10Cu + Ag2SO4 + 8H+ 🔥→ Cu2S + 8Cu+ + 2Ag + 4H2O
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- Reaction of and silver(I) sulfate under acidic condition
- 10 + Ag2SO4Silver(I) sulfate + 8H+Hydrogen ionCu2SCopper(I) sulfide + 8Cu+Copper(I) ion + 2 + 4H2OWater🔥⟶
The reaction of , silver(I) sulfate, and hydrogen ion yields copper(I) sulfide, copper(I) ion, , 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 silver(I) sulfate under acidic condition
- 10 + Ag2SO4Silver(I) sulfate + 8H+Hydrogen ionCu2SCopper(I) sulfide + 8Cu+Copper(I) ion + 2 + 4H2OWater🔥⟶
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 silver(I) sulfate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 10 | Reducing | Oxidizable | ||
| Ag2SO4 | Silver(I) sulfate | 1 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 8 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu2S | Copper(I) sulfide | 1 | Redoxed product | – |
| Cu+ | Copper(I) ion | 8 | Oxidized | – |
| 2 | Reduced | – | ||
| H2O | Water | 4 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of and silver(I) sulfate under acidic condition◆
ΔrG −44.6 kJ/mol K 6.51 × 107 pK −7.81
| 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 | 48.6 | −44.6 | 313.2 | – |
| 4.86 | −4.46 | 31.32 | – | |
per 1 mol of | 48.6 | −44.6 | 313.2 | – |
per 1 mol of Hydrogen ion | 6.08 | −5.58 | 39.15 | – |
per 1 mol of | 48.6 | −44.6 | 313.2 | – |
per 1 mol of Copper(I) ion | 6.08 | −5.58 | 39.15 | – |
| 24.3 | −22.3 | 156.6 | – | |
per 1 mol of | 12.2 | −11.2 | 78.30 | – |
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] |
| Ag2SO4 (cr) | -715.88[1] | -618.41[1] | 200.4[1] | 131.38[1] |
| Ag2SO4 (ai) | -698.10[1] | -590.30[1] | 165.7[1] | -251[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 |
|---|---|---|---|---|
| Cu2S (cr) α | -79.5[1] | -86.2[1] | 120.9[1] | 76.32[1] |
| Cu+ (g) | 1089.986[1] | – | – | – |
| Cu+ (ao) | 71.67[1] | 49.98[1] | 40.6[1] | – |
| (cr) | 0[1] | 0[1] | 42.55[1] | 25.351[1] |
| (g) | 284.55[1] | 245.65[1] | 172.997[1] | 20.786[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] |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -715.88 kJ · mol−1
- ^ ΔfG°, -618.41 kJ · mol−1
- ^ S°, 200.4 J · K−1 · mol−1
- ^ Cp°, 131.38 J · K−1 · mol−1
- ^ ΔfH°, -698.10 kJ · mol−1
- ^ ΔfG°, -590.30 kJ · mol−1
- ^ S°, 165.7 J · K−1 · mol−1
- ^ Cp°, -251. 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°, -79.5 kJ · mol−1
- ^ ΔfG°, -86.2 kJ · mol−1
- ^ S°, 120.9 J · K−1 · mol−1
- ^ Cp°, 76.32 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 42.55 J · K−1 · mol−1
- ^ Cp°, 25.351 J · K−1 · mol−1
- ^ ΔfH°, 284.55 kJ · mol−1
- ^ ΔfG°, 245.65 kJ · mol−1
- ^ S°, 172.997 J · K−1 · mol−1
- ^ Cp°, 20.786 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