3H2 + 2Au(OH)3 → 2Au + 6H2O
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- Reaction of and gold(III) hydroxide
The reaction of and gold(III) hydroxide yields and water. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and gold(III) hydroxide
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and gold(III) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reducing | Reducing | ||
| Au(OH)3 | Gold(III) hydroxide | 2 | Oxidizing | Oxidizing |
Products
Thermodynamic changes
Changes in standard condition
- Reaction of and gold(III) hydroxide◆
ΔrG −788.93 kJ/mol K 1.64 × 10138 pK −138.21
| 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 | −865.6 | −788.93 | −256.8 | – |
| −288.5 | −262.98 | −85.60 | – | |
per 1 mol of | −432.8 | −394.46 | −128.4 | – |
| −432.8 | −394.46 | −128.4 | – | |
per 1 mol of | −144.3 | −131.49 | −42.80 | – |
Changes in aqueous solution
- Reaction of and gold(III) hydroxide◆
ΔrG −908.8 kJ/mol K 1.64 × 10159 pK −159.21
| 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 | – | −908.8 | – | – |
| – | −302.9 | – | – | |
per 1 mol of | – | −454.4 | – | – |
| – | −454.4 | – | – | |
per 1 mol of | – | −151.5 | – | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
| Au(OH)3 (cr) precipitated | -424.7[1] | -316.92[1] | 189.5[1] | – |
| Au(OH)3 (ao) | – | -283.37[1] | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 47.40[1] | 25.418[1] |
| (g) | 366.1[1] | 326.3[1] | 180.503[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, (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°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- ^ ΔfH°, -424.7 kJ · mol−1
- ^ ΔfG°, -316.92 kJ · mol−1
- ^ S°, 189.5 J · K−1 · mol−1
- ^ ΔfG°, -283.37 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 47.40 J · K−1 · mol−1
- ^ Cp°, 25.418 J · K−1 · mol−1
- ^ ΔfH°, 366.1 kJ · mol−1
- ^ ΔfG°, 326.3 kJ · mol−1
- ^ S°, 180.503 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