Fe(NO3)3 + e− → Fe2+ + 3NO3−
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- Reduction of iron(III) nitrate
Reduction of iron(III) nitrate yields iron(II) ion and nitrate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of iron(III) nitrate
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of iron(III) nitrate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe(NO3)3 | Iron(III) nitrate | 1 | Oxidizing | – |
e− | Electron | 1 | – | Electron |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe2+ | Iron(II) ion | 1 | Reduced | – |
NO3− | Nitrate ion | 3 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reduction of iron(III) nitrate◆
ΔrG −74.4 kJ/mol K 1.08 × 1013 pK −13.03 - Fe(NO3)3Ionized aqueous solution + e−Fe2+Un-ionized aqueous solution + 3NO3−Un-ionized aqueous solution⟶
Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
---|---|---|---|---|
per 1 mol of Equation | −40.5 | −74.4 | 178.1 | – |
per 1 mol of | −40.5 | −74.4 | 178.1 | – |
per 1 mol of Electron | −40.5 | −74.4 | 178.1 | – |
per 1 mol of Iron(II) ion | −40.5 | −74.4 | 178.1 | – |
per 1 mol of Nitrate ion | −13.5 | −24.8 | 59.37 | – |
Changes in standard condition (2)
- Reduction of iron(III) nitrate
Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
---|---|---|---|---|
per 1 mol of Equation | −36.3 | – | – | – |
per 1 mol of | −36.3 | – | – | – |
per 1 mol of Electron | −36.3 | – | – | – |
per 1 mol of Iron(II) ion | −36.3 | – | – | – |
per 1 mol of Nitrate ion | −12.1 | – | – | – |
Thermodynamic data of reactants
Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
---|---|---|---|---|
Fe(NO3)3 (ai) | -670.7[1] | -338.3[1] | 123.4[1] | – |
Fe(NO3)3 (aq) | -674.9[1] | – | – | – |
Fe(NO3)3 (cr) 9 hydrate | -3285.3[1] | – | – | – |
e− | – | – | – | – |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid
Thermodynamic data of products
Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
---|---|---|---|---|
Fe2+ (g) | 2749.93[1] | – | – | – |
Fe2+ (ao) | -89.1[1] | -78.90[1] | -137.7[1] | – |
NO3− (ao) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
* (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -670.7 kJ · mol−1
- ^ ΔfG°, -338.3 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -674.9 kJ · mol−1
- ^ ΔfH°, -3285.3 kJ · mol−1
- ^ ΔfH°, 2749.93 kJ · mol−1
- ^ ΔfH°, -89.1 kJ · mol−1
- ^ ΔfG°, -78.90 kJ · mol−1
- ^ S°, -137.7 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1