Back
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 44b,c
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.
b. 2 H+(aq) + Fe(s) → H2(g) + Fe2+(aq)
c. 2 NO3–(aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H2O(l) + 3 Cu2+(aq)
Problem 96b,c
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. b. KCl(aq) c. CuBr2(aq)
- Use line notation to represent each electrochemical cell described in Problem 44.
Problem 5
- The Ksp of Zn(OH)2 is 1.8 * 10^-14. Find Ecell for the half-reaction: Zn(OH)2(s) + 2 e- ⇌ Zn(s) + 2 OH-(aq)
Problem 12
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 39
Balance each redox reaction occurring in acidic aqueous solution. a. PbO2(s) + I–(aq) → Pb2+(aq) + I2(s) b. SO32–(aq) + MnO4–(aq) → SO42–(aq) + Mn2+(aq) c. S2O32–(aq) + Cl2(g) → SO42–(aq) + Cl–(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 41c
Balance each redox reaction occurring in basic aqueous solution. c. Cl2(g) → Cl–(aq) + ClO–(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 43
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. 2 Ag+(aq) + Pb(s) → 2 Ag(s) + Pb2+(aq)
b. 2 ClO2(g) + 2 I–(aq) → 2 ClO2–(aq) + I2(s)
c. O2(g) + 4 H+(aq) + 2 Zn(s) → 2 H2O(l) + 2 Zn2+(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.
- Calculate the standard cell potential for each of the electrochemical cells in Problem 44.
Problem 46
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)
- Is the question formulating correctly? If yes, return the question without changes. If not, please fix it and return the output as a JSON of the form: {'question': 'question text'}. Here is the question: Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell. Mn(s) | Mn2+(aq) || ClO2-(aq) | ClO2(g) | Pt(s)
Problem 52
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)
