10NO + Mg(OH)2 → Mg(NO3)2 + 4N2O + H2O2
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The reaction of nitrogen monoxide and magnesium hydroxide yields magnesium nitrate, dinitrotgen monoxide, 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 nitrogen monoxide and magnesium hydroxide
General equation
- Reaction of self redoxing species and base
- Self-redoxing speciesSelf redox agent + BaseNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of nitrogen monoxide and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 10 | – | Self redoxing |
| Mg(OH)2 | Magnesium hydroxide | 1 | – | Base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg(NO3)2 | Magnesium nitrate | 1 | Oxidized | – |
| N2O | Dinitrotgen monoxide | 4 | Reduced | – |
| 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of nitrogen monoxide and magnesium hydroxide◆
ΔrG −324.9 kJ/mol K 8.32 × 1056 pK −56.92
| 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 | −628.19 | −324.9 | −1017.8 | 9.3 |
per 1 mol of | −62.819 | −32.49 | −101.78 | 0.93 |
per 1 mol of | −628.19 | −324.9 | −1017.8 | 9.3 |
per 1 mol of | −628.19 | −324.9 | −1017.8 | 9.3 |
per 1 mol of | −157.05 | −81.22 | −254.45 | 2.3 |
| −628.19 | −324.9 | −1017.8 | 9.3 |
Changes in standard condition (2)
- Reaction of nitrogen monoxide and magnesium hydroxide
| 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 | −632.2 | – | – | – |
per 1 mol of | −63.22 | – | – | – |
per 1 mol of | −632.2 | – | – | – |
per 1 mol of | −632.2 | – | – | – |
per 1 mol of | −158.1 | – | – | – |
| −632.2 | – | – | – |
Changes in aqueous solution (1)
- Reaction of nitrogen monoxide and magnesium hydroxide◆
ΔrG −426.5 kJ/mol K 5.24 × 1074 pK −74.72
| 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 | −722.50 | −426.5 | −992.7 | – |
per 1 mol of | −72.250 | −42.65 | −99.27 | – |
per 1 mol of | −722.50 | −426.5 | −992.7 | – |
per 1 mol of | −722.50 | −426.5 | −992.7 | – |
per 1 mol of | −180.63 | −106.6 | −248.2 | – |
| −722.50 | −426.5 | −992.7 | – |
Changes in aqueous solution (2)
- Reaction of nitrogen monoxide and magnesium hydroxide
| 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 | −826.3 | – | – | – |
per 1 mol of | −82.63 | – | – | – |
per 1 mol of | −826.3 | – | – | – |
per 1 mol of | −826.3 | – | – | – |
per 1 mol of | −206.6 | – | – | – |
| −826.3 | – | – | – |
Changes in aqueous solution (3)
- Reaction of nitrogen monoxide and magnesium hydroxide
| 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 | −726.5 | – | – | – |
per 1 mol of | −72.65 | – | – | – |
per 1 mol of | −726.5 | – | – | – |
per 1 mol of | −726.5 | – | – | – |
per 1 mol of | −181.6 | – | – | – |
| −726.5 | – | – | – |
Changes in aqueous solution (4)
- Reaction of nitrogen monoxide and magnesium hydroxide
| 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 | −830.3 | – | – | – |
per 1 mol of | −83.03 | – | – | – |
per 1 mol of | −830.3 | – | – | – |
per 1 mol of | −830.3 | – | – | – |
per 1 mol of | −207.6 | – | – | – |
| −830.3 | – | – | – |
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 |
|---|---|---|---|---|
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| Mg(OH)2 (cr) | -924.54[1] | -833.51[1] | 63.18[1] | 77.03[1] |
| Mg(OH)2 (am) precipitated | -920.5[1] | – | – | – |
| Mg(OH)2 (g) | -561[1] | – | – | – |
| Mg(OH)2 (ai) | -926.84[1] | -769.4[1] | -159.4[1] | – |
* (g):Gas, (cr):Crystalline solid, (am):Amorphous solid, (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 |
|---|---|---|---|---|
| Mg(NO3)2 (cr) | -790.65[1] | -589.4[1] | 164.0[1] | 141.92[1] |
| Mg(NO3)2 (ai) | -881.57[1] | -677.3[1] | 154.8[1] | – |
| Mg(NO3)2 (cr) 2 hydrate | -1409.2[1] | – | – | – |
| Mg(NO3)2 (cr) 6 hydrate | -2613.28[1] | -2080.3[1] | 452[1] | – |
| N2O (g) | 82.05[1] | 104.20[1] | 219.85[1] | 38.45[1] |
| N2O (aq) | 56.1[1] | – | – | – |
| (l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
| (g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
| (ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (aq):Aqueous solution, (l):Liquid, (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°, 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°, -924.54 kJ · mol−1
- ^ ΔfG°, -833.51 kJ · mol−1
- ^ S°, 63.18 J · K−1 · mol−1
- ^ Cp°, 77.03 J · K−1 · mol−1
- ^ ΔfH°, -920.5 kJ · mol−1
- ^ ΔfH°, -561. kJ · mol−1
- ^ ΔfH°, -926.84 kJ · mol−1
- ^ ΔfG°, -769.4 kJ · mol−1
- ^ S°, -159.4 J · K−1 · mol−1
- ^ ΔfH°, -790.65 kJ · mol−1
- ^ ΔfG°, -589.4 kJ · mol−1
- ^ S°, 164.0 J · K−1 · mol−1
- ^ Cp°, 141.92 J · K−1 · mol−1
- ^ ΔfH°, -881.57 kJ · mol−1
- ^ ΔfG°, -677.3 kJ · mol−1
- ^ S°, 154.8 J · K−1 · mol−1
- ^ ΔfH°, -1409.2 kJ · mol−1
- ^ ΔfH°, -2613.28 kJ · mol−1
- ^ ΔfG°, -2080.3 kJ · mol−1
- ^ S°, 452. J · K−1 · mol−1
- ^ ΔfH°, 82.05 kJ · mol−1
- ^ ΔfG°, 104.20 kJ · mol−1
- ^ S°, 219.85 J · K−1 · mol−1
- ^ Cp°, 38.45 J · K−1 · mol−1
- ^ ΔfH°, 56.1 kJ · mol−1
- ^ ΔfH°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1