2HSCN + 8H2O 💧⚡→ 2NO↑ + 2H2S↑ + 2H2CO3 + 5H2↑
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- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
- 2HSCNThiocyanic acid + 8H2OWater2NO↑Nitrogen monoxide + 2H2S↑Hydrogen sulfide + 2H2CO3Carbonic acid + 5↑💧⚡⟶
Electrolysis of aqueous thiocyanic acid yields nitrogen monoxide, hydrogen sulfide, carbonic acid, 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 oxidizing agent
- 2HSCNThiocyanic acid + 8H2OWater2NO↑Nitrogen monoxide + 2H2S↑Hydrogen sulfide + 2H2CO3Carbonic acid + 5↑💧⚡⟶
General equation
- Electrolysis of aqueous solution with water as oxidizing agent
- Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSCN | Thiocyanic acid | 2 | Reducing | Miscible with water |
| H2O | Water | 8 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 2 | Oxidized | – |
| H2S | Hydrogen sulfide | 2 | – | – |
| H2CO3 | Carbonic acid | 2 | – | – |
| 5 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 571.43 kJ/mol K 0.78 × 10−100 pK 100.11
| 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 | 873.70 | 571.43 | 1013.4 | – |
per 1 mol of | 436.85 | 285.71 | 506.70 | – |
per 1 mol of | 109.21 | 71.429 | 126.67 | – |
per 1 mol of | 436.85 | 285.71 | 506.70 | – |
per 1 mol of | 436.85 | 285.71 | 506.70 | – |
per 1 mol of | 436.85 | 285.71 | 506.70 | – |
| 174.74 | 114.29 | 202.68 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 659.4 kJ/mol K 0.30 × 10−115 pK 115.52
| 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 | 852.7 | 659.4 | 3245 | – |
per 1 mol of | 426.4 | 329.7 | 1623 | – |
per 1 mol of | 106.6 | 82.42 | 405.6 | – |
per 1 mol of | 426.4 | 329.7 | 1623 | – |
per 1 mol of | 426.4 | 329.7 | 1623 | – |
per 1 mol of | 426.4 | 329.7 | 1623 | – |
| 170.5 | 131.9 | 649.0 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 582.89 kJ/mol K 0.76 × 10−102 pK 102.12
| 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 | 835.6 | 582.89 | 844 | – |
per 1 mol of | 417.8 | 291.44 | 422 | – |
per 1 mol of | 104.5 | 72.861 | 106 | – |
per 1 mol of | 417.8 | 291.44 | 422 | – |
per 1 mol of | 417.8 | 291.44 | 422 | – |
per 1 mol of | 417.8 | 291.44 | 422 | – |
| 167.1 | 116.58 | 169 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 670.9 kJ/mol K 0.29 × 10−117 pK 117.54
| 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 | 814.6 | 670.9 | 3075 | – |
per 1 mol of | 407.3 | 335.4 | 1538 | – |
per 1 mol of | 101.8 | 83.86 | 384.4 | – |
per 1 mol of | 407.3 | 335.4 | 1538 | – |
per 1 mol of | 407.3 | 335.4 | 1538 | – |
per 1 mol of | 407.3 | 335.4 | 1538 | – |
| 162.9 | 134.2 | 615.0 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 561.73 kJ/mol K 0.39 × 10−98 pK 98.41
| 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 | – | 561.73 | – | – |
per 1 mol of | – | 280.87 | – | – |
per 1 mol of | – | 70.216 | – | – |
per 1 mol of | – | 280.87 | – | – |
per 1 mol of | – | 280.87 | – | – |
per 1 mol of | – | 280.87 | – | – |
| – | 112.35 | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 649.7 kJ/mol K 0.15 × 10−113 pK 113.82
| 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 | – | 649.7 | – | – |
per 1 mol of | – | 324.9 | – | – |
per 1 mol of | – | 81.21 | – | – |
per 1 mol of | – | 324.9 | – | – |
per 1 mol of | – | 324.9 | – | – |
per 1 mol of | – | 324.9 | – | – |
| – | 129.9 | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 573.19 kJ/mol K 0.38 × 10−100 pK 100.42
| 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 | – | 573.19 | – | – |
per 1 mol of | – | 286.60 | – | – |
per 1 mol of | – | 71.649 | – | – |
per 1 mol of | – | 286.60 | – | – |
per 1 mol of | – | 286.60 | – | – |
per 1 mol of | – | 286.60 | – | – |
| – | 114.64 | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 661.2 kJ/mol K 0.15 × 10−115 pK 115.84
| 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 | – | 661.2 | – | – |
per 1 mol of | – | 330.6 | – | – |
per 1 mol of | – | 82.65 | – | – |
per 1 mol of | – | 330.6 | – | – |
per 1 mol of | – | 330.6 | – | – |
per 1 mol of | – | 330.6 | – | – |
| – | 132.2 | – | – |
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 |
|---|---|---|---|---|
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (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°, 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°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 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