Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated steel, a line at a factory operates at a current of 100.0 A for exactly 8 hours on a continuously fed sheet of unplated steel. If the electrolyte contains tin(II) ions, what is the total mass of tin that has plated out in this operation?

When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PbSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 80.0 A is fed into a car battery for 63.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. x10 0.0 X μ 010 3

an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a Zn(NO3)2 solution. When a current of 1.95 A was used, it took exactly 1.7 hours to deposit a 0.0267-mm layer of zinc on the part. What was the total surface area of the part? The density of zinc is 7.410 g/cm^3. Assume the efficiency is 100%. Calculate your answer to at least 2 decimal places.

A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt bridge.  In one beaker, an iron plate was immersed in a 1 M solution of iron(II) nitrate, Fe(NO3)2.  In the other beaker, a lead plate was immersed in a 1 M solution of lead(II) nitrate, Pb(NO3)2.  What voltage is generated by this cell under standard conditions at 25 oC?  Note the following standard half-cell reduction potentials:Fe2+(aq)  +  2e-  ----->  Fe(s)     Eo  =  -0.45 VPb2+(aq)  +  2e-  ----->  Pb(s)     Eo  =  -0.13 V In the voltaic cell described previously, which consists of iron and lead plates, each immersed in a 1 M solution of their respective ions, which beaker contains the anode? Group of answer choices The beaker with the lead plate. The beaker with the iron plate.   Consider again, the voltaic cell described previously, that consists of iron and lead plates, each immersed in a 1 M solution of their respective ions.  Based on the standard cell voltage that…

In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by electrolyzing brine, essentially an aqueous solution of sodium chloride. Suppose a current of 920. A is passed through an aqueous solution of NaCl for 61.0 seconds. Calculate the mass of pure chlorine produced. Be sure your answer has a unit symbol and the correct number of significant digits.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Cu²+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 5.47 M Cu²+ in one half-cell and 2.98 M Zn²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 ロ・ロ X H 00