2Na + 3AgSCN → 2NaSCN + Ag2S + AgCN
Last updated:
- Reaction of and silver(I) thiocyanate
The reaction of and silver(I) thiocyanate yields sodium thiocyanate, silver(I) sulfide, and silver(I) cyanide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and silver(I) thiocyanate
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and silver(I) thiocyanate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reducing | Reducing | ||
| AgSCN | Silver(I) thiocyanate | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaSCN | Sodium thiocyanate | 2 | Oxidized | – |
| Ag2S | Silver(I) sulfide | 1 | – | – |
| AgCN | Silver(I) cyanide | 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and silver(I) thiocyanate
| 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 | −541.1 | – | – | – |
| −270.6 | – | – | – | |
per 1 mol of | −180.4 | – | – | – |
per 1 mol of | −270.6 | – | – | – |
per 1 mol of | −541.1 | – | – | – |
per 1 mol of | −541.1 | – | – | – |
Changes in standard condition (2)
- Reaction of and silver(I) thiocyanate
| 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 | – | – | – |
| −268.9 | – | – | – | |
per 1 mol of | −179.3 | – | – | – |
per 1 mol of | −268.9 | – | – | – |
per 1 mol of | −537.9 | – | – | – |
per 1 mol of | −537.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and silver(I) thiocyanate◆
ΔrG −777.1 kJ/mol K 1.39 × 10136 pK −136.14
| 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 | −809.8 | −777.1 | −118.6 | – |
| −404.9 | −388.6 | −59.30 | – | |
per 1 mol of | −269.9 | −259.0 | −39.53 | – |
per 1 mol of | −404.9 | −388.6 | −59.30 | – |
per 1 mol of | −809.8 | −777.1 | −118.6 | – |
per 1 mol of | −809.8 | −777.1 | −118.6 | – |
Changes in aqueous solution (2)
- Reaction of and silver(I) thiocyanate◆
ΔrG −695.8 kJ/mol K 7.92 × 10121 pK −121.90
| 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 | – | −695.8 | – | – |
| – | −347.9 | – | – | |
per 1 mol of | – | −231.9 | – | – |
per 1 mol of | – | −347.9 | – | – |
per 1 mol of | – | −695.8 | – | – |
per 1 mol of | – | −695.8 | – | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 51.21[1] | 28.24[1] |
| (g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
| AgSCN (cr) | 87.9[1] | 101.39[1] | 131.0[1] | 63[1] |
| AgSCN (ai) | 182.00[1] | 169.80[1] | 217.1[1] | -18.4[1] |
| AgSCN (ao) | – | 142.7[1] | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
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 |
|---|---|---|---|---|
| NaSCN (cr) | -170.50[1] | – | – | – |
| NaSCN (ai) | -163.68[1] | -169.18[1] | 203.3[1] | 6.3[1] |
| Ag2S (cr) α, orthorhombic | -32.59[1] | -40.67[1] | 144.01[1] | 76.53[1] |
| Ag2S (cr) β | -29.41[1] | -39.46[1] | 150.6[1] | – |
| AgCN (cr) | 96.2[1] | 111.3[1] | 84.5[1] | – |
* (cr):Crystalline solid, (ai):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 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 51.21 J · K−1 · mol−1
- ^ Cp°, 28.24 J · K−1 · mol−1
- ^ ΔfH°, 107.32 kJ · mol−1
- ^ ΔfG°, 76.761 kJ · mol−1
- ^ S°, 153.712 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 87.9 kJ · mol−1
- ^ ΔfG°, 101.39 kJ · mol−1
- ^ S°, 131.0 J · K−1 · mol−1
- ^ Cp°, 63. J · K−1 · mol−1
- ^ ΔfH°, 182.00 kJ · mol−1
- ^ ΔfG°, 169.80 kJ · mol−1
- ^ S°, 217.1 J · K−1 · mol−1
- ^ Cp°, -18.4 J · K−1 · mol−1
- ^ ΔfG°, 142.7 kJ · mol−1
- ^ ΔfH°, -170.50 kJ · mol−1
- ^ ΔfH°, -163.68 kJ · mol−1
- ^ ΔfG°, -169.18 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1
- ^ Cp°, 6.3 J · K−1 · mol−1
- ^ ΔfH°, -32.59 kJ · mol−1
- ^ ΔfG°, -40.67 kJ · mol−1
- ^ S°, 144.01 J · K−1 · mol−1
- ^ Cp°, 76.53 J · K−1 · mol−1
- ^ ΔfH°, -29.41 kJ · mol−1
- ^ ΔfG°, -39.46 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfH°, 96.2 kJ · mol−1
- ^ ΔfG°, 111.3 kJ · mol−1
- ^ S°, 84.5 J · K−1 · mol−1