SOLVED

41) Which of the following reactions would have the smallest value of K at 298 K? A) A + B → C; E°cell = +1.22 V B) A + 2 B → C; E°cell = +0.98 V C) A + B → 2 C; E°cell = -0.030 V D) A + B → 3 C; E°cell = +0.15 V E) More information is needed to determine. 42) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) A) 1.1 × 1072 B) 8.9 × 10-73 C) 1.1 × 10-72 D) 1.0 × 1024 E) 4.6 × 1031 43) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I?(aq) A) 3.5 × 10-59 B) 1.1 × 1017 C) 6.1 × 1058 D) 8.9 × 10-18 E) 1.7 × 1029 44) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) A) 7.9 × 10-8 B) 8.9 × 107 C) 7.9 × 1015 D) 1.1 × 10-22 E) 1.1 × 10-8 45) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ? Sn2+(aq, 1.8 M) Ag+(aq, 0.055 M) ? Ag(s) A) -0.94 V B) -0.85 V C) +1.02 V D) +0.98 V E) +0.86 V 46) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ? Sn2+(aq, 0.022 M) Ag+(aq, 2.7 M) ? Ag(s) A) +1.01 V B) -0.83 V C) +1.31 V D) +0.01 V E) -0.66 V 47) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ? Mg2+(aq, 2.74 M) Cu2+(aq, 0.0033 M) ? Cu(s) A) -2.80 V B) +2.62 V C) +2.71 V D) +2.12 V E) -1.94 V 48) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Fe(s) ? Fe3+(aq, 0.0011 M) Fe3+(aq, 2.33 M) ? Fe(s) A) +0.066 V B) -0.036 V C) 0.00 V D) -0.099 V E) +0.20 V 49) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mn(s) ? Mn2+(aq, 1.28 M) Ag+(aq, 0.000837 M) ? Ag(s) A) 1.98 V B) -1.28 V C) 0.00 V D) 1.79 V E) -0.84 V 50) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ? Cu2+(aq, 0.0032 M) Cu2+(aq, 4.48 M) ? Cu(s) A) 0.00 V B) +0.093 V C) +0.34 V D) +0.186 V E) +0.052 V