NH4SCN + 2H2O 💧⚡→ NH4CN + SO2↑ + 2H2↑
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- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
Electrolysis of aqueous ammonium thiocyanate yields ammonium cyanide, sulfur 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 ammonium thiocyanate 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 ammonium thiocyanate with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4SCN | Ammonium thiocyanate | 1 | Self redox agent | Very soluble in water |
| H2O | Water | 2 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4CN | Ammonium cyanide | 1 | Reduced | – |
| SO2 | Sulfur dioxide | 1 | Oxidized | – |
| 2 | – | – |
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 | 354.0 | – | – | – |
per 1 mol of | 354.0 | – | – | – |
per 1 mol of | 177.0 | – | – | – |
per 1 mol of | 354.0 | – | – | – |
per 1 mol of | 354.0 | – | – | – |
| 177.0 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 253.7 kJ/mol K 0.36 × 10−44 pK 44.45
| 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 | 348.9 | 253.7 | 319.6 | – |
per 1 mol of | 348.9 | 253.7 | 319.6 | – |
per 1 mol of | 174.4 | 126.8 | 159.8 | – |
per 1 mol of | 348.9 | 253.7 | 319.6 | – |
per 1 mol of | 348.9 | 253.7 | 319.6 | – |
| 174.4 | 126.8 | 159.8 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 288.9 kJ/mol K 0.24 × 10−50 pK 50.61
| 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 | 340.5 | 288.9 | 1212 | – |
per 1 mol of | 340.5 | 288.9 | 1212 | – |
per 1 mol of | 170.3 | 144.4 | 606.0 | – |
per 1 mol of | 340.5 | 288.9 | 1212 | – |
per 1 mol of | 340.5 | 288.9 | 1212 | – |
| 170.3 | 144.4 | 606.0 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 253.2 kJ/mol K 0.44 × 10−44 pK 44.36
| 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 | 322.8 | 253.2 | 233.2 | – |
per 1 mol of | 322.8 | 253.2 | 233.2 | – |
per 1 mol of | 161.4 | 126.6 | 116.6 | – |
per 1 mol of | 322.8 | 253.2 | 233.2 | – |
per 1 mol of | 322.8 | 253.2 | 233.2 | – |
| 161.4 | 126.6 | 116.6 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 288.4 kJ/mol K 0.30 × 10−50 pK 50.53
| 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 | 314.4 | 288.4 | 1126 | – |
per 1 mol of | 314.4 | 288.4 | 1126 | – |
per 1 mol of | 157.2 | 144.2 | 563.0 | – |
per 1 mol of | 314.4 | 288.4 | 1126 | – |
per 1 mol of | 314.4 | 288.4 | 1126 | – |
| 157.2 | 144.2 | 563.0 | – |
Changes in aqueous solution (5)
- 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 | 363.1 | – | – | – |
per 1 mol of | 363.1 | – | – | – |
per 1 mol of | 181.6 | – | – | – |
per 1 mol of | 363.1 | – | – | – |
per 1 mol of | 363.1 | – | – | – |
| 181.6 | – | – | – |
Changes in aqueous solution (6)
- 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 | 354.7 | – | – | – |
per 1 mol of | 354.7 | – | – | – |
per 1 mol of | 177.3 | – | – | – |
per 1 mol of | 354.7 | – | – | – |
per 1 mol of | 354.7 | – | – | – |
| 177.3 | – | – | – |
Changes in aqueous solution (7)
- 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 | 337.0 | – | – | – |
per 1 mol of | 337.0 | – | – | – |
per 1 mol of | 168.5 | – | – | – |
per 1 mol of | 337.0 | – | – | – |
per 1 mol of | 337.0 | – | – | – |
| 168.5 | – | – | – |
Changes in aqueous solution (8)
- 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 | 328.6 | – | – | – |
per 1 mol of | 328.6 | – | – | – |
per 1 mol of | 164.3 | – | – | – |
per 1 mol of | 328.6 | – | – | – |
per 1 mol of | 328.6 | – | – | – |
| 164.3 | – | – | – |
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 |
|---|---|---|---|---|
| NH4CN (cr) | 0.42[1] | – | – | 134[1] |
| NH4CN (ai) | 18.0[1] | 93.0[1] | 207.5[1] | – |
| NH4CN (aq) | 32.2[1] | – | – | – |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[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, (aq):Aqueous solution, (l):Liquid, (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°, 0.42 kJ · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, 18.0 kJ · mol−1
- ^ ΔfG°, 93.0 kJ · mol−1
- ^ S°, 207.5 J · K−1 · mol−1
- ^ ΔfH°, 32.2 kJ · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 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