034 M Zn(NO)(aq) solution and the other electrode composed of a Zn strip dipped into a 0.414 M Zn(NO)(aq) solution? Assume all other cell components are in place and the temperature is 25.0°C.   To produce 1.21 kg of solid potassium from molten KCl, how many hours must 0.721 amps be passed through the KCl?   How many hours will you have to electrolyze the forks to apply 0.500 g of Ag to each one? Your electrolysis device operates at a current of 3.75 amps.

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg? +] = 0.788 M and [Fe² +] = 0.0200 M. Use the standard reduction potentials in this table. Mg(s) + Fe2+(aq) = Mg2+(aq) + Fe(s) E = V

The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard conditions. Zn(s) + Cu2+(aq) => Cu(S) + Zn2+(aq) What is the cell potential when one of the following deviations from standard conditions are made?  A) [Zn2+] = 0.25 M; [Cu2+] = 0.25 M B)  [Zn2+] = 0.25 M; [Cu2+] = 0.50 M C)  [Zn2+] = 0.75 M; [Cu2+] = 0.75 M D)  [Zn2+] = 0.75 M; [Cu2+] = 0.25 M E)  [Zn2+] = 0.25 M; [Cu2+] = 0.75 M

What is the overall cell reaction and the standard cell potential of a galvanic cell employing the following half-reactions ? NiO 2(s) +2H 2 O+2e^ -. ---> Ni(OH) 2(s) +2OH^- (aq) E ^ 0 = 0.49V   Fe(OH) 2(s) +2e^ - ----> Fe (s) +2OH^- (aq) E ^ 0 = - 0.88 V

Calculate the standard free-energy change of a voltaic cell with a potential of 0.35 V under standard conditions. Assume that 2 moles of electrons are transferred in the balanced oxidation-reduction reaction