3(NH4)2Cr2O7 + 6H2O 💧⚡→ 6NH2OH + 6Cr(OH)3 + O3↑
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- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
- 3(NH4)2Cr2O7Ammonium dichromate + 6H2OWater6NH2OHHydroxylamine + 6Cr(OH)3Chromium(III) hydroxide + ↑💧⚡⟶
Electrolysis of aqueous ammonium dichromate yields hydroxylamine, chromium(III) hydroxide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
- 3(NH4)2Cr2O7Ammonium dichromate + 6H2OWater6NH2OHHydroxylamine + 6Cr(OH)3Chromium(III) hydroxide + ↑💧⚡⟶
General equation
- Electrolysis of aqueous solution with water as non redox agent
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
(NH4)2Cr2O7 | Ammonium dichromate | 3 | Self redox agent | Very soluble in water |
H2O | Water | 6 | – | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH2OH | Hydroxylamine | 6 | Oxidized | – |
Cr(OH)3 | Chromium(III) hydroxide | 6 | Reduced | – |
1 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
- 3(NH4)2Cr2O7Crystalline solid + 6H2OLiquid6NH2OHCrystalline solid + 6Cr(OH)3Crystalline solidprecipitated + ↑Gas💧⚡⟶
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 | 208.6 | – | – | – |
per 1 mol of | 69.53 | – | – | – |
per 1 mol of | 34.77 | – | – | – |
per 1 mol of Hydroxylamine | 34.77 | – | – | – |
per 1 mol of | 34.77 | – | – | – |
208.6 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
- 3(NH4)2Cr2O7Ionized aqueous solution + 6H2OLiquid6NH2OHAqueous solution + 6Cr(OH)3Crystalline solidprecipitated + ↑Gas💧⚡⟶
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 | 149.5 | – | – | – |
per 1 mol of | 49.83 | – | – | – |
per 1 mol of | 24.92 | – | – | – |
per 1 mol of Hydroxylamine | 24.92 | – | – | – |
per 1 mol of | 24.92 | – | – | – |
149.5 | – | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium dichromate with water as non-redox agent
- 3(NH4)2Cr2O7Ionized aqueous solution + 6H2OLiquid6NH2OHAqueous solution + 6Cr(OH)3Crystalline solidprecipitated + ↑Un-ionized aqueous solution💧⚡⟶
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 | 132.7 | – | – | – |
per 1 mol of | 44.23 | – | – | – |
per 1 mol of | 22.12 | – | – | – |
per 1 mol of Hydroxylamine | 22.12 | – | – | – |
per 1 mol of | 22.12 | – | – | – |
132.7 | – | – | – |
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 |
---|---|---|---|---|
(NH4)2Cr2O7 (cr) | -1806.7[1] | – | – | – |
(NH4)2Cr2O7 (ai) | -1755.2[1] | -1459.5[1] | 488.7[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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 |
---|---|---|---|---|
NH2OH (cr) | -114.2[1] | – | – | – |
NH2OH (aq) | -98.3[1] | – | – | – |
Cr(OH)3 (cr) precipitated | -1064.0[1] | – | – | – |
(g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
(ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (g):Gas, (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°, -1806.7 kJ · mol−1
- ^ ΔfH°, -1755.2 kJ · mol−1
- ^ ΔfG°, -1459.5 kJ · mol−1
- ^ S°, 488.7 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°, -114.2 kJ · mol−1
- ^ ΔfH°, -98.3 kJ · mol−1
- ^ ΔfH°, -1064.0 kJ · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1