In a dry cell, MnO2 occurs in a semisolid electrolyte paste and is reduced at the cathode. The MnO2 used in dry cells can itself be produced by an electrochemical process of which one half-reaction is shown below. Mn(aq) + 2 H20(/) → MnO2(s) + 4 H*(aq) + 2 e 2+ If a current of 27.5 A is used, how many hours are needed to produce 2.70 kg of MnO2? 4.0 At which electrode is the MnO2 formed? (NOTE: Only ONE submission is allowed for this part of the question.) anode cathode

A galvanic cell is powered by the following redox reaction: 2+ + 3 Cu²+ (aq) + Cr(OH)3(s) + 5OH¯(aq) → 3 Cut (aq) + Cro (aq) + 4H₂O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 0 E = v V ロ→ロ X 5

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

How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 23.2 A is passed through an aqueous solution of CUSO4?