2NH4SCN + 8H2O 💧⚡→ NH4NO2 + 2H2S↑ + 2NH4HCO3 + 3H2↑
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- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
Electrolysis of aqueous ammonium thiocyanate yields ammonium nitrite, hydrogen sulfide, ammonium hydrogencarbonate, 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 | 2 | Reducing | Very soluble in water |
H2O | Water | 8 | – | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH4NO2 | Ammonium nitrite | 1 | Oxidized | – |
H2S | Hydrogen sulfide | 2 | – | – |
NH4HCO3 | Ammonium hydrogencarbonate | 2 | – | – |
3 | – | – |
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 | 447.5 | – | – | – |
per 1 mol of | 223.8 | – | – | – |
per 1 mol of | 55.94 | – | – | – |
per 1 mol of | 447.5 | – | – | – |
per 1 mol of | 223.8 | – | – | – |
per 1 mol of | 223.8 | – | – | – |
149.2 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 359.4 kJ/mol K 0.11 × 10−62 pK 62.96
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 | 471.3 | 359.4 | 374.6 | – |
per 1 mol of | 235.7 | 179.7 | 187.3 | – |
per 1 mol of | 58.91 | 44.92 | 46.83 | – |
per 1 mol of | 471.3 | 359.4 | 374.6 | – |
per 1 mol of | 235.7 | 179.7 | 187.3 | – |
per 1 mol of | 235.7 | 179.7 | 187.3 | – |
157.1 | 119.8 | 124.9 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 412.2 kJ/mol K 0.61 × 10−72 pK 72.21
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 | 458.7 | 412.2 | 1714 | – |
per 1 mol of | 229.3 | 206.1 | 857.0 | – |
per 1 mol of | 57.34 | 51.52 | 214.3 | – |
per 1 mol of | 458.7 | 412.2 | 1714 | – |
per 1 mol of | 229.3 | 206.1 | 857.0 | – |
per 1 mol of | 229.3 | 206.1 | 857.0 | – |
152.9 | 137.4 | 571.3 | – |
Changes in aqueous solution (3)
- 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 | 476.9 | – | – | – |
per 1 mol of | 238.4 | – | – | – |
per 1 mol of | 59.61 | – | – | – |
per 1 mol of | 476.9 | – | – | – |
per 1 mol of | 238.4 | – | – | – |
per 1 mol of | 238.4 | – | – | – |
159.0 | – | – | – |
Changes in aqueous solution (4)
- 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 | 464.3 | – | – | – |
per 1 mol of | 232.2 | – | – | – |
per 1 mol of | 58.04 | – | – | – |
per 1 mol of | 464.3 | – | – | – |
per 1 mol of | 232.2 | – | – | – |
per 1 mol of | 232.2 | – | – | – |
154.8 | – | – | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 370.8 kJ/mol K 0.11 × 10−64 pK 64.96
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 | 433.2 | 370.8 | 205 | – |
per 1 mol of | 216.6 | 185.4 | 103 | – |
per 1 mol of | 54.15 | 46.35 | 25.6 | – |
per 1 mol of | 433.2 | 370.8 | 205 | – |
per 1 mol of | 216.6 | 185.4 | 103 | – |
per 1 mol of | 216.6 | 185.4 | 103 | – |
144.4 | 123.6 | 68.3 | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent◆
ΔrG 423.6 kJ/mol K 0.61 × 10−74 pK 74.21
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 | 420.6 | 423.6 | 1544 | – |
per 1 mol of | 210.3 | 211.8 | 772.0 | – |
per 1 mol of | 52.58 | 52.95 | 193.0 | – |
per 1 mol of | 420.6 | 423.6 | 1544 | – |
per 1 mol of | 210.3 | 211.8 | 772.0 | – |
per 1 mol of | 210.3 | 211.8 | 772.0 | – |
140.2 | 141.2 | 514.7 | – |
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 | 438.8 | – | – | – |
per 1 mol of | 219.4 | – | – | – |
per 1 mol of | 54.85 | – | – | – |
per 1 mol of | 438.8 | – | – | – |
per 1 mol of | 219.4 | – | – | – |
per 1 mol of | 219.4 | – | – | – |
146.3 | – | – | – |
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 | 426.2 | – | – | – |
per 1 mol of | 213.1 | – | – | – |
per 1 mol of | 53.27 | – | – | – |
per 1 mol of | 426.2 | – | – | – |
per 1 mol of | 213.1 | – | – | – |
per 1 mol of | 213.1 | – | – | – |
142.1 | – | – | – |
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 |
---|---|---|---|---|
NH4NO2 (cr) | -256.5[1] | – | – | – |
NH4NO2 (ai) | -237.2[1] | -111.6[1] | 236.4[1] | -17.6[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] | – |
NH4HCO3 (cr) | -849.4[1] | -665.9[1] | 120.9[1] | – |
NH4HCO3 (ai) | -824.50[1] | -666.07[1] | 204.6[1] | – |
NH4HCO3 (aq) | -821.7[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, (g):Gas, (ao):Un-ionized aqueous solution, (aq):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°, -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°, -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°, -849.4 kJ · mol−1
- ^ ΔfG°, -665.9 kJ · mol−1
- ^ S°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -824.50 kJ · mol−1
- ^ ΔfG°, -666.07 kJ · mol−1
- ^ S°, 204.6 J · K−1 · mol−1
- ^ ΔfH°, -821.7 kJ · 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