Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: Fe + Ni^2+     →      Fe^2+ + Ni (b) What is the value of E if the concentration of Ni^2+ is 4.17 x 10^-2 and the concentration of Fe^2+ is 5.06 x 10^-3? (c) If E = 0.36 V and Ni^2+ = 0.10 M, what is the concentration of Fe^2

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 (Equation 6). Your answer should have 3 sig figs.  Use your answer from question 4. Question 4 + answer: Calculate the experimental standard state free energy change, ΔGo, for the reaction: ANSWER:  -1.99e5 Equation 6 Attached:

If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long , (in hours) will it take to produce 2.0 Ibs of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs) hr

A student wanted to measure the concentration of cobalt(II) ion in an aqueous solution. For the cathode half-reaction, she used a silver electrode with a 0.51 M solution of AgNO3. For the anode half-reaction, she used a cobalt electrode dipped into the aqueous solution. If the cell gave a potential of 1.043 V at 25 °C, what was the concentration of Co2+ in the solution? Half-reaction E° (V) Ag*(aq) + e- Ag(s) +0.7996 Co2+(aq) + 2 e- -0.28 Co(s) Your Answer: Answer units

A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo = 0.34 V. If the cell contains 0.00178 M concentrations of HCl and CuSO4, what potential does it produce?

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 Your answer should have 3 sig figs.

In the electrolysis of a solution containing Ag* (aq), metallic Ag(s) deposits on the cathode. Using a current of 1.42 A for 2.30 hours, what mass of silver forms? Mass =

Which of the following reactions occurs at the anode of an electrochemical cell composed of Zn│Zn2+(aq) and Fe│Fe2+(aq) half-cells? Their reduction potentials are as follows:                 Zn2+   +  2e–   -->  Zn;    Eo = -0.763 V                              Fe2+  +  2e–   -->  Fe;      Eo = -0.447 V     (A) Zn2+ + 2e– -->  Cr;                     (B) Zn -->  Zn2+ + 2e–;                    (C) Fe -->  Fe2+ + 2e–;              (D) Fe2+ + 2e– -->  Fe;