12) A container made of steel, having base dimensions of 100 x 150 mm and a wall thiickness of 10 filled to a height of 300 mm with a corrosive liquid. A current is produced due to an electrolytic cell. The current is 0.15 Amp. (Density of Fe: 7.8 g/cm, molecular weight of Fe: 55.85 g/mol, number of electrons transferred: 2) mm is (a) Determine the weight loss of the container after 1 year. (b) Determine the decrease of the container thickness after 1 year.

2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)

75. Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should include a working electrode, a reference electrode, and a counter electrode. (B) The pH meter is unable to determine the pH of 0.1 M NaOH. (C) Silver chloride-coated silver wire is commonly used as a reference electrode in the pH meter. (D) The glass membrane must be hydrated. (E) The difference in potential between the inner and outer layers is the boundary potential.

Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);