4Na2S + P4O10 + 6H2O → 4NaHS + 4NaH2PO4
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The reaction of sodium sulfide, tetraphosphorus decaoxide, and water yields sodium hydrogensulfide and sodium dihydrogenphosphate (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium sulfide, tetraphosphorus decaoxide, and water
General equation
- SaltBrønsted base + Acidic oxideLewis acid + H2O ⟶ Acid salt
Oxidation state of each atom
- Reaction of sodium sulfide, tetraphosphorus decaoxide, and water
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2S | Sodium sulfide | 4 | Brønsted base | Salt |
| P4O10 | Tetraphosphorus decaoxide | 1 | Lewis acid | Acidic oxide |
| H2O | Water | 6 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHS | Sodium hydrogensulfide | 4 | – | Acid salt |
| NaH2PO4 | Sodium dihydrogenphosphate | 4 | – | Acid salt |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium sulfide, tetraphosphorus decaoxide, and water
| 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 | −937.9 | – | – | – |
per 1 mol of | −234.5 | – | – | – |
per 1 mol of | −937.9 | – | – | – |
per 1 mol of | −156.3 | – | – | – |
per 1 mol of | −234.5 | – | – | – |
per 1 mol of | −234.5 | – | – | – |
Changes in standard condition (2)
- Reaction of sodium sulfide, tetraphosphorus decaoxide, and water
| 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 | −880 | – | – | – |
per 1 mol of | −220 | – | – | – |
per 1 mol of | −880 | – | – | – |
per 1 mol of | −147 | – | – | – |
per 1 mol of | −220 | – | – | – |
per 1 mol of | −220 | – | – | – |
Changes in aqueous solution
- Reaction of sodium sulfide, tetraphosphorus decaoxide, and water◆
ΔrG −695.0 kJ/mol K 5.74 × 10121 pK −121.76
| 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 | −688.4 | −695.0 | 23.3 | – |
per 1 mol of | −172.1 | −173.8 | 5.83 | – |
per 1 mol of | −688.4 | −695.0 | 23.3 | – |
per 1 mol of | −114.7 | −115.8 | 3.88 | – |
per 1 mol of | −172.1 | −173.8 | 5.83 | – |
per 1 mol of | −172.1 | −173.8 | 5.83 | – |
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 |
|---|---|---|---|---|
| Na2S (cr) | -364.8[1] | -349.8[1] | 83.7[1] | – |
| Na2S (ai) | -447.3[1] | -438.1[1] | 103.3[1] | – |
| Na2S (cr) 4.5 hydrate | -1725.9[1] | – | – | – |
| Na2S (cr) 5 hydrate | -1886.6[1] | – | – | – |
| Na2S (cr) 9 hydrate | -3074.0[1] | – | – | – |
| P4O10 (cr) hexagonal | -2984.0[1] | -2697.7[1] | 228.86[1] | 211.71[1] |
| P4O10 (am) | -3042[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, (am):Amorphous solid, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| NaHS (cr) | -237.23[1] | – | – | – |
| NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
| NaHS (cr) 2 hydrate | -838.47[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
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°, -364.8 kJ · mol−1
- ^ ΔfG°, -349.8 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ ΔfH°, -447.3 kJ · mol−1
- ^ ΔfG°, -438.1 kJ · mol−1
- ^ S°, 103.3 J · K−1 · mol−1
- ^ ΔfH°, -1725.9 kJ · mol−1
- ^ ΔfH°, -1886.6 kJ · mol−1
- ^ ΔfH°, -3074.0 kJ · 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
- ^ 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
- ^ ΔfH°, -237.23 kJ · mol−1
- ^ ΔfH°, -257.73 kJ · mol−1
- ^ ΔfG°, -249.81 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -838.47 kJ · mol−1
- ^ 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