7Cu + 8Mn(NO3)2 + 17H+ → 7Cu(NO3)2 + N2H5+ + 8Mn2+ + 6H2O
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- Reaction of and manganese(II) nitrate under acidic condition
- 7 + 8Mn(NO3)2Manganese(II) nitrate + 17H+Hydrogen ion7Cu(NO3)2Copper(II) nitrate + N2H5+Hydrazinium ion + 8Mn2+Manganese(II) ion + 6H2OWater⟶
The reaction of , manganese(II) nitrate, and hydrogen ion yields copper(II) nitrate, hydrazinium ion, manganese(II) ion, 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 and manganese(II) nitrate under acidic condition
- 7 + 8Mn(NO3)2Manganese(II) nitrate + 17H+Hydrogen ion7Cu(NO3)2Copper(II) nitrate + N2H5+Hydrazinium ion + 8Mn2+Manganese(II) ion + 6H2OWater⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of and manganese(II) nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 7 | Reducing | Oxidizable | ||
| Mn(NO3)2 | Manganese(II) nitrate | 8 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 17 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu(NO3)2 | Copper(II) nitrate | 7 | Oxidized | – |
| N2H5+ | Hydrazinium ion | 1 | Reduced | – |
| Mn2+ | Manganese(II) ion | 8 | – | – |
| H2O | Water | 6 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of and manganese(II) nitrate under acidic condition◆
ΔrG −657.0 kJ/mol K 1.26 × 10115 pK −115.10
| 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 | −854.1 | −657.0 | −641 | – |
| −122.0 | −93.86 | −91.6 | – | |
per 1 mol of | −106.8 | −82.13 | −80.1 | – |
per 1 mol of Hydrogen ion | −50.24 | −38.65 | −37.7 | – |
per 1 mol of | −122.0 | −93.86 | −91.6 | – |
per 1 mol of Hydrazinium ion | −854.1 | −657.0 | −641 | – |
per 1 mol of Manganese(II) ion | −106.8 | −82.13 | −80.1 | – |
per 1 mol of | −142.3 | −109.5 | −107 | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 33.150[1] | 24.435[1] |
| (g) | 338.32[1] | 298.58[1] | 166.38[1] | 20.786[1] |
| Mn(NO3)2 (cr) | -576.26[1] | – | – | – |
| Mn(NO3)2 (ai) | -635.5[1] | -450.9[1] | 218[1] | -121[1] |
| Mn(NO3)2 (vit) 6 hydrate | -2371.9[1] | – | – | – |
| Mn(NO3)2 (l) 6 hydrate | -2331.62[1] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (vit):Vitreous liquid, (l):Liquid, (ao):Un-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 |
|---|---|---|---|---|
| Cu(NO3)2 (cr) | -302.9[1] | – | – | – |
| Cu(NO3)2 (ai) | -349.95[1] | -157.02[1] | 193.3[1] | – |
| Cu(NO3)2 (cr) 3 hydrate | -1217.1[1] | – | – | – |
| Cu(NO3)2 (cr) 6 hydrate | -2110.8[1] | – | – | – |
| N2H5+ (ao) | -7.5[1] | 82.5[1] | 151[1] | 70.3[1] |
| Mn2+ (g) | 2519.69[1] | – | – | – |
| Mn2+ (ao) | -220.75[1] | -228.1[1] | -73.6[1] | 50[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 33.150 J · K−1 · mol−1
- ^ Cp°, 24.435 J · K−1 · mol−1
- ^ ΔfH°, 338.32 kJ · mol−1
- ^ ΔfG°, 298.58 kJ · mol−1
- ^ S°, 166.38 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -576.26 kJ · mol−1
- ^ ΔfH°, -635.5 kJ · mol−1
- ^ ΔfG°, -450.9 kJ · mol−1
- ^ S°, 218. J · K−1 · mol−1
- ^ Cp°, -121. J · K−1 · mol−1
- ^ ΔfH°, -2371.9 kJ · mol−1
- ^ ΔfH°, -2331.62 kJ · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, -302.9 kJ · mol−1
- ^ ΔfH°, -349.95 kJ · mol−1
- ^ ΔfG°, -157.02 kJ · mol−1
- ^ S°, 193.3 J · K−1 · mol−1
- ^ ΔfH°, -1217.1 kJ · mol−1
- ^ ΔfH°, -2110.8 kJ · mol−1
- ^ ΔfH°, -7.5 kJ · mol−1
- ^ ΔfG°, 82.5 kJ · mol−1
- ^ S°, 151. J · K−1 · mol−1
- ^ Cp°, 70.3 J · K−1 · mol−1
- ^ ΔfH°, 2519.69 kJ · mol−1
- ^ ΔfH°, -220.75 kJ · mol−1
- ^ ΔfG°, -228.1 kJ · mol−1
- ^ S°, -73.6 J · K−1 · mol−1
- ^ Cp°, 50. 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