4NaH2PO4 → 4Na+ + 3O22− + P4O10 + 8H+ + 6e−
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- Oxidation of sodium dihydrogenphosphate
- 4NaH2PO4Sodium dihydrogenphosphate4Na+Sodium ion + 3O22−Peroxide ion + P4O10Tetraphosphorus decaoxide + 8H+Hydrogen ion + 6e−Electron⟶
Oxidation of sodium dihydrogenphosphate yields sodium ion, peroxide ion, tetraphosphorus decaoxide, hydrogen ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Oxidation of sodium dihydrogenphosphate
- 4NaH2PO4Sodium dihydrogenphosphate4Na+Sodium ion + 3O22−Peroxide ion + P4O10Tetraphosphorus decaoxide + 8H+Hydrogen ion + 6e−Electron⟶
General equation
- Oxidation of oxidizable species
- ReactantReducing agent ⟶ ProductOxidation product + e−
Oxidation state of each atom
- Oxidation of sodium dihydrogenphosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaH2PO4 | Sodium dihydrogenphosphate | 4 | Reducing | – |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na+ | Sodium ion | 4 | – | – |
| O22− | Peroxide ion | 3 | Oxidized | – |
| P4O10 | Tetraphosphorus decaoxide | 1 | – | – |
| H+ | Hydrogen ion | 8 | – | – |
| e− | Electron | 6 | – | Electron |
Thermodynamic changes
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 |
|---|---|---|---|---|
| NaH2PO4 (cr) | -1536.8[1] | -1386.1[1] | 127.49[1] | 116.86[1] |
| NaH2PO4 (ai) | -1536.41[1] | -1392.17[1] | 149.4[1] | – |
| NaH2PO4 (cr) 1 hydrate | -1833.0[1] | – | – | – |
| NaH2PO4 (cr) 2 hydrate | -2128.4[1] | – | – | – |
* (cr):Crystalline solid, (ai):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 |
|---|---|---|---|---|
| Na+ (g) | 609.358[1] | – | – | – |
| Na+ (ao) | -240.12[1] | -261.905[1] | 59.0[1] | 46.4[1] |
| O22− | – | – | – | – |
| P4O10 (cr) hexagonal | -2984.0[1] | -2697.7[1] | 228.86[1] | 211.71[1] |
| P4O10 (am) | -3042[1] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
| e− | – | – | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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°, -1536.8 kJ · mol−1
- ^ ΔfG°, -1386.1 kJ · mol−1
- ^ S°, 127.49 J · K−1 · mol−1
- ^ Cp°, 116.86 J · K−1 · mol−1
- ^ ΔfH°, -1536.41 kJ · mol−1
- ^ ΔfG°, -1392.17 kJ · mol−1
- ^ S°, 149.4 J · K−1 · mol−1
- ^ ΔfH°, -1833.0 kJ · mol−1
- ^ ΔfH°, -2128.4 kJ · mol−1
- ^ ΔfH°, 609.358 kJ · mol−1
- ^ ΔfH°, -240.12 kJ · mol−1
- ^ ΔfG°, -261.905 kJ · mol−1
- ^ S°, 59.0 J · K−1 · mol−1
- ^ Cp°, 46.4 J · K−1 · mol−1
- ^ ΔfH°, -2984.0 kJ · mol−1
- ^ ΔfG°, -2697.7 kJ · mol−1
- ^ S°, 228.86 J · K−1 · mol−1
- ^ Cp°, 211.71 J · K−1 · mol−1
- ^ ΔfH°, -3042. 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