MnCl2 + 12HNO3 🔥→ MnO2 + 2ClO2↑ + 6N2O4 + 6H2O
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The reaction of manganese(II) chloride and nitric acid yields manganese(IV) oxide, chlorine dioxide, dinitrogen tetraoxide, 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 manganese(II) chloride and nitric acid
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of manganese(II) chloride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnCl2 | Manganese(II) chloride | 1 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 12 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnO2 | Manganese(IV) oxide | 1 | Oxidized | – |
| ClO2 | Chlorine dioxide | 2 | Oxidized | – |
| N2O4 | Dinitrogen tetraoxide | 6 | Reduced | – |
| H2O | Water | 6 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of manganese(II) chloride and nitric acid◆
ΔrG 347.3 kJ/mol K 0.14 × 10−60 pK 60.84
| 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 | 423.5 | 347.3 | 256.0 | 54.7 |
per 1 mol of | 423.5 | 347.3 | 256.0 | 54.7 |
per 1 mol of | 35.29 | 28.94 | 21.33 | 4.56 |
per 1 mol of | 423.5 | 347.3 | 256.0 | 54.7 |
per 1 mol of | 211.8 | 173.7 | 128.0 | 27.4 |
per 1 mol of | 70.58 | 57.88 | 42.67 | 9.12 |
per 1 mol of | 70.58 | 57.88 | 42.67 | 9.12 |
Changes in standard condition (2)
- Reaction of manganese(II) chloride and nitric acid
| 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 | 441.0 | – | – | – |
per 1 mol of | 441.0 | – | – | – |
per 1 mol of | 36.75 | – | – | – |
per 1 mol of | 441.0 | – | – | – |
per 1 mol of | 220.5 | – | – | – |
per 1 mol of | 73.50 | – | – | – |
per 1 mol of | 73.50 | – | – | – |
Changes in aqueous solution (1)
- Reaction of manganese(II) chloride and nitric acid◆
ΔrG 764.1 kJ/mol K 0.14 × 10−133 pK 133.86
| 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 | 896.4 | 764.1 | 445.7 | 2707 |
per 1 mol of | 896.4 | 764.1 | 445.7 | 2707 |
per 1 mol of | 74.70 | 63.68 | 37.14 | 225.6 |
per 1 mol of | 896.4 | 764.1 | 445.7 | 2707 |
per 1 mol of | 448.2 | 382.1 | 222.8 | 1354 |
per 1 mol of | 149.4 | 127.4 | 74.28 | 451.2 |
per 1 mol of | 149.4 | 127.4 | 74.28 | 451.2 |
Changes in aqueous solution (2)
- Reaction of manganese(II) chloride and nitric acid◆
ΔrG 763.3 kJ/mol K 0.19 × 10−133 pK 133.72
| 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 | 841.2 | 763.3 | 261.6 | – |
per 1 mol of | 841.2 | 763.3 | 261.6 | – |
per 1 mol of | 70.10 | 63.61 | 21.80 | – |
per 1 mol of | 841.2 | 763.3 | 261.6 | – |
per 1 mol of | 420.6 | 381.6 | 130.8 | – |
per 1 mol of | 140.2 | 127.2 | 43.60 | – |
per 1 mol of | 140.2 | 127.2 | 43.60 | – |
Changes in aqueous solution (3)
- Reaction of manganese(II) chloride and nitric acid◆
ΔrG 765.3 kJ/mol K 0.84 × 10−134 pK 134.07
| 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 | – | 765.3 | – | – |
per 1 mol of | – | 765.3 | – | – |
per 1 mol of | – | 63.77 | – | – |
per 1 mol of | – | 765.3 | – | – |
per 1 mol of | – | 382.6 | – | – |
per 1 mol of | – | 127.5 | – | – |
per 1 mol of | – | 127.5 | – | – |
Changes in aqueous solution (4)
- Reaction of manganese(II) chloride and nitric acid◆
ΔrG 764.5 kJ/mol K 0.12 × 10−133 pK 133.93
| 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 | – | 764.5 | – | – |
per 1 mol of | – | 764.5 | – | – |
per 1 mol of | – | 63.71 | – | – |
per 1 mol of | – | 764.5 | – | – |
per 1 mol of | – | 382.3 | – | – |
per 1 mol of | – | 127.4 | – | – |
per 1 mol of | – | 127.4 | – | – |
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 |
|---|---|---|---|---|
| MnCl2 (cr) | -481.29[1] | -440.50[1] | 118.24[1] | 72.93[1] |
| MnCl2 (g) | -263.6[1] | – | – | – |
| MnCl2 (ai) | -555.05[1] | -490.8[1] | 38.9[1] | -222[1] |
| MnCl2 (ao) | – | -492.0[1] | – | – |
| MnCl2 (cr) 1 hydrate | -789.9[1] | -696.1[1] | 174.1[1] | – |
| MnCl2 (cr) 2 hydrate | -1092.0[1] | -942.1[1] | 218.8[1] | – |
| MnCl2 (cr) 4 hydrate | -1687.4[1] | -1423.6[1] | 303.3[1] | – |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
| ClO2 (g) | 102.5[1] | 120.5[1] | 256.84[1] | 41.97[1] |
| ClO2 (ao) | 74.9[1] | 120.1[1] | 164.8[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] |
| 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] |
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -481.29 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 118.24 J · K−1 · mol−1
- ^ Cp°, 72.93 J · K−1 · mol−1
- ^ ΔfH°, -263.6 kJ · mol−1
- ^ ΔfH°, -555.05 kJ · mol−1
- ^ ΔfG°, -490.8 kJ · mol−1
- ^ S°, 38.9 J · K−1 · mol−1
- ^ Cp°, -222. J · K−1 · mol−1
- ^ ΔfG°, -492.0 kJ · mol−1
- ^ ΔfH°, -789.9 kJ · mol−1
- ^ ΔfG°, -696.1 kJ · mol−1
- ^ S°, 174.1 J · K−1 · mol−1
- ^ ΔfH°, -1092.0 kJ · mol−1
- ^ ΔfG°, -942.1 kJ · mol−1
- ^ S°, 218.8 J · K−1 · mol−1
- ^ ΔfH°, -1687.4 kJ · mol−1
- ^ ΔfG°, -1423.6 kJ · mol−1
- ^ S°, 303.3 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 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°, 102.5 kJ · mol−1
- ^ ΔfG°, 120.5 kJ · mol−1
- ^ S°, 256.84 J · K−1 · mol−1
- ^ Cp°, 41.97 J · K−1 · mol−1
- ^ ΔfH°, 74.9 kJ · mol−1
- ^ ΔfG°, 120.1 kJ · mol−1
- ^ S°, 164.8 J · K−1 · 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°, -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