4Cu + Fe(NO3)3 + 6H+ → 4Cu+ + Fe2+ + 3NO2↑ + 3H2O
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- Reaction of and iron(III) nitrate under acidic condition
- 4 + Fe(NO3)3Iron(III) nitrate + 6H+Hydrogen ion4Cu+Copper(I) ion + Fe2+Iron(II) ion + 3NO2↑Nitrogen dioxide + 3H2OWater⟶
The reaction of , iron(III) nitrate, and hydrogen ion yields copper(I) ion, iron(II) ion, nitrogen dioxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and iron(III) nitrate under acidic condition
- 4 + Fe(NO3)3Iron(III) nitrate + 6H+Hydrogen ion4Cu+Copper(I) ion + Fe2+Iron(II) ion + 3NO2↑Nitrogen dioxide + 3H2OWater⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of and iron(III) nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | Reducing | Oxidizable | ||
| Fe(NO3)3 | Iron(III) nitrate | 1 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 6 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu+ | Copper(I) ion | 4 | Oxidized | – |
| Fe2+ | Iron(II) ion | 1 | Reduced | – |
| NO2 | Nitrogen dioxide | 3 | Reduced | – |
| H2O | Water | 3 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and iron(III) nitrate under acidic condition◆
ΔrG −98.1 kJ/mol K 1.54 × 1017 pK −17.19
| 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 | 110.3 | −98.1 | 698.6 | – |
| 27.57 | −24.5 | 174.7 | – | |
per 1 mol of | 110.3 | −98.1 | 698.6 | – |
per 1 mol of Hydrogen ion | 18.38 | −16.3 | 116.4 | – |
per 1 mol of Copper(I) ion | 27.57 | −24.5 | 174.7 | – |
per 1 mol of Iron(II) ion | 110.3 | −98.1 | 698.6 | – |
per 1 mol of | 36.77 | −32.7 | 232.9 | – |
per 1 mol of | 36.77 | −32.7 | 232.9 | – |
Changes in standard condition (2)
- Reaction of and iron(III) nitrate under acidic condition
| 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 | 114.5 | – | – | – |
| 28.63 | – | – | – | |
per 1 mol of | 114.5 | – | – | – |
per 1 mol of Hydrogen ion | 19.08 | – | – | – |
per 1 mol of Copper(I) ion | 28.63 | – | – | – |
per 1 mol of Iron(II) ion | 114.5 | – | – | – |
per 1 mol of | 38.17 | – | – | – |
per 1 mol of | 38.17 | – | – | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 33.150[1] | 24.435[1] |
| (g) | 338.32[1] | 298.58[1] | 166.38[1] | 20.786[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] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):Aqueous solution, (ao):Un-ionized aqueous solution
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 |
|---|---|---|---|---|
| Cu+ (g) | 1089.986[1] | – | – | – |
| Cu+ (ao) | 71.67[1] | 49.98[1] | 40.6[1] | – |
| Fe2+ (g) | 2749.93[1] | – | – | – |
| Fe2+ (ao) | -89.1[1] | -78.90[1] | -137.7[1] | – |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[1] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 33.150 J · K−1 · mol−1
- ^ Cp°, 24.435 J · K−1 · mol−1
- ^ ΔfH°, 338.32 kJ · mol−1
- ^ ΔfG°, 298.58 kJ · mol−1
- ^ S°, 166.38 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ 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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 1089.986 kJ · mol−1
- ^ ΔfH°, 71.67 kJ · mol−1
- ^ ΔfG°, 49.98 kJ · mol−1
- ^ S°, 40.6 J · K−1 · 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°, 33.18 kJ · mol−1
- ^ ΔfG°, 51.31 kJ · mol−1
- ^ S°, 240.06 J · K−1 · mol−1
- ^ Cp°, 37.20 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1