12Na2HPO4 → 8Na3PO4 + O2↑ + P4O10 + 4H3O+ + 4e−
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- Oxidation of sodium hydrogenphosphate
- 12Na2HPO4Sodium hydrogenphosphate8Na3PO4Sodium phosphate + ↑ + P4O10Tetraphosphorus decaoxide + 4H3O+Hydronium ion + 4e−Electron⟶
Oxidation of sodium hydrogenphosphate yields sodium phosphate, , tetraphosphorus decaoxide, hydronium 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 hydrogenphosphate
- 12Na2HPO4Sodium hydrogenphosphate8Na3PO4Sodium phosphate + ↑ + P4O10Tetraphosphorus decaoxide + 4H3O+Hydronium ion + 4e−Electron⟶
General equation
- Oxidation of oxidizable species
- ReactantReducing agent ⟶ ProductOxidation product + e−
Oxidation state of each atom
- Oxidation of sodium hydrogenphosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2HPO4 | Sodium hydrogenphosphate | 12 | Reducing | – |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na3PO4 | Sodium phosphate | 8 | – | – |
| 1 | Oxidized | – | ||
| P4O10 | Tetraphosphorus decaoxide | 1 | – | – |
| H3O+ | Hydronium ion | 4 | – | – |
| e− | Electron | 4 | – | Electron |
Thermodynamic changes
Changes in standard condition (1)
- Oxidation of sodium hydrogenphosphate◆
ΔrG 1273.5 kJ/mol K 0.78 × 10−223 pK 223.11
| 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 | 1158.0 | 1273.5 | −646.8 | – |
per 1 mol of | 96.500 | 106.13 | −53.90 | – |
per 1 mol of | 144.75 | 159.19 | −80.85 | – |
| 1158.0 | 1273.5 | −646.8 | – | |
per 1 mol of | 1158.0 | 1273.5 | −646.8 | – |
per 1 mol of Hydronium ion | 289.50 | 318.38 | −161.7 | – |
per 1 mol of Electron | 289.50 | 318.38 | −161.7 | – |
Changes in standard condition (2)
- Oxidation of sodium hydrogenphosphate◆
ΔrG 1289.9 kJ/mol K 0.10 × 10−225 pK 225.98
| 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 | 1146.3 | 1289.9 | −741.0 | – |
per 1 mol of | 95.525 | 107.49 | −61.75 | – |
per 1 mol of | 143.29 | 161.24 | −92.63 | – |
| 1146.3 | 1289.9 | −741.0 | – | |
per 1 mol of | 1146.3 | 1289.9 | −741.0 | – |
per 1 mol of Hydronium ion | 286.57 | 322.48 | −185.3 | – |
per 1 mol of Electron | 286.57 | 322.48 | −185.3 | – |
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 |
|---|---|---|---|---|
| Na2HPO4 (cr) | -1748.1[1] | -1608.2[1] | 150.50[1] | 135.31[1] |
| Na2HPO4 (ai) | -1772.38[1] | -1612.98[1] | 84.5[1] | – |
| Na2HPO4 (cr) 2 hydrate | -2346.0[1] | -2088.5[1] | 221.3[1] | – |
| Na2HPO4 (cr) 7 hydrate | -3821.7[1] | -3279.8[1] | 434.59[1] | – |
| Na2HPO4 (cr) 12 hydrate | -5297.8[1] | -4467.8[1] | 633.83[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 |
|---|---|---|---|---|
| Na3PO4 (cr) | -1917.40[1] | -1788.80[1] | 173.80[1] | 153.47[1] |
| Na3PO4 (ai) | -1997.9[1] | -1804.5[1] | -43.3[1] | – |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| P4O10 (cr) hexagonal | -2984.0[1] | -2697.7[1] | 228.86[1] | 211.71[1] |
| P4O10 (am) | -3042[1] | – | – | – |
| H3O+ (ao) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| e− | – | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -1748.1 kJ · mol−1
- ^ ΔfG°, -1608.2 kJ · mol−1
- ^ S°, 150.50 J · K−1 · mol−1
- ^ Cp°, 135.31 J · K−1 · mol−1
- ^ ΔfH°, -1772.38 kJ · mol−1
- ^ ΔfG°, -1612.98 kJ · mol−1
- ^ S°, 84.5 J · K−1 · mol−1
- ^ ΔfH°, -2346.0 kJ · mol−1
- ^ ΔfG°, -2088.5 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ ΔfH°, -3821.7 kJ · mol−1
- ^ ΔfG°, -3279.8 kJ · mol−1
- ^ S°, 434.59 J · K−1 · mol−1
- ^ ΔfH°, -5297.8 kJ · mol−1
- ^ ΔfG°, -4467.8 kJ · mol−1
- ^ S°, 633.83 J · K−1 · mol−1
- ^ ΔfH°, -1917.40 kJ · mol−1
- ^ ΔfG°, -1788.80 kJ · mol−1
- ^ S°, 173.80 J · K−1 · mol−1
- ^ Cp°, 153.47 J · K−1 · mol−1
- ^ ΔfH°, -1997.9 kJ · mol−1
- ^ ΔfG°, -1804.5 kJ · mol−1
- ^ S°, -43.3 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 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°, -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