2HSCN + 6H2O 💧⚡→ 2S + NH4NO2 + 2CO2↑ + 5H2↑
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- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
Electrolysis of aqueous thiocyanic acid yields , ammonium nitrite, carbon dioxide, 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
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 | 6 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Oxidized | – | ||
| NH4NO2 | Ammonium nitrite | 1 | Oxidized | – |
| CO2 | Carbon dioxide | 2 | – | – |
| 5 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 337.0 kJ/mol K 0.91 × 10−59 pK 59.04
| 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 | 537.9 | 337.0 | 672.8 | −125.3 |
per 1 mol of | 268.9 | 168.5 | 336.4 | −62.65 |
per 1 mol of | 89.65 | 56.17 | 112.1 | −20.88 |
| 268.9 | 168.5 | 336.4 | −62.65 | |
per 1 mol of | 537.9 | 337.0 | 672.8 | −125.3 |
per 1 mol of | 268.9 | 168.5 | 336.4 | −62.65 |
| 107.6 | 67.40 | 134.6 | −25.06 |
Changes in aqueous solution (2)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 425.0 kJ/mol K 0.35 × 10−74 pK 74.46
| 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 | 516.9 | 425.0 | 2904 | – |
per 1 mol of | 258.4 | 212.5 | 1452 | – |
per 1 mol of | 86.15 | 70.83 | 484.0 | – |
| 258.4 | 212.5 | 1452 | – | |
per 1 mol of | 516.9 | 425.0 | 2904 | – |
per 1 mol of | 258.4 | 212.5 | 1452 | – |
| 103.4 | 85.00 | 580.8 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 353.8 kJ/mol K 0.10 × 10−61 pK 61.98
| 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 | 497.3 | 353.8 | 480.6 | – |
per 1 mol of | 248.7 | 176.9 | 240.3 | – |
per 1 mol of | 82.88 | 58.97 | 80.10 | – |
| 248.7 | 176.9 | 240.3 | – | |
per 1 mol of | 497.3 | 353.8 | 480.6 | – |
per 1 mol of | 248.7 | 176.9 | 240.3 | – |
| 99.46 | 70.76 | 96.12 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 441.8 kJ/mol K 0.40 × 10−77 pK 77.40
| 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 | 476.3 | 441.8 | 2712 | – |
per 1 mol of | 238.2 | 220.9 | 1356 | – |
per 1 mol of | 79.38 | 73.63 | 452.0 | – |
| 238.2 | 220.9 | 1356 | – | |
per 1 mol of | 476.3 | 441.8 | 2712 | – |
per 1 mol of | 238.2 | 220.9 | 1356 | – |
| 95.26 | 88.36 | 542.4 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 327.3 kJ/mol K 0.46 × 10−57 pK 57.34
| 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 | – | 327.3 | – | – |
per 1 mol of | – | 163.7 | – | – |
per 1 mol of | – | 54.55 | – | – |
| – | 163.7 | – | – | |
per 1 mol of | – | 327.3 | – | – |
per 1 mol of | – | 163.7 | – | – |
| – | 65.46 | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 415.3 kJ/mol K 0.17 × 10−72 pK 72.76
| 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 | – | 415.3 | – | – |
per 1 mol of | – | 207.7 | – | – |
per 1 mol of | – | 69.22 | – | – |
| – | 207.7 | – | – | |
per 1 mol of | – | 415.3 | – | – |
per 1 mol of | – | 207.7 | – | – |
| – | 83.06 | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 344.1 kJ/mol K 0.52 × 10−60 pK 60.28
| 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 | – | 344.1 | – | – |
per 1 mol of | – | 172.1 | – | – |
per 1 mol of | – | 57.35 | – | – |
| – | 172.1 | – | – | |
per 1 mol of | – | 344.1 | – | – |
per 1 mol of | – | 172.1 | – | – |
| – | 68.82 | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 432.1 kJ/mol K 0.20 × 10−75 pK 75.70
| 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 | – | 432.1 | – | – |
per 1 mol of | – | 216.1 | – | – |
per 1 mol of | – | 72.02 | – | – |
| – | 216.1 | – | – | |
per 1 mol of | – | 432.1 | – | – |
per 1 mol of | – | 216.1 | – | – |
| – | 86.42 | – | – |
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 |
|---|---|---|---|---|
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| NH4NO2 (cr) | -256.5[1] | – | – | – |
| NH4NO2 (ai) | -237.2[1] | -111.6[1] | 236.4[1] | -17.6[1] |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 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°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 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