2CH3COONH4 + 12MnO2 → NH4NO3 + 4MnCO3 + 5Mn(OH)2 + 3MnO
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The reaction of ammonium acetate and manganese(IV) oxide yields ammonium nitrate, manganese(II) carbonate, manganese(II) hydroxide, and manganese(II) oxide (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 acetate 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 acetate and manganese(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COONH4 | Ammonium acetate | 2 | Reducing | Reducing |
| MnO2 | Manganese(IV) oxide | 12 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO3 | Ammonium nitrate | 1 | Oxidized | – |
| MnCO3 | Manganese(II) carbonate | 4 | Redoxed product | – |
| Mn(OH)2 | Manganese(II) hydroxide | 5 | Reduced | – |
| MnO | Manganese(II) oxide | 3 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of ammonium acetate 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 | −1102.0 | – | – | – |
per 1 mol of | −551.00 | – | – | – |
per 1 mol of | −91.833 | – | – | – |
per 1 mol of | −1102.0 | – | – | – |
per 1 mol of | −275.50 | – | – | – |
per 1 mol of | −220.40 | – | – | – |
per 1 mol of | −367.33 | – | – | – |
Changes in standard condition (2)
- Reaction of ammonium acetate 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 | −1058.4 | – | – | – |
per 1 mol of | −529.20 | – | – | – |
per 1 mol of | −88.200 | – | – | – |
per 1 mol of | −1058.4 | – | – | – |
per 1 mol of | −264.60 | – | – | – |
per 1 mol of | −211.68 | – | – | – |
per 1 mol of | −352.80 | – | – | – |
Changes in standard condition (3)
- Reaction of ammonium acetate 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 | −1312.3 | – | – | – |
per 1 mol of | −656.15 | – | – | – |
per 1 mol of | −109.36 | – | – | – |
per 1 mol of | −1312.3 | – | – | – |
per 1 mol of | −328.07 | – | – | – |
per 1 mol of | −262.46 | – | – | – |
per 1 mol of | −437.43 | – | – | – |
Changes in standard condition (4)
- Reaction of ammonium acetate 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 | −1268.7 | – | – | – |
per 1 mol of | −634.35 | – | – | – |
per 1 mol of | −105.73 | – | – | – |
per 1 mol of | −1268.7 | – | – | – |
per 1 mol of | −317.18 | – | – | – |
per 1 mol of | −253.74 | – | – | – |
per 1 mol of | −422.90 | – | – | – |
Changes in aqueous solution
- Reaction of ammonium acetate and manganese(IV) oxide◆
ΔrG −1142.2 kJ/mol K 1.27 × 10200 pK −200.10
| 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 | −1071.5 | −1142.2 | 241.5 | – |
per 1 mol of | −535.75 | −571.10 | 120.8 | – |
per 1 mol of | −89.292 | −95.183 | 20.13 | – |
per 1 mol of | −1071.5 | −1142.2 | 241.5 | – |
per 1 mol of | −267.88 | −285.55 | 60.38 | – |
per 1 mol of | −214.30 | −228.44 | 48.30 | – |
per 1 mol of | −357.17 | −380.73 | 80.50 | – |
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 |
|---|---|---|---|---|
| CH3COONH4 (cr) | -616.14[1] | – | – | – |
| CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[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 |
|---|---|---|---|---|
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
| MnCO3 (cr) precipitated | -883.2[1] | – | – | – |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (g):Gas
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°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 J · K−1 · 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°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1
- ^ ΔfH°, -894.1 kJ · mol−1
- ^ ΔfG°, -816.7 kJ · mol−1
- ^ S°, 85.8 J · K−1 · mol−1
- ^ Cp°, 81.50 J · K−1 · mol−1
- ^ ΔfH°, -883.2 kJ · mol−1
- ^ ΔfH°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1