Consider the electrolysis of molten barium chloride, BaCl₂. a) Write the half-reactions for anode and cathode. b) How many grams of barium metal can be produced by supplying 0.50 A for 30 min?

10. Balance the following redox reaction using the half-reaction method and tell how many electrons are transferred in the reaction. Ag(s) + CN (aq) +O2 (g) → Ag(CN), + H2O (BASIC medium) HINT: CN- is neither oxidized nor reduced

4. In the electrolysis of a sodium chloride solution, what volume of Cl2 (g) is produced in the same time it takes to produce 6.0 L of H2(g), both volumes measured at 0 °C and 1.0 atm?

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.

Balance the following reaction using the half-reaction method, in both acidic and basic conditions. Cr(OH)3 + Br2 → CrO42−+Br− When balanced, determine the entity which is reduced, the entity which is oxidized, the reducing agent and the oxidizing agent.

Be sure to answer all parts. Electrolysis of molten NaCl in a Downs cell is the major isolation step in the production of sodium metal. Assuming that 217 g of Na metal forms, answer the following questions. (a) How many moles of electrons are required? mol e (b) How many coulombs are required? x 100 Enter your answer in scientific notation. (c) How many amps will produce this amount in 9.50 h? A