Question

The following shows cell notation of an electrochemical cell: Fe(s) | Fe2+(aq) || NO3-(aq), H+(aq) | NO(g) | Pt(s) a. Write the half-reactions and balanced overall electrochemical reaction of this cell. b. Calculate the standard cell potential (E°) of this cell. c. If you run this cell with 0.050 M of Fe2+, 0.100 M of NO3-, 0.250 M of H+, and 0.010 M of NO, what would be the cell potential of this cell? The following shows oxidation-reduction reactions. Balance the following reactions. a. NO3-(aq) + Sn2+(aq) ? Sn4+(aq) + NO(g) in acidic aqueous solution b. S2O32-(aq) + Cl2(g) ? SO42-(aq) + Cl-(aq) in basic aqueous solution

          The following shows cell notation of an electrochemical cell:
Fe(s) | Fe2+(aq) || NO3-(aq), H+(aq) | NO(g) | Pt(s)
a. Write the half-reactions and balanced overall electrochemical reaction of this cell.
b. Calculate the standard cell potential (E°) of this cell.
c. If you run this cell with 0.050 M of Fe2+, 0.100 M of NO3-, 0.250 M of H+, and 0.010 M of NO, what would be the cell potential of this cell?

The following shows oxidation-reduction reactions. Balance the following reactions.
a. NO3-(aq) + Sn2+(aq) ? Sn4+(aq) + NO(g) in acidic aqueous solution
b. S2O32-(aq) + Cl2(g) ? SO42-(aq) + Cl-(aq) in basic aqueous solution

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The following shows cell notation of an electrochemical cell:
Fe(s) | Fe2+(aq) || NO3-(aq), H+(aq) | NO(g) | Pt(s)
a. Write the half-reactions and balanced overall electrochemical reaction of this cell.
b. Calculate the standard cell potential (E°) of this cell.
c. If you run this cell with 0.050 M of Fe2+, 0.100 M of NO3-, 0.250 M of H+, and 0.010 M of NO, what would be the cell potential of this cell?

The following shows oxidation-reduction reactions. Balance the following reactions.
a. NO3-(aq) + Sn2+(aq) ? Sn4+(aq) + NO(g) in acidic aqueous solution
b. S2O32-(aq) + Cl2(g) ? SO42-(aq) + Cl-(aq) in basic aqueous solution

Added by Gabriel T.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Madhur L

06/05/2023

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Write the half-reactions and balanced overall electrochemical reaction of this cell. Oxidation half-reaction: $\text{Fe}(s) \rightarrow \text{Fe}^{2+}(aq) + 2\text{e}^-$ Reduction half-reaction: $\text{NO}_3^-(aq) + 2\text{H}^+(aq) + \text{e}^- \rightarrow Show more…

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The following shows cell notation of an electrochemical cell: Fe(s) | Fe2+(aq) || NO3-(aq), H+(aq) | NO(g) | Pt(s) a. Write the half-reactions and balanced overall electrochemical reaction of this cell. b. Calculate the standard cell potential (E°) of this cell. c. If you run this cell with 0.050 M of Fe2+, 0.100 M of NO3-, 0.250 M of H+, and 0.010 M of NO, what would be the cell potential of this cell? The following shows oxidation-reduction reactions. Balance the following reactions. a. NO3-(aq) + Sn2+(aq) → Sn4+(aq) + NO(g) in acidic aqueous solution b. S2O32-(aq) + Cl2(g) → SO42-(aq) + Cl-(aq) in basic aqueous solution

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