36Cu + 8Fe2(SO4)3 + 104H+ 🔥→ 36Cu2+ + 16Fe2+ + 7H2S↑ + 45H2O + 17SO3
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- Reaction of and iron(III) sulfate under acidic condition
- 36 + 8Fe2(SO4)3Iron(III) sulfate + 104H+Hydrogen ion36Cu2+Copper(II) ion + 16Fe2+Iron(II) ion + 7H2S↑Hydrogen sulfide + 45H2OWater + 17SO3Sulfur trioxide🔥⟶
The reaction of , iron(III) sulfate, and hydrogen ion yields copper(II) ion, iron(II) ion, hydrogen sulfide, water, and sulfur trioxide (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
- 36 + 8Fe2(SO4)3Iron(III) sulfate + 104H+Hydrogen ion36Cu2+Copper(II) ion + 16Fe2+Iron(II) ion + 7H2S↑Hydrogen sulfide + 45H2OWater + 17SO3Sulfur trioxide🔥⟶
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 |
|---|---|---|---|---|
| 36 | Reducing | Oxidizable | ||
| Fe2(SO4)3 | Iron(III) sulfate | 8 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 104 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu2+ | Copper(II) ion | 36 | Oxidized | – |
| Fe2+ | Iron(II) ion | 16 | Reduced | – |
| H2S | Hydrogen sulfide | 7 | Reduced | – |
| H2O | Water | 45 | – | Water |
| SO3 | Sulfur trioxide | 17 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 1770.3 kJ/mol K 0.72 × 10−310 pK 310.14
| 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 | 2772.7 | 1770.3 | 3378.2 | – |
| 77.019 | 49.175 | 93.839 | – | |
per 1 mol of | 346.59 | 221.29 | 422.27 | – |
per 1 mol of Hydrogen ion | 26.661 | 17.022 | 32.483 | – |
per 1 mol of Copper(II) ion | 77.019 | 49.175 | 93.839 | – |
per 1 mol of Iron(II) ion | 173.29 | 110.64 | 211.14 | – |
per 1 mol of | 396.10 | 252.90 | 482.60 | – |
per 1 mol of | 61.616 | 39.340 | 75.071 | – |
per 1 mol of | 163.10 | 104.14 | 198.72 | – |
Changes in standard condition (2)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 1810.5 kJ/mol K 0.65 × 10−317 pK 317.19
| 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 | 2639.2 | 1810.5 | 2785 | – |
| 73.311 | 50.292 | 77.36 | – | |
per 1 mol of | 329.90 | 226.31 | 348.1 | – |
per 1 mol of Hydrogen ion | 25.377 | 17.409 | 26.78 | – |
per 1 mol of Copper(II) ion | 73.311 | 50.292 | 77.36 | – |
per 1 mol of Iron(II) ion | 164.95 | 113.16 | 174.1 | – |
per 1 mol of | 377.03 | 258.64 | 397.9 | – |
per 1 mol of | 58.649 | 40.233 | 61.89 | – |
per 1 mol of | 155.25 | 106.50 | 163.8 | – |
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 |
|---|---|---|---|---|
| Cu2+ (g) | 3054.07[1] | – | – | – |
| Cu2+ (ao) | 64.77[1] | 65.49[1] | -99.6[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] |
| SO3 (cr) β | -454.51[1] | -374.21[1] | 70.7[1] | – |
| SO3 (l) | -441.04[1] | -373.75[1] | 113.8[1] | – |
| SO3 (g) | -395.72[1] | -371.06[1] | 256.76[1] | 50.67[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°, 3054.07 kJ · mol−1
- ^ ΔfH°, 64.77 kJ · mol−1
- ^ ΔfG°, 65.49 kJ · mol−1
- ^ S°, -99.6 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
- ^ ΔfH°, -454.51 kJ · mol−1
- ^ ΔfG°, -374.21 kJ · mol−1
- ^ S°, 70.7 J · K−1 · mol−1
- ^ ΔfH°, -441.04 kJ · mol−1
- ^ ΔfG°, -373.75 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -395.72 kJ · mol−1
- ^ ΔfG°, -371.06 kJ · mol−1
- ^ S°, 256.76 J · K−1 · mol−1
- ^ Cp°, 50.67 J · K−1 · mol−1