2HSCN + 13H2O 💧⚡→ 2SO3 + NH4NO3 + 2CO2↑ + 12H2↑
Last updated:
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
- 2HSCNThiocyanic acid + 13H2OWater2SO3Sulfur trioxide + NH4NO3Ammonium nitrate + 2CO2↑Carbon dioxide + 12↑💧⚡⟶
Electrolysis of aqueous thiocyanic acid yields sulfur trioxide, ammonium nitrate, 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
- 2HSCNThiocyanic acid + 13H2OWater2SO3Sulfur trioxide + NH4NO3Ammonium nitrate + 2CO2↑Carbon dioxide + 12↑💧⚡⟶
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 | 13 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SO3 | Sulfur trioxide | 2 | Oxidized | – |
| NH4NO3 | Ammonium nitrate | 1 | Oxidized | – |
| CO2 | Carbon dioxide | 2 | – | – |
| 12 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1169.56 kJ/mol K 0.13 × 10−204 pK 204.90
| 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 | 1527.00 | 1169.56 | 1199.5 | – |
per 1 mol of | 763.500 | 584.780 | 599.75 | – |
per 1 mol of | 117.462 | 89.9662 | 92.269 | – |
per 1 mol of | 763.500 | 584.780 | 599.75 | – |
per 1 mol of | 1527.00 | 1169.56 | 1199.5 | – |
per 1 mol of | 763.500 | 584.780 | 599.75 | – |
| 127.250 | 97.4633 | 99.958 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1380.8 kJ/mol K 0.12 × 10−241 pK 241.91
| 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 | 1476.6 | 1380.8 | 6555 | – |
per 1 mol of | 738.30 | 690.40 | 3278 | – |
per 1 mol of | 113.58 | 106.22 | 504.2 | – |
per 1 mol of | 738.30 | 690.40 | 3278 | – |
per 1 mol of | 1476.6 | 1380.8 | 6555 | – |
per 1 mol of | 738.30 | 690.40 | 3278 | – |
| 123.05 | 115.07 | 546.3 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1186.32 kJ/mol K 0.15 × 10−207 pK 207.83
| 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 | 1486.42 | 1186.32 | 1007.2 | – |
per 1 mol of | 743.210 | 593.160 | 503.60 | – |
per 1 mol of | 114.340 | 91.2554 | 77.477 | – |
per 1 mol of | 743.210 | 593.160 | 503.60 | – |
per 1 mol of | 1486.42 | 1186.32 | 1007.2 | – |
per 1 mol of | 743.210 | 593.160 | 503.60 | – |
| 123.868 | 98.8600 | 83.933 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1397.5 kJ/mol K 0.15 × 10−244 pK 244.83
| 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 | 1436.0 | 1397.5 | 6363 | – |
per 1 mol of | 718.00 | 698.75 | 3182 | – |
per 1 mol of | 110.46 | 107.50 | 489.5 | – |
per 1 mol of | 718.00 | 698.75 | 3182 | – |
per 1 mol of | 1436.0 | 1397.5 | 6363 | – |
per 1 mol of | 718.00 | 698.75 | 3182 | – |
| 119.67 | 116.46 | 530.3 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1159.86 kJ/mol K 0.63 × 10−203 pK 203.20
| 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 | – | 1159.86 | – | – |
per 1 mol of | – | 579.930 | – | – |
per 1 mol of | – | 89.2200 | – | – |
per 1 mol of | – | 579.930 | – | – |
per 1 mol of | – | 1159.86 | – | – |
per 1 mol of | – | 579.930 | – | – |
| – | 96.6550 | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1371.1 kJ/mol K 0.62 × 10−240 pK 240.21
| 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 | – | 1371.1 | – | – |
per 1 mol of | – | 685.55 | – | – |
per 1 mol of | – | 105.47 | – | – |
per 1 mol of | – | 685.55 | – | – |
per 1 mol of | – | 1371.1 | – | – |
per 1 mol of | – | 685.55 | – | – |
| – | 114.26 | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1176.62 kJ/mol K 0.73 × 10−206 pK 206.13
| 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 | – | 1176.62 | – | – |
per 1 mol of | – | 588.310 | – | – |
per 1 mol of | – | 90.5092 | – | – |
per 1 mol of | – | 588.310 | – | – |
per 1 mol of | – | 1176.62 | – | – |
per 1 mol of | – | 588.310 | – | – |
| – | 98.0517 | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous thiocyanic acid with water as oxidizing agent◆
ΔrG 1387.8 kJ/mol K 0.74 × 10−243 pK 243.13
| 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 | – | 1387.8 | – | – |
per 1 mol of | – | 693.90 | – | – |
per 1 mol of | – | 106.75 | – | – |
per 1 mol of | – | 693.90 | – | – |
per 1 mol of | – | 1387.8 | – | – |
per 1 mol of | – | 693.90 | – | – |
| – | 115.65 | – | – |
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 |
|---|---|---|---|---|
| SO3 (cr) β | -454.51[1] | -374.21[1] | 70.7[1] | – |
| SO3 (l) | -441.04[1] | -373.75[1] | 113.8[1] | – |
| SO3 (g) | -395.72[1] | -371.06[1] | 256.76[1] | 50.67[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] |
| 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, (l):Liquid, (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°, -454.51 kJ · mol−1
- ^ ΔfG°, -374.21 kJ · mol−1
- ^ S°, 70.7 J · K−1 · mol−1
- ^ ΔfH°, -441.04 kJ · mol−1
- ^ ΔfG°, -373.75 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -395.72 kJ · mol−1
- ^ ΔfG°, -371.06 kJ · mol−1
- ^ S°, 256.76 J · K−1 · mol−1
- ^ Cp°, 50.67 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°, -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