26Cu + Fe2(SO4)3 + 30H+ 🔥→ 26Cu+ + 2Fe2+ + 3H2S↑ + 12H2O
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- Reaction of and iron(III) sulfate under acidic condition
- 26 + Fe2(SO4)3Iron(III) sulfate + 30H+Hydrogen ion26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3H2S↑Hydrogen sulfide + 12H2OWater🔥⟶
The reaction of , iron(III) sulfate, and hydrogen ion yields copper(I) ion, iron(II) ion, hydrogen sulfide, 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) sulfate under acidic condition
- 26 + Fe2(SO4)3Iron(III) sulfate + 30H+Hydrogen ion26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3H2S↑Hydrogen sulfide + 12H2OWater🔥⟶
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) sulfate under acidic condition
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
26 | Reducing | Oxidizable | ||
Fe2(SO4)3 | Iron(III) sulfate | 1 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 30 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cu+ | Copper(I) ion | 26 | Oxidized | – |
Fe2+ | Iron(II) ion | 2 | Reduced | – |
H2S | Hydrogen sulfide | 3 | Reduced | – |
H2O | Water | 12 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 438.3 kJ/mol K 0.16 × 10−76 pK 76.79
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 | 1018.4 | 438.3 | 1946.1 | – |
39.169 | 16.86 | 74.850 | – | |
per 1 mol of | 1018.4 | 438.3 | 1946.1 | – |
per 1 mol of Hydrogen ion | 33.947 | 14.61 | 64.870 | – |
per 1 mol of Copper(I) ion | 39.169 | 16.86 | 74.850 | – |
per 1 mol of Iron(II) ion | 509.20 | 219.2 | 973.05 | – |
per 1 mol of | 339.47 | 146.1 | 648.70 | – |
per 1 mol of | 84.867 | 36.52 | 162.17 | – |
Changes in standard condition (2)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 455.4 kJ/mol K 0.16 × 10−79 pK 79.78
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 | 961.2 | 455.4 | 1692 | – |
36.97 | 17.52 | 65.08 | – | |
per 1 mol of | 961.2 | 455.4 | 1692 | – |
per 1 mol of Hydrogen ion | 32.04 | 15.18 | 56.40 | – |
per 1 mol of Copper(I) ion | 36.97 | 17.52 | 65.08 | – |
per 1 mol of Iron(II) ion | 480.6 | 227.7 | 846.0 | – |
per 1 mol of | 320.4 | 151.8 | 564.0 | – |
per 1 mol of | 80.10 | 37.95 | 141.0 | – |
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] |
Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[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, (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] | – |
H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
H2S (ao) | -39.7[1] | -27.83[1] | 121[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°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 J · K−1 · 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°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. 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