(NH4)2SO3 + 2MnO2 → N2H4 + MnSO4 + Mn(OH)2 + H2O
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The reaction of ammonium sulfite and manganese(IV) oxide yields hydrazine, manganese(II) sulfate, manganese(II) hydroxide, and water (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 ammonium sulfite and manganese(IV) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of ammonium sulfite and manganese(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2SO3 | Ammonium sulfite | 1 | Reducing | Reducing |
| MnO2 | Manganese(IV) oxide | 2 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| N2H4 | Hydrazine | 1 | Oxidized | – |
| MnSO4 | Manganese(II) sulfate | 1 | Redoxed product | – |
| Mn(OH)2 | Manganese(II) hydroxide | 1 | Reduced | – |
| H2O | Water | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of ammonium sulfite and manganese(IV) oxide
| 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 | −70.5 | – | – | – |
per 1 mol of | −70.5 | – | – | – |
per 1 mol of | −35.3 | – | – | – |
per 1 mol of | −70.5 | – | – | – |
per 1 mol of | −70.5 | – | – | – |
per 1 mol of | −70.5 | – | – | – |
per 1 mol of | −70.5 | – | – | – |
Changes in standard condition (2)
- Reaction of ammonium sulfite and manganese(IV) oxide
| 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 | −105.6 | – | – | – |
per 1 mol of | −105.6 | – | – | – |
per 1 mol of | −52.80 | – | – | – |
per 1 mol of | −105.6 | – | – | – |
per 1 mol of | −105.6 | – | – | – |
per 1 mol of | −105.6 | – | – | – |
per 1 mol of | −105.6 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium sulfite and manganese(IV) oxide◆
ΔrG −134.4 kJ/mol K 3.51 × 1023 pK −23.55
| 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 | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −61.20 | −67.20 | 20 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
Changes in aqueous solution (2)
- Reaction of ammonium sulfite and manganese(IV) oxide◆
ΔrG −121.4 kJ/mol K 1.86 × 1021 pK −21.27
| 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 | −136.6 | −121.4 | −50 | – |
per 1 mol of | −136.6 | −121.4 | −50 | – |
per 1 mol of | −68.30 | −60.70 | −25 | – |
per 1 mol of | −136.6 | −121.4 | −50 | – |
per 1 mol of | −136.6 | −121.4 | −50 | – |
per 1 mol of | −136.6 | −121.4 | −50 | – |
per 1 mol of | −136.6 | −121.4 | −50 | – |
Changes in aqueous solution (3)
- Reaction of ammonium sulfite and manganese(IV) oxide◆
ΔrG −134.4 kJ/mol K 3.51 × 1023 pK −23.55
| 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 | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −61.20 | −67.20 | 20 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
per 1 mol of | −122.4 | −134.4 | 40 | – |
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)2SO3 (cr) | -885.3[1] | – | – | – |
| (NH4)2SO3 (ai) | -900.4[1] | -645.0[1] | 197.5[1] | – |
| (NH4)2SO3 (cr) 1 hydrate | -1187.4[1] | – | – | – |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid
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 |
|---|---|---|---|---|
| N2H4 (l) | 50.63[1] | 149.34[1] | 121.21[1] | 98.87[1] |
| N2H4 (g) | 95.40[1] | 159.35[1] | 238.47[1] | 49.58[1] |
| N2H4 (ao) | 34.31[1] | 128.1[1] | 138[1] | – |
| MnSO4 (cr) | -1065.25[1] | -957.36[1] | 112.1[1] | 100.50[1] |
| MnSO4 (ai) | -1130.1[1] | -972.7[1] | -53.6[1] | -243[1] |
| MnSO4 (ao) | -1115.9[1] | -985.7[1] | 36.4[1] | – |
| MnSO4 (cr) 1 hydrate α | -1376.5[1] | – | – | – |
| MnSO4 (cr) 1 hydrate β | -1348.1[1] | – | – | – |
| MnSO4 (cr) 4 hydrate | -2258.1[1] | – | – | – |
| MnSO4 (cr) 5 hydrate | -2553.1[1] | – | – | 326[1] |
| MnSO4 (cr) 7 hydrate | -3139.3[1] | – | – | – |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[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] |
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous 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°, -885.3 kJ · mol−1
- ^ ΔfH°, -900.4 kJ · mol−1
- ^ ΔfG°, -645.0 kJ · mol−1
- ^ S°, 197.5 J · K−1 · mol−1
- ^ ΔfH°, -1187.4 kJ · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · mol−1
- ^ ΔfH°, 50.63 kJ · mol−1
- ^ ΔfG°, 149.34 kJ · mol−1
- ^ S°, 121.21 J · K−1 · mol−1
- ^ Cp°, 98.87 J · K−1 · mol−1
- ^ ΔfH°, 95.40 kJ · mol−1
- ^ ΔfG°, 159.35 kJ · mol−1
- ^ S°, 238.47 J · K−1 · mol−1
- ^ Cp°, 49.58 J · K−1 · mol−1
- ^ ΔfH°, 34.31 kJ · mol−1
- ^ ΔfG°, 128.1 kJ · mol−1
- ^ S°, 138. J · K−1 · mol−1
- ^ ΔfH°, -1065.25 kJ · mol−1
- ^ ΔfG°, -957.36 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 100.50 J · K−1 · mol−1
- ^ ΔfH°, -1130.1 kJ · mol−1
- ^ ΔfG°, -972.7 kJ · mol−1
- ^ S°, -53.6 J · K−1 · mol−1
- ^ Cp°, -243. J · K−1 · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfG°, -985.7 kJ · mol−1
- ^ S°, 36.4 J · K−1 · mol−1
- ^ ΔfH°, -1376.5 kJ · mol−1
- ^ ΔfH°, -1348.1 kJ · mol−1
- ^ ΔfH°, -2258.1 kJ · mol−1
- ^ ΔfH°, -2553.1 kJ · mol−1
- ^ Cp°, 326. J · K−1 · mol−1
- ^ ΔfH°, -3139.3 kJ · mol−1
- ^ ΔfH°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 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