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문제 48b
Balance the following half-reactions. (b) (basic) CrO42-(aq) → Cr(OH)4-(aq)
문제 48c
Balance the following half-reactions. (c) (basic) Br3+(aq) → BiO3-(aq)
문제 48d
Balance the following half-reactions. (d) (basic) ClO-(aq) → Cl-(aq)
문제 49a
Balance the following half-reactions. (a) (acidic) VO2+(aq) → V3+(aq)
문제 49b
Balance the following half-reactions. (b) (basic) Ni(OH)2(s) → Ni2O3(s)
문제 49c
Balance the following half-reactions. (c) (acidic) NO3-(aq) → NO2(aq)
문제 49d
Balance the following half-reactions. (d) (basic) Br2(aq) → BrO3-(aq)
문제 50b
Write balanced net ionic equations for the following reactions in acidic solution. (b) TeO2(s) + Cr2+(aq) → Te(s) + Cr3+(aq)
문제 50c
Write balanced net ionic equations for the following reactions in acidic solution. (c) I-(aq) + IO3-(aq) → I3-(aq)
문제 51a
Write balanced net ionic equations for the following reactions in acidic solution. (a)
문제 51b
Write balanced net ionic equations for the following reactions in acidic solution. (b)
문제 51c
Write balanced net ionic equations for the following reactions in acidic solution. (c)
문제 52a
Write balanced net ionic equations for the following reactions in basic solution. (a)
문제 52b
Write balanced net ionic equations for the following reactions in basic solution. (b)
문제 52c
Write balanced net ionic equations for the following reactions in basic solution. (c)
문제 53a
Write balanced net ionic equations for the following reactions in basic solution. (a)
문제 53b
Write balanced net ionic equations for the following reactions in basic solution. (b)
문제 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?
문제 54
- What is the function of a salt bridge in a galvanic cell?
문제 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)
문제 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)
문제 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)
문제 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
문제 59
문제 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.
문제 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.
문제 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.
문제 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) .
문제 64
- What conditions must be met for a cell potential E to qualify as a standard cell potential E°?
문제 66