3Mg(NO3)2 🔥→ 3MgO + 3N2O3↑ + 2O3↑
Last updated:
- Decomposition of magnesium nitrate
Decomposition of magnesium nitrate yields magnesium oxide, dinitrogen trioxide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of magnesium nitrate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of magnesium nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg(NO3)2 | Magnesium nitrate | 3 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgO | Magnesium oxide | 3 | – | – |
| N2O3 | Dinitrogen trioxide | 3 | Reduced | – |
| 2 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Decomposition of magnesium nitrate◆
ΔrG 815.1 kJ/mol K 0.16 × 10−142 pK 142.80
| 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 | 1114.6 | 815.1 | 1006.4 | −37.55 |
per 1 mol of | 371.53 | 271.7 | 335.47 | −12.52 |
per 1 mol of | 371.53 | 271.7 | 335.47 | −12.52 |
per 1 mol of | 371.53 | 271.7 | 335.47 | −12.52 |
| 557.30 | 407.6 | 503.20 | −18.77 |
Changes in aqueous solution (1)
- Decomposition of magnesium nitrate◆
ΔrG 1078.8 kJ/mol K 0.10 × 10−188 pK 189.00
| 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 | 1387.3 | 1078.8 | 1034.0 | – |
per 1 mol of | 462.43 | 359.60 | 344.67 | – |
per 1 mol of | 462.43 | 359.60 | 344.67 | – |
per 1 mol of | 462.43 | 359.60 | 344.67 | – |
| 693.65 | 539.40 | 517.00 | – |
Changes in aqueous solution (2)
- Decomposition of magnesium nitrate◆
ΔrG 1100.6 kJ/mol K 0.15 × 10−192 pK 192.82
| 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 | 1353.7 | 1100.6 | 848 | – |
per 1 mol of | 451.23 | 366.87 | 283 | – |
per 1 mol of | 451.23 | 366.87 | 283 | – |
per 1 mol of | 451.23 | 366.87 | 283 | – |
| 676.85 | 550.30 | 424 | – |
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 |
|---|---|---|---|---|
| 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] | – |
* (cr):Crystalline 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 |
|---|---|---|---|---|
| MgO (cr) | -597.98[1] | -565.95[1] | 27.91[1] | 37.66[1] |
| MgO (g) | 17[1] | – | – | – |
| N2O3 (l) | 50.29[1] | – | – | – |
| N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, -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°, -597.98 kJ · mol−1
- ^ ΔfG°, -565.95 kJ · mol−1
- ^ S°, 27.91 J · K−1 · mol−1
- ^ Cp°, 37.66 J · K−1 · mol−1
- ^ ΔfH°, 17. kJ · mol−1
- ^ ΔfH°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1