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Problem 48b
Balance the following half-reactions. (b) (basic) CrO42-(aq) → Cr(OH)4-(aq)
Problem 48c
Balance the following half-reactions. (c) (basic) Br3+(aq) → BiO3-(aq)
Problem 48d
Balance the following half-reactions. (d) (basic) ClO-(aq) → Cl-(aq)
Problem 49a
Balance the following half-reactions. (a) (acidic) VO2+(aq) → V3+(aq)
Problem 49b
Balance the following half-reactions. (b) (basic) Ni(OH)2(s) → Ni2O3(s)
Problem 49c
Balance the following half-reactions. (c) (acidic) NO3-(aq) → NO2(aq)
Problem 49d
Balance the following half-reactions. (d) (basic) Br2(aq) → BrO3-(aq)
Problem 50b
Write balanced net ionic equations for the following reactions in acidic solution. (b) TeO2(s) + Cr2+(aq) → Te(s) + Cr3+(aq)
Problem 50c
Write balanced net ionic equations for the following reactions in acidic solution. (c) I-(aq) + IO3-(aq) → I3-(aq)
Problem 51a
Write balanced net ionic equations for the following reactions in acidic solution. (a)
Problem 51b
Write balanced net ionic equations for the following reactions in acidic solution. (b)
Problem 51c
Write balanced net ionic equations for the following reactions in acidic solution. (c)
Problem 52a
Write balanced net ionic equations for the following reactions in basic solution. (a)
Problem 52b
Write balanced net ionic equations for the following reactions in basic solution. (b)
Problem 52c
Write balanced net ionic equations for the following reactions in basic solution. (c)
Problem 53a
Write balanced net ionic equations for the following reactions in basic solution. (a)
Problem 53b
Write balanced net ionic equations for the following reactions in basic solution. (b)
Problem 53c
Write balanced net ionic equations for the following reactions in basic solution. (c)
- Why is the cathode of a galvanic cell considered to be the positive electrode?
Problem 54
- What is the function of a salt bridge in a galvanic cell?
Problem 55
- Describe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b)
Problem 56
- Describe galvanic cells that use the following reactions. In each case, write the anode and cathode half-reactions and sketch the experimental setup. Label the anode and cathode, identify the sign of each electrode, and indicate the direction of electron and ion flow. (b)
Problem 57
- Write a balanced equation for the overall cell reaction in the following galvanic cell, and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br-(aq) | Br2(l2) || Cl2(g) | Cl-(aq) || Pt(s)
Problem 58
- Write the shorthand notation for a galvanic cell that uses the following cell reaction. Include inert electrodes if necessary. 2 Fe1s2 + Cr2O72-1aq2 + 14 H+1aq2¡2 Fe3+1aq2 + 2 Cr3+1aq2 + 7 H2O1l2
Problem 59
Problem 62a
An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.
Problem 62b
An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (b) Write balanced equations for the electrode and overall cell reactions.
Problem 62c
An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (c) Give the shorthand notation for the cell.
- A galvanic cell is constructed from a Zn/Zn2+ half-cell (anode) and a Cl2/Cl- half-cell (cathode). (c) Give the shorthand notation for the cell.
Problem 63
- Write balanced equations for the electrode and overall cell reactions in the following galvanic cells. Sketch each cell, labeling the anode and cathode and showing the direction of electron and ion flow. (a) .
Problem 64
- What conditions must be met for a cell potential E to qualify as a standard cell potential E°?
Problem 66