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- Calculate the standard cell potential for each of the electrochemical cells in Problem 44.
Problem 5
- A 0.0251-L sample of a solution of Cu+ requires 0.0322 L of 0.129 M KMnO4 solution to reach the equivalence point. The products of the reaction are Cu2+ and Mn2+. What is the concentration of the Cu+ solution?
Problem 13
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 37c
Balance each redox reaction occurring in acidic aqueous solution. c. BrO3–(aq) + N2H4(g) → Br–(aq) + N2(g)
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 42a
Balance each redox reaction occurring in basic aqueous solution. a. MnO4–(aq) + Br–(aq) → MnO2(s) + BrO3–(aq)
Problem 42c
Balance each redox reaction occurring in basic aqueous solution. c. NO2–(aq) + Al(s) → NH3(g) + AlO2–(aq)
Problem 51d
Consider the voltaic cell:
d. Indicate the direction of anion and cation flow in the salt bridge
Problem 53
Use line notation to represent each electrochemical cell in Problem 43.
- 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 56
Problem 57
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 58
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 59
Which metal could you use to reduce Zn2+ ions but not Al3+ ions?
Problem 60
Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?
Problem 61a
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. Cu
Problem 63a
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. Ag
Problem 65a
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 65b,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 66a,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 66c
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 67
Which metal cation is the best oxidizing agent? a. Zn2+ b. Sn2+ c. Cd2+ d. Ni2+
Problem 69c
Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. c. O2( g) + 2 H2O(l) + 2 Cu(s)¡4 OH-(aq) + 2 Cu2+(aq)
Problem 70a
Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. a. MnO2(s) + 4 H+(aq) + Cu(s)¡Mn2+(aq) + 2 H2O(l) + Cu2+(aq)
Problem 70c
Use tabulated electrode potentials to calculate 𝛥𝐺rxn° for each reaction at 25 °C. c. Br2(l) + 2Cl–(aq) → 2 Br–(aq) + Cl2(g)
Problem 71
Calculate the equilibrium constant for each of the reactions in Problem 70.
- Calculate the equilibrium constant for the reaction between Ni2+(aq) and Cd(s) at 25 °C.
Problem 73
Problem 74
Calculate the equilibrium constant for the reaction between Fe2+(aq) and Zn(s) (at 25 °C).
- Calculate ΔG°_rxn and E°_cell for a redox reaction with n = 2 that has an equilibrium constant of K = 25 (at 25 °C).
Problem 75