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Problem 37a,b
Balance each redox reaction occurring in acidic aqueous solution. a. K(s) + Cr3+(aq) → Cr(s) + K+(aq) b. Al(s) + Fe2+(aq) → Al3+(aq) + Fe(s)
Problem 62a,b
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O2(g) + 2 H2O(l) + 4 Ag(s) → 4 OH–(aq) + 4 Ag+(aq) b. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
Problem 65b,c
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. b. Br2(l) + 2 Cl–(aq) → 2 Br–(aq) + Cl2(g) c. MnO2(s) + 4 H+(aq) + Cu(s) → Mn2+(aq) + 2 H2O(l) + Cu2+(aq)
Problem 61b,c
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)
Problem 37c
Balance each redox reaction occurring in acidic aqueous solution. c. BrO3–(aq) + N2H4(g) → Br–(aq) + N2(g)
Problem 38a
Balance each redox reaction occurring in acidic aqueous solution. a. Zn(s) + Sn2+(aq) → Zn2+(aq) + Sn(s)
Problem 38b
Balance each redox reaction occurring in acidic aqueous solution. b. Mg(s) + Cr3+(aq) → Mg2+(aq) + Cr(s)
Problem 38c
Balance each redox reaction occurring in acidic aqueous solution. c. MnO4–(aq) + Al(s) → Mn2+(aq) + Al3+(aq)
Problem 40a
Balance each redox reaction occurring in acidic aqueous solution. a. I–(aq) + NO2–(aq) → I2(s) + NO(g) b. ClO4–(aq) + Cl–(aq) → ClO3–(aq) + Cl2(g)
Problem 40c
Balance each redox reaction occurring in acidic aqueous solution. c. NO3–(aq) + Sn2+(aq) → Sn4+(aq) + NO(g)
Problem 41a
Balance each redox reaction occurring in basic aqueous solution. a. H2O2(aq) + ClO2(aq) → ClO2–(aq) + O2(g)
Problem 41b
Balance each redox reaction occurring in basic aqueous solution. b. Al(s) + MnO4–(aq) → MnO2(s) + Al(OH)4–(aq)
Problem 42a
Balance each redox reaction occurring in basic aqueous solution. a. MnO4–(aq) + Br–(aq) → MnO2(s) + BrO3–(aq)
Problem 42b
Balance each redox reaction occurring in basic aqueous solution. b. Ag(s) + CN–(aq) + O2(g) → Ag(CN)2–(aq)
Problem 42c
Balance each redox reaction occurring in basic aqueous solution. c. NO2–(aq) + Al(s) → NH3(g) + AlO2–(aq)
Problem 44a
Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)
Problem 45
Calculate the standard cell potential for each of the electro- chemical cells in Problem 43.
Problem 47d
Consider the voltaic cell:
d. Indicate the direction of anion and cation flow in the salt bridge
Problem 49
Use line notation to represent each electrochemical cell in Problem 43.
Problem 51
Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell. Sn(s) | Sn2+(aq) || NO(g) | NO3–(aq), H+(aq) | Pt(s)
Problem 53
Determine whether or not each redox reaction occurs spontaneously in the forward direction.
a. Ni(s) + Zn2+(aq) → Ni2+(aq) + Zn(s)
b. Ni(s) + Pb2+(aq) → Ni2+(aq) + Pb(s)
c. Al(s) + 3 Ag+(aq) → Al3+(aq) + 3 Ag(s)
d. Pb(s) + Mn2+(aq) → Pb2+(aq) + Mn(s)
Problem 54
Determine whether or not each redox reaction occurs spontaneously in the forward direction.
a. Ca2+(aq) + Zn(s) → Ca(s) + Zn2+(aq)
b. 2 Ag+(aq) + Ni(s) → 2 Ag(s) + Ni2+(aq)
c. Fe(s) + Mn2+(aq) → Fe2+(aq) + Mn(s)
d. 2 Al(s) + 3 Pb2+(aq) → 2 Al3+(aq) + 3 Pb(s)
Problem 55
Which metal could you use to reduce Mn2+ ions but not Mg2+ ions?
Problem 56
Which metal can be oxidized with an Sn2+ solution but not with an Fe2+ solution?
Problem 57
Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Al b. Ag c. Pb
Problem 59
Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu b. Au
Problem 60
Determine whether or not each metal dissolves in 1 M HIO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au b. Cr
Problem 61a
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn2+(aq) → 2 Cu+(aq) + Mn(s)
Problem 62c
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO2(s) + 4 H+(aq) + Sn(s) → Pb2+(aq) + 2 H2O(l) + Sn2+(aq)
Problem 63
Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+
