Cu + Fe2(SO4)3 + 8H+ 🔥→ Cu2+ + SO2↑ + 2Fe3+ + 4H2O + 2SO3
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- Reaction of and iron(III) sulfate under acidic condition
- + Fe2(SO4)3Iron(III) sulfate + 8H+Hydrogen ionCu2+Copper(II) ion + SO2↑Sulfur dioxide + 2Fe3+Iron(III) ion + 4H2OWater + 2SO3Sulfur trioxide🔥⟶
The reaction of , iron(III) sulfate, and hydrogen ion yields copper(II) ion, sulfur dioxide, iron(III) ion, 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
- + Fe2(SO4)3Iron(III) sulfate + 8H+Hydrogen ionCu2+Copper(II) ion + SO2↑Sulfur dioxide + 2Fe3+Iron(III) ion + 4H2OWater + 2SO3Sulfur 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 |
|---|---|---|---|---|
| 1 | Reducing | Oxidizable | ||
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 8 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu2+ | Copper(II) ion | 1 | Oxidized | – |
| SO2 | Sulfur dioxide | 1 | Reduced | – |
| Fe3+ | Iron(III) ion | 2 | – | – |
| H2O | Water | 4 | – | Water |
| SO3 | Sulfur trioxide | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 301.8 kJ/mol K 0.13 × 10−52 pK 52.87
| 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 | 443.6 | 301.8 | 476.2 | – |
| 443.6 | 301.8 | 476.2 | – | |
per 1 mol of | 443.6 | 301.8 | 476.2 | – |
per 1 mol of Hydrogen ion | 55.45 | 37.73 | 59.52 | – |
per 1 mol of Copper(II) ion | 443.6 | 301.8 | 476.2 | – |
per 1 mol of | 443.6 | 301.8 | 476.2 | – |
per 1 mol of Iron(III) ion | 221.8 | 150.9 | 238.1 | – |
per 1 mol of | 110.9 | 75.45 | 119.0 | – |
per 1 mol of | 221.8 | 150.9 | 238.1 | – |
Changes in standard condition (2)
- Reaction of and iron(III) sulfate under acidic condition◆
ΔrG 301.3 kJ/mol K 0.16 × 10−52 pK 52.79
| 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 | 417.5 | 301.3 | 389.9 | – |
| 417.5 | 301.3 | 389.9 | – | |
per 1 mol of | 417.5 | 301.3 | 389.9 | – |
per 1 mol of Hydrogen ion | 52.19 | 37.66 | 48.74 | – |
per 1 mol of Copper(II) ion | 417.5 | 301.3 | 389.9 | – |
per 1 mol of | 417.5 | 301.3 | 389.9 | – |
per 1 mol of Iron(III) ion | 208.8 | 150.7 | 194.9 | – |
per 1 mol of | 104.4 | 75.33 | 97.47 | – |
per 1 mol of | 208.8 | 150.7 | 194.9 | – |
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] | – |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[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, (l):Liquid, (cr):Crystalline solid
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°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, 5712.8 kJ · mol−1
- ^ ΔfH°, -48.5 kJ · mol−1
- ^ ΔfG°, -4.7 kJ · mol−1
- ^ S°, -315.9 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