Sketch the galvanic cell based on the following overall reactions. Calculate e°; show the direction of electron flow and the direction of ion migration through the salt bridge; identify the cathode and anode; and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. Refer to the table above for the standard reduction potential a. Cr3+ (aq) + Clz(9)= Cr,03-(aq) + C-

A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was needed to plate 3.25 g of Zn onto the metal using a current of 25.99 A? 21.

Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction of electron flow and the direction of ion migration through the salt bridge; identify the cathode and anode; and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. Refer to the table above for the standard reduction potential. Also, calculate AG° and K at 25 °C for the galvanic cell reaction a. Clz + 2e- - 201- E° = 1.36 V Brz + 2e → 2Br E° = 1.09 V

A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution.  The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction experimental standard cell potential, Eocell, for the reaction=1.06 Your answer should have 3 sig figs.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2VO (aq) + 4H (aq) + Fe(s) → 2V0²+ (aq) + 2H₂O (1) + Fe²+ (aq) - Suppose the cell is prepared with 0.0538 M VO and 7.99 M H* in one half-cell and 5.62 M VO2+ and 2.30 M Fe2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 μ X G

An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a current of 9.00 A. If inert electrodes are used in the process, how many grams of copper were removed from the solution?

An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping a cobalt rod in a solution of CoCl2(aq), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. d. The standard cell potential for this electrochemical cell is 0.482 V and two moles of electrons are exchanged per mole of reaction. What is equilibrium constant, K, for the redox reaction described by this electrochemical cell at 298 K?

20. A galvanic cell is constructed at 25°C as indicated in the shorthand cell notation: Determine the Eºcell, AG° and Kc. Eºcell = AGO = Au(s) | 1.0 M Au³+ (aq) || 1.0 M Au³+ (aq) | Au(s) Kc = ကိုယ် E° = +1.50 V cat-an

Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter. Calculate the standard cell potential.  If the initial concentrations of Zn2+ and of OH– are 1.0 × 10–7 and 2.0 × 10–7, respectively, calculate the cell potential after the Zn2+ concentration has increased by a factor of 100. At this point, what percentage of the initial voltage remains?

A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate solution (4M). Calculate the molarity of the solution at the end of electrolysis