2KSCN + 16HNO3 → 2KHSO4 + 9N2O4 + 2CO2↑ + 7H2↑
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- Reaction of potassium thiocyanate and nitric acid
The reaction of potassium thiocyanate and nitric acid yields potassium hydrogensulfate, dinitrogen tetraoxide, 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
- Reaction of potassium thiocyanate and nitric acid
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium thiocyanate and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KSCN | Potassium thiocyanate | 2 | Reducing | Reducing |
| HNO3 | Nitric acid | 16 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KHSO4 | Potassium hydrogensulfate | 2 | Oxidized | – |
| N2O4 | Dinitrogen tetraoxide | 9 | Redoxed product | – |
| CO2 | Carbon dioxide | 2 | – | – |
| 7 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium thiocyanate and nitric acid◆
ΔrG −325.5 kJ/mol K 1.06 × 1057 pK −57.03
| 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 | −97.8 | −325.5 | 763.1 | – |
per 1 mol of | −48.9 | −162.8 | 381.6 | – |
per 1 mol of | −6.11 | −20.34 | 47.69 | – |
per 1 mol of | −48.9 | −162.8 | 381.6 | – |
per 1 mol of | −10.9 | −36.17 | 84.79 | – |
per 1 mol of | −48.9 | −162.8 | 381.6 | – |
| −14.0 | −46.50 | 109.0 | – |
Changes in aqueous solution (1)
- Reaction of potassium thiocyanate and nitric acid◆
ΔrG 171.90 kJ/mol K 0.77 × 10−30 pK 30.12
| 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 | 427.68 | 171.90 | 857.5 | 2857 |
per 1 mol of | 213.84 | 85.950 | 428.8 | 1429 |
per 1 mol of | 26.730 | 10.744 | 53.59 | 178.6 |
per 1 mol of | 213.84 | 85.950 | 428.8 | 1429 |
per 1 mol of | 47.520 | 19.100 | 95.28 | 317.4 |
per 1 mol of | 213.84 | 85.950 | 428.8 | 1429 |
| 61.097 | 24.557 | 122.5 | 408.1 |
Changes in aqueous solution (2)
- Reaction of potassium thiocyanate and nitric acid◆
ΔrG 295.1 kJ/mol K 0.20 × 10−51 pK 51.70
| 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 | 398.3 | 295.1 | 3982 | – |
per 1 mol of | 199.2 | 147.6 | 1991 | – |
per 1 mol of | 24.89 | 18.44 | 248.9 | – |
per 1 mol of | 199.2 | 147.6 | 1991 | – |
per 1 mol of | 44.26 | 32.79 | 442.4 | – |
per 1 mol of | 199.2 | 147.6 | 1991 | – |
| 56.90 | 42.16 | 568.9 | – |
Changes in aqueous solution (3)
- Reaction of potassium thiocyanate and nitric acid◆
ΔrG 188.66 kJ/mol K 0.89 × 10−33 pK 33.05
| 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 | 387.10 | 188.66 | 665.2 | – |
per 1 mol of | 193.55 | 94.330 | 332.6 | – |
per 1 mol of | 24.194 | 11.791 | 41.58 | – |
per 1 mol of | 193.55 | 94.330 | 332.6 | – |
per 1 mol of | 43.011 | 20.962 | 73.91 | – |
per 1 mol of | 193.55 | 94.330 | 332.6 | – |
| 55.300 | 26.951 | 95.03 | – |
Changes in aqueous solution (4)
- Reaction of potassium thiocyanate and nitric acid◆
ΔrG 311.9 kJ/mol K 0.23 × 10−54 pK 54.64
| 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 | 357.7 | 311.9 | 3789 | – |
per 1 mol of | 178.8 | 155.9 | 1895 | – |
per 1 mol of | 22.36 | 19.49 | 236.8 | – |
per 1 mol of | 178.8 | 155.9 | 1895 | – |
per 1 mol of | 39.74 | 34.66 | 421.0 | – |
per 1 mol of | 178.8 | 155.9 | 1895 | – |
| 51.10 | 44.56 | 541.3 | – |
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 |
|---|---|---|---|---|
| KSCN (cr) | -200.16[1] | -178.31[1] | 124.26[1] | 88.53[1] |
| KSCN (ai) | -175.94[1] | -190.56[1] | 246.9[1] | -18.4[1] |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[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 |
|---|---|---|---|---|
| KHSO4 (cr) | -1160.6[1] | -1031.3[1] | 138.1[1] | – |
| KHSO4 (ai) | -1139.72[1] | -1039.18[1] | 234.3[1] | -63[1] |
| N2O4 (l) | -19.50[1] | 97.54[1] | 209.2[1] | 142.7[1] |
| N2O4 (g) | 9.16[1] | 97.89[1] | 304.29[1] | 77.28[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, (ai):Ionized 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°, -200.16 kJ · mol−1
- ^ ΔfG°, -178.31 kJ · mol−1
- ^ S°, 124.26 J · K−1 · mol−1
- ^ Cp°, 88.53 J · K−1 · mol−1
- ^ ΔfH°, -175.94 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 246.9 J · K−1 · mol−1
- ^ Cp°, -18.4 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -1160.6 kJ · mol−1
- ^ ΔfG°, -1031.3 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1139.72 kJ · mol−1
- ^ ΔfG°, -1039.18 kJ · mol−1
- ^ S°, 234.3 J · K−1 · mol−1
- ^ Cp°, -63. J · K−1 · mol−1
- ^ ΔfH°, -19.50 kJ · mol−1
- ^ ΔfG°, 97.54 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ Cp°, 142.7 J · K−1 · mol−1
- ^ ΔfH°, 9.16 kJ · mol−1
- ^ ΔfG°, 97.89 kJ · mol−1
- ^ S°, 304.29 J · K−1 · mol−1
- ^ Cp°, 77.28 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