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General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
- The black silver sulfide discoloration of silverware can be removed by heating the silver article in a sodium carbonate solution in an aluminum pan. The reaction is 3Ag2S(s)+2Al(s)6Ag(s)+3S2(aq)+2Al3+(aq) a. Using data in Appendix 4, calculate G, K, and for the above reaction at 25C. [For Al3+(aq), Gf = 480. kJ/mol.] b. Calculate the value of the standard reduction potential for the following half-reaction: 2e+Ag2S(s)2Ag(s)+S2(aq)arrow_forwardAn aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardThe 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.arrow_forward
- Under standard conditions, what reaction occurs, if any, when each of the following operations is performed? a. Crystals of I2 are added to a solution of NaCl. b. Cl2 gas is bubbled into a solution of NaI. c. A silver wire is placed in a solution of CuCl2 d. An acidic solution of FeSO4 is exposed to air. For the reactions that occur, write a balanced equation and calculate ,G, and K at 25C.arrow_forwardAn aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forwardIf a plating line that deposits nickel (from NiCl2 solutions) operates at a voltage of 0.40 V with a current of 400.0 A and a total mass of 49.0 kg of nickel is deposited, what is the minimum number of kWh consumed in this process?arrow_forward
- Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O 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 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?arrow_forwardConsider 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)arrow_forwardFor each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mg(s)+Ni2+(aq)Mg2+(aq)+Ni(s) (b) 2Ag+(aq)+Cu(s)Cu2+(aq)+2Ag(s) (c) Mn(s)+Sn(NO3)2(aq)Mn(NO3)2(aq)+Sn(s) (d) 3Fe(NO3)2(aq)+Au(NO3)3(aq)3Fe(NO3)3(aq)+Au(s)arrow_forward
- The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)arrow_forwardWhen copper reacts with nitric acid, a mixture of NO(g) and NO2(g) is evolved. The volume ratio of the two product gases depends on the concentration of the nitric acid according to the equilibrium 2H+(aq)+2NO3(aq)+NO(g)3NO2(g)+H2O(l) Consider the following standard reduction potentials at 25C: a. Calculate the equilibrium constant for the above reaction. b. What concentration of nitric acid will produce a NO and NO2 mixture with only 0.20% NO2 (by moles) at 25C and 1.00 atm? Assume that no other gases are present and that the change in acid concentration can be neglected.arrow_forwardConsider 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?arrow_forward
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