NH4CN + 2H2O 💧⚡→ NH4NO2 + CH4↑
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- Electrolysis of aqueous ammonium cyanide with water as non-redox agent
Electrolysis of aqueous ammonium cyanide yields ammonium nitrite 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 cyanide 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 cyanide with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4CN | Ammonium cyanide | 1 | Self redox agent | Very soluble in water |
| H2O | Water | 2 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO2 | Ammonium nitrite | 1 | Oxidized | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous ammonium cyanide 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 | 239.9 | – | – | – |
per 1 mol of | 239.9 | – | – | – |
per 1 mol of | 120.0 | – | – | – |
per 1 mol of | 239.9 | – | – | – |
| 239.9 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium cyanide with water as non-redox agent◆
ΔrG 218.9 kJ/mol K 0.45 × 10−38 pK 38.35
| 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 | 241.7 | 218.9 | 75.3 | – |
per 1 mol of | 241.7 | 218.9 | 75.3 | – |
per 1 mol of | 120.8 | 109.5 | 37.6 | – |
per 1 mol of | 241.7 | 218.9 | 75.3 | – |
| 241.7 | 218.9 | 75.3 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium cyanide with water as non-redox agent◆
ΔrG 235.3 kJ/mol K 0.60 × 10−41 pK 41.22
| 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 | 227.4 | 235.3 | −27.2 | – |
per 1 mol of | 227.4 | 235.3 | −27.2 | – |
per 1 mol of | 113.7 | 117.7 | −13.6 | – |
per 1 mol of | 227.4 | 235.3 | −27.2 | – |
| 227.4 | 235.3 | −27.2 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous ammonium cyanide 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 | 227.5 | – | – | – |
per 1 mol of | 227.5 | – | – | – |
per 1 mol of | 113.8 | – | – | – |
per 1 mol of | 227.5 | – | – | – |
| 227.5 | – | – | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous ammonium cyanide 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 | 213.2 | – | – | – |
per 1 mol of | 213.2 | – | – | – |
per 1 mol of | 106.6 | – | – | – |
per 1 mol of | 213.2 | – | – | – |
| 213.2 | – | – | – |
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 |
|---|---|---|---|---|
| NH4CN (cr) | 0.42[1] | – | – | 134[1] |
| NH4CN (ai) | 18.0[1] | 93.0[1] | 207.5[1] | – |
| NH4CN (aq) | 32.2[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, (aq):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] |
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, 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°, -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°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1