5(NH4)2SO4 🔥→ 2NO↑ + 5SO2↑ + 8H2O + 8NH3↑
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- Decomposition of ammonium sulfate
Decomposition of ammonium sulfate yields nitrogen monoxide, sulfur dioxide, water, and ammonia (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 ammonium sulfate
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 ammonium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2SO4 | Ammonium sulfate | 5 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 2 | Oxidized | – |
| SO2 | Sulfur dioxide | 5 | Reduced | – |
| H2O | Water | 8 | – | – |
| NH3 | Ammonia | 8 | – | – |
Thermodynamic changes
Changes in standard condition
- Decomposition of ammonium sulfate◆
ΔrG 1151.85 kJ/mol K 0.16 × 10−201 pK 201.80
| 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 | 1945.08 | 1151.85 | 2661.0 | 204.40 |
per 1 mol of | 389.016 | 230.370 | 532.20 | 40.880 |
per 1 mol of | 972.540 | 575.925 | 1330.5 | 102.20 |
per 1 mol of | 389.016 | 230.370 | 532.20 | 40.880 |
per 1 mol of | 243.135 | 143.981 | 332.63 | 25.550 |
per 1 mol of | 243.135 | 143.981 | 332.63 | 25.550 |
Changes in aqueous solution (1)
- Decomposition of ammonium sulfate◆
ΔrG 1159.20 kJ/mol K 0.83 × 10−203 pK 203.08
| 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 | 1912.23 | 1159.20 | 2527.0 | 1807.3 |
per 1 mol of | 382.446 | 231.840 | 505.40 | 361.46 |
per 1 mol of | 956.115 | 579.600 | 1263.5 | 903.65 |
per 1 mol of | 382.446 | 231.840 | 505.40 | 361.46 |
per 1 mol of | 239.029 | 144.900 | 315.88 | 225.91 |
per 1 mol of | 239.029 | 144.900 | 315.88 | 225.91 |
Changes in aqueous solution (2)
- Decomposition of ammonium sulfate◆
ΔrG 1078.80 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 | 1638.79 | 1078.80 | 1877.8 | – |
per 1 mol of | 327.758 | 215.760 | 375.56 | – |
per 1 mol of | 819.395 | 539.400 | 938.90 | – |
per 1 mol of | 327.758 | 215.760 | 375.56 | – |
per 1 mol of | 204.849 | 134.850 | 234.72 | – |
per 1 mol of | 204.849 | 134.850 | 234.72 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium sulfate◆
ΔrG 1156.79 kJ/mol K 0.22 × 10−202 pK 202.66
| 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 | 1781.48 | 1156.79 | 2095.4 | – |
per 1 mol of | 356.296 | 231.358 | 419.08 | – |
per 1 mol of | 890.740 | 578.395 | 1047.7 | – |
per 1 mol of | 356.296 | 231.358 | 419.08 | – |
per 1 mol of | 222.685 | 144.599 | 261.93 | – |
per 1 mol of | 222.685 | 144.599 | 261.93 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium sulfate◆
ΔrG 1076.39 kJ/mol K 0.27 × 10−188 pK 188.58
| 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 | 1508.04 | 1076.39 | 1446.2 | – |
per 1 mol of | 301.608 | 215.278 | 289.24 | – |
per 1 mol of | 754.020 | 538.195 | 723.10 | – |
per 1 mol of | 301.608 | 215.278 | 289.24 | – |
per 1 mol of | 188.505 | 134.549 | 180.78 | – |
per 1 mol of | 188.505 | 134.549 | 180.78 | – |
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 |
|---|---|---|---|---|
| (NH4)2SO4 (cr) | -1180.85[1] | -901.67[1] | 220.1[1] | 187.49[1] |
| (NH4)2SO4 (ai) | -1174.28[1] | -903.14[1] | 246.9[1] | -133.1[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 |
|---|---|---|---|---|
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[1] | – |
* (g):Gas, (l):Liquid, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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°, -1180.85 kJ · mol−1
- ^ ΔfG°, -901.67 kJ · mol−1
- ^ S°, 220.1 J · K−1 · mol−1
- ^ Cp°, 187.49 J · K−1 · mol−1
- ^ ΔfH°, -1174.28 kJ · mol−1
- ^ ΔfG°, -903.14 kJ · mol−1
- ^ S°, 246.9 J · K−1 · mol−1
- ^ Cp°, -133.1 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°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1