What is the electrode potential of mercury?
Standard Electrode Potentials in Aqueous Solution at 25°C
| Cathode (Reduction) Half-Reaction | Standard Potential E° (volts) |
|---|---|
| Ag+(aq) + e- -> Ag(s) | 0.80 |
| Hg2+(aq) + 2e- -> Hg(l) | 0.85 |
| ClO-(aq) + H2O(l) + 2e- -> Cl-(aq) + 2OH-(aq) | 0.90 |
| 2Hg2+(aq) + 2e- -> Hg22+(aq) | 0.90 |
What is the reduction potential of mercury?
P1: Standard Reduction Potentials by Element
| Mercury | E° (V) |
|---|---|
| Hg22+ + 2e− ⇌ 2Hg(l) | 0.7960 |
| Hg2Cl2(s) + 2e− ⇌ 2Hg(l) + 2Cl− | 0.2682 |
| HgO(s) + 2H+ + 2e− ⇌ Hg(l) + H2O(l) | 0.926 |
| Hg2Br2(s) + 2e− ⇌ 2Hg(l) + 2Br− | 1.392 |
What is the reduction potential of palladium?
| Standard Reduction Potentials in Aqueous Solution at 25oC | |
|---|---|
| Acidic Solution | Eo (V) |
| Pd2+(aq) + 2e– Pd(s) | +0.987 |
| NO3–(aq) + 4H+(aq) + 3e– NO(g) + 2H2O | +0.96 |
| NO3–(aq) + 3H+(aq) + 2e– HNO2(aq) + H2O | +0.94 |
How is EO calculated?
Determine Ecell, the cell potential at the non-standard state conditions using the Nernst equation….
| oxidation: | 4 Br-(aq) 2 Br2(l) + 4 e- | Eoox. = – Eored. = – (+ 1.077 V) = – 1.077 V |
|---|---|---|
| reduction: | O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) | Eored. = + 1.229 V |
| overall: | O2(g) + 4 H+(aq) + 4 Br-(aq) 2 H2O(l) + 2 Br2(l) | Eocell = + 0.152 V |
Can cell potential negative?
The standard cell potential is quite negative, so the reaction will not occur spontaneously as written.
How do we calculate cell potential?
The overall cell potential can be calculated by using the equation E0cell=E0red−E0oxid. Step 2: Solve. Before adding the two reactions together, the number of electrons lost in the oxidation must equal the number of electrons gained in the reduction. The silver half-cell reaction must be multiplied by two.
What does higher reduction potential mean?
A solution with a higher (more positive) reduction potential than the new species will have a tendency to gain electrons from the new species (i.e. to be reduced by oxidizing the new species) and a solution with a lower (more negative) reduction potential will have a tendency to lose electrons to the new species (i.e. …
Which element has highest reduction potential?
Fluorine gas
Fluorine gas is one of the best oxidizing agents there are and it is at the top of the table with the biggest most positive standard potential (+2.87 V). Reducing Agents: At the other end, are reactions with negative standard potentials.
What does it mean when a cell potential is negative?
reducing environment
A negative value of cell potential indicates a reducing environment, while a positive value indicates an oxidizing environment.
What is the difference between oxidation potential and reduction potential?
The key difference between oxidation potential and reduction potential is that oxidation potential indicates the tendency of a chemical element to be oxidized. In contrast, reduction potential indicates the tendency of a chemical element to be reduced.
Does cell potential have to be positive?
A positive E°cell means that the reaction will occur spontaneously as written. A negative E°cell means that the reaction will proceed spontaneously in the opposite direction….Calculating Standard Cell Potentials.
| Half-Reaction | E° (V) |
|---|---|
| H2O2(aq) + 2H+(aq) + 2e− ⇌ 2H2O(l) | 1.763 |
| F2(g) + 2e−⇌ 2F−(aq) | 2.87 |
How do you calculate redox potential?
The minus sign is necessary because oxidation is the reverse of reduction. Figure 3. A galvanic cell can be used to determine the standard reduction potential of Cu2+….Learning Objectives.
| Table 1. Selected Standard Reduction Potentials at 25 °C | |
|---|---|
| Half-Reaction | E° (V) |
| Fe3+(aq)+e−⟶Fe2+(aq) | +0.771 |