5. A spontaneous reaction would occur between Fe (aq) solution and: A. 1(s) B. Zn(s) C. Hg(1) D. Fe (aq) 6. One reason that copper pipes rather than iron pipes are used in household plumbing is that: A. Iron has a greater tendency to be oxidized than copper. B. Iron will react with dissolved minerals such as calcium salts. C. Copper is a better conductor of heat energy than iron. D. Commercial drain cleaners containing sodium hydroxide will react with iron.

5. A spontaneous reaction would occur between Fe (aq) solution and: A. 1(s) B. Zn(s) C. Hg(1) D. Fe (aq) 6. One reason that copper pipes rather than iron pipes are used in household plumbing is that: A. Iron has a greater tendency to be oxidized than copper. B. Iron will react with dissolved minerals such as calcium salts. C. Copper is a better conductor of heat energy than iron. D. Commercial drain cleaners containing sodium hydroxide will react with iron.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 73QAP: Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table...

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The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4 ions by periodate ion (IO4) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate and G at 25C for each reaction.
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
Electrochemical Cells II Consider this cell running under standard conditions: Ni(s)Ni2(aq)Cu+(aq)Cu(s) a Is this cell a voltaic or an electrolytic cell? How do you know? b Does current flow in this cell spontaneously? c What is the maximum cell potential for this cell? d Say the cell is connected to a voltmeter. Describe what you might see for an initial voltage and what voltage changes, if any, you would observe as time went by. e What is the free energy of this cell when it is first constructed? f Does the free energy of the cell change over time as the cell runs? If so, how does it change?
Use the data in Appendix L to determine the equilibrium constant for the following reactions. Assume 298.15 K if no temperature is given. (a) AgCl(s)Ag+(aq)+Cl(aq) (b) CdS(s)Cd2+(aq)+S2(aq) t 377 k (c) Hg2+(aq)+4Br(aq)[HgBr4]2(aq) (d) H2O(l)H+(aq)+OH(aq) at 25 C
The free energy change for a reaction, G, is an extensive property. What is an extensive property? Surprisingly, one can calculate G from the cell potential. , for the reaction. This is surprising because : is an intensive property. How can the extensive property G be calculated from the intensive property ?
Calculate G and K at 25C for the reactions in Exercises 38 and 42.
Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
Calculate the standard free energy change for the following reactions using the standard cell potentials for the half-reactions that are involved. (a) Fe(s)+Hg22+(aq)Fe2+(aq)+2Hg(l) (b Fe3+(aq)+Ag(s)+Cl-(aq)Fe2+(aq)+AgCl(s) (c) 2MnO4(aq)+5Zn(s)+16H3O+(aq)2Mn2+(aq)+5Zn2+(aq)+24H2O(l)
The overall reaction in the lead storage battery is Pb(s)+PbO2(s)+2H+(aq)+2HSO4(aq)2PbSO4(s)+2H2O(l) a. For the cell reaction H = 315.9 kJ and S = 263.5 J/K. Calculate at 20.C. Assume H and S do not depend on temperature. b. Calculate at 20.C when [HSO4] = [H+] = 4.5 M. c. Consider your answer to Exercise 71. Why does it seem that batteries fail more often on cold days than on warm days?