SOLVED

41) Which of the following metals will not dissolve in nitric acid or hydrochloric acid? A) Al B) Fe C) Mn D) K E) none of the above 42) A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Pb(s) and Pb2+(aq). What species are produced at the electrodes under standard conditions? Ag+(aq) + e- → Ag(s)E° = +0.80 V Pb2+(aq) + 2 e- → Pb(s)E° = -0.13 V A) Ag(aq) is formed at the cathode and, Pb(s) is formed at the anode. B) Ag(s) is formed at the cathode, and Pb2+(aq) is formed at the anode. C) Pb(s) is formed at the cathode, and Ag+(aq) is formed at the anode. D) Pb2+(aq) is formed at the cathode, and Cu(s) is formed at the anode. 43) Consider the following standard reduction potentials, Al3+(aq) + 3 e- → Al(s)E° = -1.66 V I2(s) + 2 e- → 2 I-(aq)E° = +0.54 V Under standard conditions, A) Al3+(aq) is a stronger oxidizing agent than I2(s) and I-(aq) is a stronger reducing agent than Al(s). B) I2(s) is a stronger oxidizing agent than Al3+(aq) and Al(s) is a stronger reducing agent than I-(aq). C) Al(s) is a stronger oxidizing agent than I-(aq) and Al3+(aq) is a stronger reducing agent than I2(s). D) I-(aq) is a stronger oxidizing agent than Al(s) and I2(s) is a stronger reducing agent than Al3+(aq). 44) Consider the galvanic cell, Which one of the following changes to the cell would cause the cell potential to increase (i.e., become more positive)? A) increase the [Zn2+] concentration B) increase the [Pb2+] concentration C) increase the mass of Zn(s) D) decrease the mass of Zn(s) 45) Based on the following information, Br2(l) + 2 e- → 2 Br-(aq)E° = +1.09 V Mg2+(aq) + 2 e- → 2 Mg(s)E° = -2.37 V which of the following chemical species is the strongest reducing agent? A) Br2(l) B) Mg2+(aq) C) Br-(aq) D) Mg(s) 46) A galvanic cell consists of a Al3+/Al half-cell and a standard hydrogen electrode. If the Al3+/Al half-cell standard cell functions as the anode, and the standard cell potential is 1.66 V, what is the standard reduction potential for the Al3+/Al half-cell? A) -1.66 V B) -0.55 V C) +0.55 V D) +1.66 V 47) Using the following standard reduction potentials, Fe3+(aq) + e- →Fe2+(aq)E° = +0.77 V Cu2+(aq) + 2 e- →Cu(s)E° = +0.34 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions. Cu2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Cu(s) A) E° = -0.43 V, nonspontaneous B) E° = -0.43 V, spontaneous C) E° = +0.43 V, nonspontaneous D) E° = +0.43 V, spontaneous 48) Given that E°red = -0.45 V for Fe2+/Fe at 25°C, find E° and E for the concentration cell expressed using shorthand notation below. Fe(s) ? Fe2+(1.0 × 10-5 M) ?? Fe2+(0.100 M) ? Fe(s) A) E° = 0.00 V and E = +0.24 V B) E° = 0.00 V and E = +0.12 V C) E° = -0.45 V and E = -0.21 V D) E° = -0.45 V and E = -0.33 V 49) The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g) With = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.53 V. The concentration of H+ in the cathode compartment is ________ M. A) 1.3 × 10