2) Enter the balanced half reaction that takes place at the cathode for the elec

Question

2) Enter the balanced half reaction that takes place at the cathode for the electrochemical cell shown. Be sure to include electrons.

Pt(s) l F-(aq) l F2(g) ll Cl-(aq), AuCl4-(aq) l Au(s)

+0.99

3) Give the balanced equation with states for both the cathode and the anode reactions of the electrochemical cell shown. Be sure to include electrons in your equations.

Cu(s) l Cu2+(aq) ll Cl-(aq) l AgCl(s), Ag(s)

St. Red. Pot. (V)

Anode reaction:
Cathode reaction:

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 NO(g) l NO3-(aq), H+(aq) ll SO42-(aq), H+(aq) l PbO2(s) l PbSO4(s) l Pt(s)
St. Red. Pot. (V) NO3-/NO +0.96 PbO2/PbSO4 +1.69

2) Enter the balanced half reaction that takes place at the cathode for the electrochemical cell shown. Be sure to include electrons.

Pt(s) l F-(aq) l F2(g) ll Cl-(aq), AuCl4-(aq) l Au(s)

St. Red. Pot. (V) F2/F- +2.87 AuCl4-/Au

+0.99

3) Give the balanced equation with states for both the cathode and the anode reactions of the electrochemical cell shown. Be sure to include electrons in your equations.

Cu(s) l Cu2+(aq) ll Cl-(aq) l AgCl(s), Ag(s)

St. Red. Pot. (V)

Cu2+/Cu +0.34 AgCl/Ag +0.22

Anode reaction:
Cathode reaction:

Explanation / Answer

2NO(G)+3PbO2(s) +4H+(aq)+3SO42-(aq)-------> 2NO3-(aq) + 3PbSO4(s) + 2H2O(l)

2. Au(s) + 4Cl-(aq) + F2(g)-------> AuCl4-(aq) + 2F-

Au (s) + 4Cl- (aq) + F2 (g) -----> AuCl41- (aq) + 2F- (aq)

Au(s) + 4Cl- -------> AuCl4- +3e-oxidation half reaction

F2 + 2e- -----> 2F- reduction half reaction

3. Cu------> Cu+2 +2e-    oxidation half reaction

AgCl+e- ------> Ag + Cl-   reduction half reaction

  

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