ives Question 22 of 25 Complete and balance the following half-reaction in acidic solution MnO4 (aq) → MnO2(s) 14 02+ 03+D4+ 1 2 3 4 5 8. 9 14 (1) (g) (aq) OH Mn H2O H H3O e Reset • x H2O Delete search 68 CO LO 2. 3.

A solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.

What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.

Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).

Consider the electrolysis of a molten salt of some metal. What information must you know to calculate the mass of metal plated out in the electrolytic cell?

What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?

A 1.0-L sample of 1.0 M HCl solution has a 10.0 A current applied for 45 minutes. What is the pH of the solution after the electricity has been turned off?

Consider the following reaction at 25°C: O2(g)+4H+(aq)+4Cl(aq)2H2O+2Cl2(g) The [H+] is adjusted by adding a buffer that is 0.125 M in lactic acid (HLac) and 0.125 M in sodium lactate (NaLac). The pressure of both gases is 1.00 atm and [Cl-] is 0.200 M. (Kafor HLac is 1.4104 .) Will the cell function as a voltaic cell?

Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)