24 Jun 1) Which of the following metals could really
1) Which of the following metals could really be used as sacrificial anodes for iron (Fe2+(aq) + 2e−↔Fe(s), E0 =-0.44V )? A) Tin F) Lead B) Zinc G) Nickel C) Aluminum H) Lithium D) Sodium I) Copper E) Magnesium J) None of the above Enter all that apply in alphabetical order (e.g. AB, ABDF, etc.) 2) A galvanic cell is constructed with a silver-silver chloride electrode, and a nickel strip immersed in a beaker containing 3.97 x 10-2 M solution of NiCl2. Determine the balanced cell reaction and calculate the potential of the cell. Enter in volts. (assume a temperature of 25°C) 3) When Thomas Edison first sold electricity, he used zinc coulometers to measure charge consumption. (In a coulometer the cathode is weighed before a current is passed through it, and then again after the passage of current. The weight increase is proportional to the amount of current that flows through the cathode.) If the zinc plate in one of Edisons coulometers increased in mass by 14.84 g, how much charge had passed through it. Enter in Coulombs. 4) A digital watch battery draws 0.15 milliamperes of current, which is provided by a mercury battery whose net reaction is: HgO(s) + Zn(s) → ZnO(s) + Hg(l) If a partially used battery contains 1.80 g of each of these four substances, for how many hours will the watch continue to run? 5) Consider an electrochemical cell consisting of two vessels connected by a porous separator. One vessel contains 0.750 M HCl solution and an Ag wire electrode coated with AgCl solid. The other vessel contains 2.10 M MgCl2 solution and a Mg wire electrode. First determine the net reaction, and then calculate the emf of this cell. Enter your answer in volts. 6) A “dead” 12-Volt lead/acid storage battery has 8.30 g of PbSO4 (molar mass = 303.3 g), deposited on its electrodes. To recharge it, a “trickle charger” is attached to the Pb anode that supplies 0.140 amperes of current at a voltage of 13.0 V. Calculate how much time it would take to convert all the PbSO4 back into SO42− ions in solution. Enter your answer in hours. 7) How long would it take to electrodeposit all the Cu2+ in 0.400 L of 0.260 M CuSO4 solution with an applied potential difference of 0.265 V and a current of 3.40 amperes? Enter your answer in minutes. 8) Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis apparatus operates at 25.50 A, how many grams of calcium metal will be produced in 36 hours? 9) If the equilibrium constant (Keq) equals 8.61×1012 for the following reaction between strontium and magnesium: Sr(s) + Mg2+(aq)<==> Sr2+(aq) + Mg(s) Calculate Eo for a strontium=magnesium battery. Enter in volts. 10) How much electricity is required to produce a ton of sodium metal in a commercial electrolysis plant? Assume that a ton is 2000 lbs, and that the process is 100% efficient and enter the answer in Coulombs. (One pound = 0.454 kg) 11) A radioactivity counter gives a reading of 350 counts per minute, for a 12.5-mg sample of cobalt(II)chloride, partially enriched with cobalt-60 (half-life = 5.26 yr). What percentage of the cobalt atoms in this sample are cobalt-60
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