8Na + 5H3PO4 → 4Na2HPO4 + PH3↑ + 4H2O
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- Reaction of and phosphoric acid
The reaction of and phosphoric acid yields sodium hydrogenphosphate, , 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 phosphoric acid
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 and phosphoric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 8 | Reducing | Reducing | ||
| H3PO4 | Phosphoric acid | 5 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2HPO4 | Sodium hydrogenphosphate | 4 | Oxidized | – |
| 1 | Reduced | – | ||
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and phosphoric acid◆
ΔrG −1772.4 kJ/mol K 3.24 × 10310 pK −310.51
| 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 | −1735.3 | −1772.4 | 129.69 | 123.29 |
| −216.91 | −221.55 | 16.211 | 15.411 | |
per 1 mol of | −347.06 | −354.48 | 25.938 | 24.658 |
per 1 mol of | −433.82 | −443.10 | 32.422 | 30.823 |
| −1735.3 | −1772.4 | 129.69 | 123.29 | |
per 1 mol of | −433.82 | −443.10 | 32.422 | 30.823 |
Changes in aqueous solution (1)
- Reaction of and phosphoric acid◆
ΔrG −1674.3 kJ/mol K 2.11 × 10293 pK −293.32
| 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 | −1785.7 | −1674.3 | −372.8 | – |
| −223.21 | −209.29 | −46.60 | – | |
per 1 mol of | −357.14 | −334.86 | −74.56 | – |
per 1 mol of | −446.43 | −418.57 | −93.20 | – |
| −1785.7 | −1674.3 | −372.8 | – | |
per 1 mol of | −446.43 | −418.57 | −93.20 | – |
Changes in aqueous solution (2)
- Reaction of and phosphoric acid◆
ΔrG −1662.38 kJ/mol K 1.72 × 10291 pK −291.24
| 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 | −1800.64 | −1662.38 | −462.9 | – |
| −225.080 | −207.798 | −57.86 | – | |
per 1 mol of | −360.128 | −332.476 | −92.58 | – |
per 1 mol of | −450.160 | −415.595 | −115.7 | – |
| −1800.64 | −1662.38 | −462.9 | – | |
per 1 mol of | −450.160 | −415.595 | −115.7 | – |
Changes in aqueous solution (3)
- Reaction of and phosphoric acid◆
ΔrG −2293.5 kJ/mol K 6.37 × 10401 pK −401.80
| 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 | −1840.4 | −2293.5 | 1519.7 | – |
| −230.05 | −286.69 | 189.96 | – | |
per 1 mol of | −368.08 | −458.70 | 303.94 | – |
per 1 mol of | −460.10 | −573.38 | 379.93 | – |
| −1840.4 | −2293.5 | 1519.7 | – | |
per 1 mol of | −460.10 | −573.38 | 379.93 | – |
Changes in aqueous solution (4)
- Reaction of and phosphoric acid◆
ΔrG −2281.6 kJ/mol K 5.24 × 10399 pK −399.72
| 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 | −1855.3 | −2281.6 | 1429.6 | – |
| −231.91 | −285.20 | 178.70 | – | |
per 1 mol of | −371.06 | −456.32 | 285.92 | – |
per 1 mol of | −463.82 | −570.40 | 357.40 | – |
| −1855.3 | −2281.6 | 1429.6 | – | |
per 1 mol of | −463.82 | −570.40 | 357.40 | – |
Changes in aqueous solution (5)
- Reaction of and phosphoric acid◆
ΔrG −1674.3 kJ/mol K 2.11 × 10293 pK −293.32
| 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 | −1785.7 | −1674.3 | −372.8 | – |
| −223.21 | −209.29 | −46.60 | – | |
per 1 mol of | −357.14 | −334.86 | −74.56 | – |
per 1 mol of | −446.43 | −418.57 | −93.20 | – |
| −1785.7 | −1674.3 | −372.8 | – | |
per 1 mol of | −446.43 | −418.57 | −93.20 | – |
Changes in aqueous solution (6)
- Reaction of and phosphoric acid◆
ΔrG −1662.38 kJ/mol K 1.72 × 10291 pK −291.24
| 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 | −1800.64 | −1662.38 | −462.9 | – |
| −225.080 | −207.798 | −57.86 | – | |
per 1 mol of | −360.128 | −332.476 | −92.58 | – |
per 1 mol of | −450.160 | −415.595 | −115.7 | – |
| −1800.64 | −1662.38 | −462.9 | – | |
per 1 mol of | −450.160 | −415.595 | −115.7 | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 51.21[1] | 28.24[1] |
| (g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
| H3PO4 (cr) | -1279.0[1] | -1119.1[1] | 110.50[1] | 106.06[1] |
| H3PO4 (l) | -1266.9[1] | – | – | – |
| H3PO4 (ai) | -1277.4[1] | -1018.7[1] | -220.3[1] | – |
| H3PO4 (ao) | -1288.34[1] | -1142.54[1] | 158.2[1] | – |
| H3PO4 (cr) 0.5 hydrate | -1431.3[1] | -1242.1[1] | 129.16[1] | 126.02[1] |
| H3PO4 (cr) 1 hydrate | -1568.83[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| 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] | – |
| (g) | 5.4[1] | 13.4[1] | 210.23[1] | 37.11[1] |
| (ao) | -9.50[1] | 25.36[1] | 120.1[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, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 51.21 J · K−1 · mol−1
- ^ Cp°, 28.24 J · K−1 · mol−1
- ^ ΔfH°, 107.32 kJ · mol−1
- ^ ΔfG°, 76.761 kJ · mol−1
- ^ S°, 153.712 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -1279.0 kJ · mol−1
- ^ ΔfG°, -1119.1 kJ · mol−1
- ^ S°, 110.50 J · K−1 · mol−1
- ^ Cp°, 106.06 J · K−1 · mol−1
- ^ ΔfH°, -1266.9 kJ · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1
- ^ ΔfH°, -1288.34 kJ · mol−1
- ^ ΔfG°, -1142.54 kJ · mol−1
- ^ S°, 158.2 J · K−1 · mol−1
- ^ ΔfH°, -1431.3 kJ · mol−1
- ^ ΔfG°, -1242.1 kJ · mol−1
- ^ S°, 129.16 J · K−1 · mol−1
- ^ Cp°, 126.02 J · K−1 · mol−1
- ^ ΔfH°, -1568.83 kJ · mol−1
- ^ 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°, 5.4 kJ · mol−1
- ^ ΔfG°, 13.4 kJ · mol−1
- ^ S°, 210.23 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -9.50 kJ · mol−1
- ^ ΔfG°, 25.36 kJ · mol−1
- ^ S°, 120.1 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