For the galvanic cell shown, calculate the standard emf.
Pt(s) l OH-(aq) l O2(g) ll OH-(aq), H2O(l) l H2(g), Pt(s)
Constants:
St. Red. Pot. (V) O2/OH- 0.40 H2O/H2 -0.83
For the galvanic cell shown, calculate the standard emf.
Pt(s) l OH-(aq) l O2(g) ll OH-(aq), H2O(l) l H2(g), Pt(s)
Constants:
| St. Red. Pot. (V) | ||||
|
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Related questions
Please answer all.
1)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Fe2+(aq), Fe3+(aq) ll Hg2+(aq) l Hg(l)
St. Red. Pot. (V)
| Fe3+/Fe2+ | +0.77 |
| Hg2+/Hg | +0.85 |
2)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Fe2+(aq), Fe3+(aq) ll Hg2+(aq) l Hg(l)
| St. Red. Pot. (V) | ||||
|
3)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l SO42-(aq), S2O82-(aq) ll Br2(l) l Br-(aq) l Pt(s)
St. Red. Pot. (V)
| S2O82-/SO42- | +2.01 |
| Br2/Br- | +1.07 |
4)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Pb2+(aq) l PbO2(s) l H+(aq) ll H+(aq) l MnO2(s) l Mn2+(aq) l Pt(s)
St. Red. Pot. (V)
| PbO2/Pb2+ | +1.46 |
| MnO2/Mn2+ | +1.21 |
