Standard reduction potential (E) for reduction of CT_+2) O 7 * 2- to Cr* 3+ is 1.232 V, in acidic medium. 2 If metal rod of Zn, Fe, Au and Ag is provided to you, which metal rod you wouldn't prefer for a spontaneous reduction of CL, O, to Cr in acidic medium. The reduction reactions and standard reduction potential values for Zn, Fe, Au and Ag are as follows: 3 Zn 2+ (aq) + 2e - Zn(s) E deg = -0.7618V 4 Fe 3+ (aq)+3e - Fe(s) E deg = - 0.03V B A'u (aq) +le - Au(s) E deg = 1692V 6 A'g (aq) +le - E deg = 0.7996V 7 Ag(s)

The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V

For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Cu2+(aq)+Ni(s)Cu(s)+Ni2+(aq) (b) 2Ag(s)+Cl2(g)2AgCl(s) (c) Cl2(g)+2I(aq)2Cl(aq)+I2(s)

An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?