2Mg(NO3)2 🔥→ 2MgO + 2N2O4 + O2↑
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- Decomposition of magnesium nitrate
Decomposition of magnesium nitrate yields magnesium oxide, dinitrogen tetraoxide, 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 | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgO | Magnesium oxide | 2 | – | – |
| N2O4 | Dinitrogen tetraoxide | 2 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Decomposition of magnesium nitrate◆
ΔrG 242.0 kJ/mol K 0.40 × 10−42 pK 42.40
| 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 | 346.34 | 242.0 | 351.4 | 106.2 |
per 1 mol of | 173.17 | 121.0 | 175.7 | 53.10 |
per 1 mol of | 173.17 | 121.0 | 175.7 | 53.10 |
per 1 mol of | 173.17 | 121.0 | 175.7 | 53.10 |
| 346.34 | 242.0 | 351.4 | 106.2 |
Changes in aqueous solution (1)
- Decomposition of magnesium nitrate◆
ΔrG 417.8 kJ/mol K 0.64 × 10−73 pK 73.20
| 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 | 528.18 | 417.8 | 369.8 | – |
per 1 mol of | 264.09 | 208.9 | 184.9 | – |
per 1 mol of | 264.09 | 208.9 | 184.9 | – |
per 1 mol of | 264.09 | 208.9 | 184.9 | – |
| 528.18 | 417.8 | 369.8 | – |
Changes in aqueous solution (2)
- Decomposition of magnesium nitrate◆
ΔrG 434.2 kJ/mol K 0.85 × 10−76 pK 76.07
| 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 | 516.5 | 434.2 | 275.5 | – |
per 1 mol of | 258.3 | 217.1 | 137.8 | – |
per 1 mol of | 258.3 | 217.1 | 137.8 | – |
per 1 mol of | 258.3 | 217.1 | 137.8 | – |
| 516.5 | 434.2 | 275.5 | – |
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] | – | – | – |
| 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] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1