2NH4SCN + 11H2O 💧⚡→ NH4NO3 + 2NH4HSO4 + 2CH4↑ + 4H2↑
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- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
- 2NH4SCNAmmonium thiocyanate + 11H2OWaterNH4NO3Ammonium nitrate + 2NH4HSO4Ammonium hydrogensulfate + 2↑ + 4↑💧⚡⟶
Electrolysis of aqueous ammonium thiocyanate yields ammonium nitrate, ammonium hydrogensulfate, , 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 thiocyanate with water as non-redox agent
- 2NH4SCNAmmonium thiocyanate + 11H2OWaterNH4NO3Ammonium nitrate + 2NH4HSO4Ammonium hydrogensulfate + 2↑ + 4↑💧⚡⟶
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 thiocyanate with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4SCN | Ammonium thiocyanate | 2 | Self redox agent | Very soluble in water |
| H2O | Water | 11 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO3 | Ammonium nitrate | 1 | Oxidized | – |
| NH4HSO4 | Ammonium hydrogensulfate | 2 | Oxidized | – |
| 2 | Reduced | – | ||
| 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
| 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 | 732.4 | – | – | – |
per 1 mol of | 366.2 | – | – | – |
per 1 mol of | 66.58 | – | – | – |
per 1 mol of | 732.4 | – | – | – |
per 1 mol of | 366.2 | – | – | – |
| 366.2 | – | – | – | |
| 183.1 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 619.20 kJ/mol K 0.33 × 10−108 pK 108.48
| 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 | 727.08 | 619.20 | 361.1 | −736.0 |
per 1 mol of | 363.54 | 309.60 | 180.6 | −368.0 |
per 1 mol of | 66.098 | 56.291 | 32.83 | −66.91 |
per 1 mol of | 727.08 | 619.20 | 361.1 | −736.0 |
per 1 mol of | 363.54 | 309.60 | 180.6 | −368.0 |
| 363.54 | 309.60 | 180.6 | −368.0 | |
| 181.77 | 154.80 | 90.28 | −184.0 |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 689.6 kJ/mol K 0.15 × 10−120 pK 120.81
| 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 | 710.3 | 689.6 | 2146 | – |
per 1 mol of | 355.1 | 344.8 | 1073 | – |
per 1 mol of | 64.57 | 62.69 | 195.1 | – |
per 1 mol of | 710.3 | 689.6 | 2146 | – |
per 1 mol of | 355.1 | 344.8 | 1073 | – |
| 355.1 | 344.8 | 1073 | – | |
| 177.6 | 172.4 | 536.5 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 651.98 kJ/mol K 0.60 × 10−114 pK 114.22
| 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 | 698.62 | 651.98 | 155.9 | – |
per 1 mol of | 349.31 | 325.99 | 77.95 | – |
per 1 mol of | 63.511 | 59.271 | 14.17 | – |
per 1 mol of | 698.62 | 651.98 | 155.9 | – |
per 1 mol of | 349.31 | 325.99 | 77.95 | – |
| 349.31 | 325.99 | 77.95 | – | |
| 174.66 | 163.00 | 38.98 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 722.4 kJ/mol K 0.28 × 10−126 pK 126.56
| 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 | 681.8 | 722.4 | 1941 | – |
per 1 mol of | 340.9 | 361.2 | 970.5 | – |
per 1 mol of | 61.98 | 65.67 | 176.5 | – |
per 1 mol of | 681.8 | 722.4 | 1941 | – |
per 1 mol of | 340.9 | 361.2 | 970.5 | – |
| 340.9 | 361.2 | 970.5 | – | |
| 170.4 | 180.6 | 485.3 | – |
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 |
|---|---|---|---|---|
| NH4SCN (cr) | -78.7[1] | – | – | – |
| NH4SCN (ai) | -56.07[1] | 13.40[1] | 257.7[1] | 39.7[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 |
|---|---|---|---|---|
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| NH4HSO4 (cr) | -1026.96[1] | – | – | – |
| NH4HSO4 (ai) | -1019.85[1] | -835.21[1] | 245.2[1] | -3.8[1] |
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ai):Ionized 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°, -78.7 kJ · mol−1
- ^ ΔfH°, -56.07 kJ · mol−1
- ^ ΔfG°, 13.40 kJ · mol−1
- ^ S°, 257.7 J · K−1 · mol−1
- ^ Cp°, 39.7 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°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1
- ^ ΔfH°, -1026.96 kJ · mol−1
- ^ ΔfH°, -1019.85 kJ · mol−1
- ^ ΔfG°, -835.21 kJ · mol−1
- ^ S°, 245.2 J · K−1 · mol−1
- ^ Cp°, -3.8 J · K−1 · mol−1
- ^ ΔfH°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ 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