2HSCN + 8H2O 💧⚡→ 2H2SO3 + NH4NO2 + 2CH4↑ + H2↑
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- Electrolysis of aqueous thiocyanic acid with water as non-redox agent
Electrolysis of aqueous thiocyanic acid yields sulfurous acid, ammonium nitrite, , 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 thiocyanic acid with water as non-redox agent
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 thiocyanic acid with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSCN | Thiocyanic acid | 2 | Self redox agent | Miscible with water |
| H2O | Water | 8 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2SO3 | Sulfurous acid | 2 | Oxidized | – |
| NH4NO2 | Ammonium nitrite | 1 | Oxidized | – |
| 2 | Reduced | – | ||
| 1 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 423.0 kJ/mol K 0.78 × 10−74 pK 74.11
| 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 | 529.3 | 423.0 | 356.1 | – |
per 1 mol of | 264.6 | 211.5 | 178.1 | – |
per 1 mol of | 66.16 | 52.88 | 44.51 | – |
per 1 mol of | 264.6 | 211.5 | 178.1 | – |
per 1 mol of | 529.3 | 423.0 | 356.1 | – |
| 264.6 | 211.5 | 178.1 | – | |
| 529.3 | 423.0 | 356.1 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 440.6 kJ/mol K 0.65 × 10−77 pK 77.19
| 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 | 525.1 | 440.6 | 802 | – |
per 1 mol of | 262.6 | 220.3 | 401 | – |
per 1 mol of | 65.64 | 55.08 | 100 | – |
per 1 mol of | 262.6 | 220.3 | 401 | – |
per 1 mol of | 525.1 | 440.6 | 802 | – |
| 262.6 | 220.3 | 401 | – | |
| 525.1 | 440.6 | 802 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 455.7 kJ/mol K 0.15 × 10−79 pK 79.84
| 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 | 500.9 | 455.7 | 151.0 | – |
per 1 mol of | 250.4 | 227.8 | 75.50 | – |
per 1 mol of | 62.61 | 56.96 | 18.88 | – |
per 1 mol of | 250.4 | 227.8 | 75.50 | – |
per 1 mol of | 500.9 | 455.7 | 151.0 | – |
| 250.4 | 227.8 | 75.50 | – | |
| 500.9 | 455.7 | 151.0 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 473.3 kJ/mol K 0.12 × 10−82 pK 82.92
| 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 | 496.7 | 473.3 | 597 | – |
per 1 mol of | 248.3 | 236.7 | 299 | – |
per 1 mol of | 62.09 | 59.16 | 74.6 | – |
per 1 mol of | 248.3 | 236.7 | 299 | – |
per 1 mol of | 496.7 | 473.3 | 597 | – |
| 248.3 | 236.7 | 299 | – | |
| 496.7 | 473.3 | 597 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 413.3 kJ/mol K 0.39 × 10−72 pK 72.41
| 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 | – | 413.3 | – | – |
per 1 mol of | – | 206.7 | – | – |
per 1 mol of | – | 51.66 | – | – |
per 1 mol of | – | 206.7 | – | – |
per 1 mol of | – | 413.3 | – | – |
| – | 206.7 | – | – | |
| – | 413.3 | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 430.9 kJ/mol K 0.32 × 10−75 pK 75.49
| 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 | – | 430.9 | – | – |
per 1 mol of | – | 215.4 | – | – |
per 1 mol of | – | 53.86 | – | – |
per 1 mol of | – | 215.4 | – | – |
per 1 mol of | – | 430.9 | – | – |
| – | 215.4 | – | – | |
| – | 430.9 | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 446.0 kJ/mol K 0.73 × 10−78 pK 78.14
| 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 | – | 446.0 | – | – |
per 1 mol of | – | 223.0 | – | – |
per 1 mol of | – | 55.75 | – | – |
per 1 mol of | – | 223.0 | – | – |
per 1 mol of | – | 446.0 | – | – |
| – | 223.0 | – | – | |
| – | 446.0 | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous thiocyanic acid with water as non-redox agent◆
ΔrG 463.6 kJ/mol K 0.60 × 10−81 pK 81.22
| 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 | – | 463.6 | – | – |
per 1 mol of | – | 231.8 | – | – |
per 1 mol of | – | 57.95 | – | – |
per 1 mol of | – | 231.8 | – | – |
per 1 mol of | – | 463.6 | – | – |
| – | 231.8 | – | – | |
| – | 463.6 | – | – |
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 |
|---|---|---|---|---|
| HSCN (ai) | 76.44[1] | 92.71[1] | 144.3[1] | -40.2[1] |
| HSCN (ao) | – | 97.56[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] |
* (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
| NH4NO2 (cr) | -256.5[1] | – | – | – |
| NH4NO2 (ai) | -237.2[1] | -111.6[1] | 236.4[1] | -17.6[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] | – |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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°, 76.44 kJ · mol−1
- ^ ΔfG°, 92.71 kJ · mol−1
- ^ S°, 144.3 J · K−1 · mol−1
- ^ Cp°, -40.2 J · K−1 · mol−1
- ^ ΔfG°, 97.56 kJ · 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°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1
- ^ ΔfH°, -256.5 kJ · mol−1
- ^ ΔfH°, -237.2 kJ · mol−1
- ^ ΔfG°, -111.6 kJ · mol−1
- ^ S°, 236.4 J · K−1 · mol−1
- ^ Cp°, -17.6 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