6Na + 2KNO3 → 3Na2O + 2NO↑ + K2O
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- Reaction of and potassium nitrate
The reaction of and potassium nitrate yields sodium oxide, nitrogen monoxide, and potassium oxide (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 potassium nitrate
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 and potassium nitrate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
6 | Reducing | Reducing | ||
KNO3 | Potassium nitrate | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2O | Sodium oxide | 3 | Oxidized | – |
NO | Nitrogen monoxide | 2 | Reduced | – |
K2O | Potassium oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and potassium nitrate◆
ΔrG −485.7 kJ/mol K 1.23 × 1085 pK −85.09
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 | −434.4 | −485.7 | 167.4 | −11.5 |
−72.40 | −80.95 | 27.90 | −1.92 | |
per 1 mol of | −217.2 | −242.8 | 83.70 | −5.75 |
per 1 mol of | −144.8 | −161.9 | 55.80 | −3.83 |
per 1 mol of | −217.2 | −242.8 | 83.70 | −5.75 |
per 1 mol of | −434.4 | −485.7 | 167.4 | −11.5 |
Changes in aqueous solution
- Reaction of and potassium nitrate◆
ΔrG −486.3 kJ/mol K 1.57 × 1085 pK −85.20
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 | −504.2 | −486.3 | −64.3 | 311.1 |
−84.03 | −81.05 | −10.7 | 51.85 | |
per 1 mol of | −252.1 | −243.2 | −32.1 | 155.6 |
per 1 mol of | −168.1 | −162.1 | −21.4 | 103.7 |
per 1 mol of | −252.1 | −243.2 | −32.1 | 155.6 |
per 1 mol of | −504.2 | −486.3 | −64.3 | 311.1 |
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 |
---|---|---|---|---|
(cr) | 0[1] | 0[1] | 51.21[1] | 28.24[1] |
(g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
---|---|---|---|---|
Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[1] |
NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas
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°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfH°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280