Molecular chlorine and iodine are available to carry out the processes indicated in sections a) and b). Explain which of these two substances could be used in each case, which half-reactions would occur, the overall reaction and what would be the potential of the reactions to:
A) Get Ag + from Ag.
B) Obtain Br2 from Br-. Data.E0 (Cl2 / Cl-) = 1.36 V; E0 (Br2 / Br-) = 1.06 V; E0 (I2 / I-) = 0.53 V; E0 (Ag + / Ag) = 0,80 V.
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Molecular chlorine and iodine are available to carry out the processes
indicated in sections a) and b). Explain which of these two substances could
be used in each case, which reactions would take place, the overall reaction
and what would be the potential of reactions to:
A) Obtain Ag⁺ from Ag.
For a redox process to be spontaneous, the reaction potential must be
positive. To oxidize the silver, a reduction reaction with a potential greater
than 0.80 v is needed.
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction reaction reduction: 2 × (Ag → Ag⁺ + 1e⁻) E ° = -0.80 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.56 v
b) Get Br₂ from Br⁻
To oxidize the bromide ion to molecular bromine, a reduction is required
whose potential is greater than 1.06 v
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction half-reaction: 2Br⁻ → Br₂ + 2e⁻) E ° = -1.06 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.30 v
indicated in sections a) and b). Explain which of these two substances could
be used in each case, which reactions would take place, the overall reaction
and what would be the potential of reactions to:
A) Obtain Ag⁺ from Ag.
For a redox process to be spontaneous, the reaction potential must be
positive. To oxidize the silver, a reduction reaction with a potential greater
than 0.80 v is needed.
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction reaction reduction: 2 × (Ag → Ag⁺ + 1e⁻) E ° = -0.80 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.56 v
b) Get Br₂ from Br⁻
To oxidize the bromide ion to molecular bromine, a reduction is required
whose potential is greater than 1.06 v
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction half-reaction: 2Br⁻ → Br₂ + 2e⁻) E ° = -1.06 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.30 v
Answered by
1
Molecular chlorine and iodine are available to carry out the processes
indicated in sections a) and b). Explain which of these two substances could
be used in each case, which reactions would take place, the overall reaction
and what would be the potential of reactions to:
A) Obtain Ag⁺ from Ag.
For a redox process to be spontaneous, the reaction potential must be
positive. To oxidize the silver, a reduction reaction with a potential greater
than 0.80 v is needed.
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction reaction reduction: 2 × (Ag → Ag⁺ + 1e⁻) E ° = -0.80 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.56 v
b) Get Br₂ from Br⁻
To oxidize the bromide ion to molecular bromine, a reduction is required
whose potential is greater than 1.06 v
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction half-reaction: 2Br⁻ → Br₂ + 2e⁻) E ° = -1.06 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.30
indicated in sections a) and b). Explain which of these two substances could
be used in each case, which reactions would take place, the overall reaction
and what would be the potential of reactions to:
A) Obtain Ag⁺ from Ag.
For a redox process to be spontaneous, the reaction potential must be
positive. To oxidize the silver, a reduction reaction with a potential greater
than 0.80 v is needed.
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction reaction reduction: 2 × (Ag → Ag⁺ + 1e⁻) E ° = -0.80 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.56 v
b) Get Br₂ from Br⁻
To oxidize the bromide ion to molecular bromine, a reduction is required
whose potential is greater than 1.06 v
Oxidation semi-reaction: Cl₂ + 2e⁻ → 2Cl⁻ E ° = 1.36 v
Reduction half-reaction: 2Br⁻ → Br₂ + 2e⁻) E ° = -1.06 v
Cl₂ + 2Ag → 2Cl⁻ + 2Ag⁺ E ° = 0.30
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