2Au(OH)3 🔥→ 2Au + 3H2O2
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- Decomposition of gold(III) hydroxide
Decomposition of gold(III) hydroxide yields and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of gold(III) hydroxide
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of gold(III) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Au(OH)3 | Gold(III) hydroxide | 2 | Self redox agent | Thermally decomposable |
Products
Thermodynamic changes
Changes in standard condition
- Decomposition of gold(III) hydroxide◆
ΔrG 272.79 kJ/mol K 0.16 × 10−47 pK 47.79
| 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 | 286.1 | 272.79 | 44.6 | – |
per 1 mol of | 143.1 | 136.40 | 22.3 | – |
| 143.1 | 136.40 | 22.3 | – | |
| 95.37 | 90.930 | 14.9 | – |
Changes in aqueous solution
- Decomposition of gold(III) hydroxide◆
ΔrG 164.65 kJ/mol K 0.14 × 10−28 pK 28.85
| 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 | – | 164.65 | – | – |
per 1 mol of | – | 82.325 | – | – |
| – | 82.325 | – | – | |
| – | 54.883 | – | – |
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 |
|---|---|---|---|---|
| Au(OH)3 (cr) precipitated | -424.7[1] | -316.92[1] | 189.5[1] | – |
| Au(OH)3 (ao) | – | -283.37[1] | – | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 47.40[1] | 25.418[1] |
| (g) | 366.1[1] | 326.3[1] | 180.503[1] | 20.786[1] |
| (l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
| (g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
| (ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ao):Un-ionized aqueous solution
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°, -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°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1