5CH3COONH4 + 4MnO2 → 2MnCO3 + 2Mn(CH3COO)2 + 4H2O + 5NH3↑
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The reaction of ammonium acetate and manganese(IV) oxide yields manganese(II) carbonate, manganese(II) acetate, 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
- 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 | 5 | Reducing | Reducing |
MnO2 | Manganese(IV) oxide | 4 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MnCO3 | Manganese(II) carbonate | 2 | Redoxed product | – |
Mn(CH3COO)2 | Manganese(II) acetate | 2 | Reduced | – |
H2O | Water | 4 | – | – |
NH3 | Ammonia | 5 | – | – |
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 | −297.5 | – | – | – |
per 1 mol of | −59.50 | – | – | – |
per 1 mol of | −74.38 | – | – | – |
per 1 mol of | −148.8 | – | – | – |
per 1 mol of | −148.8 | – | – | – |
per 1 mol of | −74.38 | – | – | – |
per 1 mol of | −59.50 | – | – | – |
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 | −275.7 | – | – | – |
per 1 mol of | −55.14 | – | – | – |
per 1 mol of | −68.92 | – | – | – |
per 1 mol of | −137.8 | – | – | – |
per 1 mol of | −137.8 | – | – | – |
per 1 mol of | −68.92 | – | – | – |
per 1 mol of | −55.14 | – | – | – |
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 | −367.6 | – | – | – |
per 1 mol of | −73.52 | – | – | – |
per 1 mol of | −91.90 | – | – | – |
per 1 mol of | −183.8 | – | – | – |
per 1 mol of | −183.8 | – | – | – |
per 1 mol of | −91.90 | – | – | – |
per 1 mol of | −73.52 | – | – | – |
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 | −345.8 | – | – | – |
per 1 mol of | −69.16 | – | – | – |
per 1 mol of | −86.45 | – | – | – |
per 1 mol of | −172.9 | – | – | – |
per 1 mol of | −172.9 | – | – | – |
per 1 mol of | −86.45 | – | – | – |
per 1 mol of | −69.16 | – | – | – |
Changes in aqueous solution (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 | −387.6 | – | – | – |
per 1 mol of | −77.52 | – | – | – |
per 1 mol of | −96.90 | – | – | – |
per 1 mol of | −193.8 | – | – | – |
per 1 mol of | −193.8 | – | – | – |
per 1 mol of | −96.90 | – | – | – |
per 1 mol of | −77.52 | – | – | – |
Changes in aqueous solution (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 | −558.5 | – | – | – |
per 1 mol of | −111.7 | – | – | – |
per 1 mol of | −139.6 | – | – | – |
per 1 mol of | −279.3 | – | – | – |
per 1 mol of | −279.3 | – | – | – |
per 1 mol of | −139.6 | – | – | – |
per 1 mol of | −111.7 | – | – | – |
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 |
---|---|---|---|---|
MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
MnCO3 (cr) precipitated | -883.2[1] | – | – | – |
Mn(CH3COO)2 (cr) | -1148.1[1] | – | – | – |
Mn(CH3COO)2 (aq) | -1199.1[1] | – | – | – |
Mn(CH3COO)2 (cr) 4 hydrate | -2338.0[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] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (l):Liquid, (g):Gas, (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°, -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°, -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°, -1148.1 kJ · mol−1
- ^ ΔfH°, -1199.1 kJ · mol−1
- ^ ΔfH°, -2338.0 kJ · 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