5(a) 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: Mn + Cd2+ → Mn2+ + Cd (b) What is the value of E if the concentration of Cd2+ is 5.88 x 10-5 and the concentration of Mn2+ is 6.88 x 10-3? (c) If E = 0.98 V and Cd2+ = 0.10 M, what is the concentration of Mn2+ ?

Consider the following cell. Cr | Cr³+ (1.00 M) || Ni²+(1.00 M) | Ni & = 0.68 V (a) How many milligrams of metallic nickel would be plated on the cathode if a current of 0.16 A is drawn for 1.3 hrs? 4.0 2.3e2 mg (b) What is the Cr³+ concentration when the Ni²+ concentration has dropped to 1.0 × 10-4 M? 4.0 33 X M What is the cell potential at this point? 4.0 0.666 X V

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 galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a solution containing 1.00 M Sn2+ and 1.00 M Sn4+. The other half-cell has a thallium rod immersed in a solution of 1.00 M Tl+. What is the equilibrium constant at 25° C?(Eo= Tl+ / Tl = −0.34 V.)? What is the cell voltage if the Tl+ concentration is increased 6−fold?

A current of 8.86×104 A is passed through an electrolysis cell containing molten KCl for 12.7 days.(a) How many grams of potassium are produced? _________g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? _________L

Predict the products at the anode and the cathode obtained from electrolysis of a 1 M Znl2 solution. Note that 2 H20(1) + 2e → H2(g) + 2 OH(aq) E°red = -0.83 V O2(g) + 4 H*(aq) + 4e¯ → 2 H20(1) I2(s) + 2e → 2 I'(aq) Zn2*(aq) + 2e* → Zn(s) E°re = +1.23 V red E°red = +0.54 V E°, -0.76 V red = (Show work for full or partial credit.) The product at the anode is 12(s). The product at the cathode is Zn(s). The product at the anode is O2(g) and H*(aq). The product at the cathode is Zn(s). None of these The product at the anode is Zn(s). The product at the cathode is O2lg) and H*(aq). The product at the anode is O2lg) and H*(aq). The products at the cathode are H2(g) and OH (aq). The products at the anode are H2(g) and OH"(aq). The product at the cathode is O2(g) and H*(aq). The product at the anode is Zn(s). The product at the cathode is I2(s).

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;