6NaH2PO4 🔥→ 6NaOH + 6P + 3H2O + 5O3↑
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- Decomposition of sodium dihydrogenphosphate
Decomposition of sodium dihydrogenphosphate yields sodium hydroxide, , water, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of sodium dihydrogenphosphate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of sodium dihydrogenphosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaH2PO4 | Sodium dihydrogenphosphate | 6 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaOH | Sodium hydroxide | 6 | – | – |
| 6 | Reduced | – | ||
| H2O | Water | 3 | – | – |
| 5 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of sodium dihydrogenphosphate◆
ΔrG 6144.2 kJ/mol K 0.38 × 10−1076 pK 1076.42
| 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 | 6523.2 | 6144.2 | 1272.71 | 220.99 |
per 1 mol of | 1087.2 | 1024.0 | 212.118 | 36.832 |
per 1 mol of | 1087.2 | 1024.0 | 212.118 | 36.832 |
| 1087.2 | 1024.0 | 212.118 | 36.832 | |
per 1 mol of | 2174.4 | 2048.1 | 424.237 | 73.663 |
| 1304.6 | 1228.8 | 254.542 | 44.198 |
Changes in standard condition (2)
- Decomposition of sodium dihydrogenphosphate◆
ΔrG 6071.6 kJ/mol K 0.20 × 10−1063 pK 1063.70
| 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 | 6417.6 | 6071.6 | 1162.97 | 205.21 |
per 1 mol of | 1069.6 | 1011.9 | 193.828 | 34.202 |
per 1 mol of | 1069.6 | 1011.9 | 193.828 | 34.202 |
| 1069.6 | 1011.9 | 193.828 | 34.202 | |
per 1 mol of | 2139.2 | 2023.9 | 387.657 | 68.403 |
| 1283.5 | 1214.3 | 232.594 | 41.042 |
Changes in standard condition (3)
- Decomposition of sodium dihydrogenphosphate
| 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 | 6287.4 | – | – | – |
per 1 mol of | 1047.9 | – | – | – |
per 1 mol of | 1047.9 | – | – | – |
| 1047.9 | – | – | – | |
per 1 mol of | 2095.8 | – | – | – |
| 1257.5 | – | – | – |
Changes in standard condition (4)
- Decomposition of sodium dihydrogenphosphate
| 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 | 6478.2 | – | – | – |
per 1 mol of | 1079.7 | – | – | – |
per 1 mol of | 1079.7 | – | – | – |
| 1079.7 | – | – | – | |
per 1 mol of | 2159.4 | – | – | – |
| 1295.6 | – | – | – |
Changes in aqueous solution (1)
- Decomposition of sodium dihydrogenphosphate◆
ΔrG 5942.7 kJ/mol K 0.77 × 10−1041 pK 1041.12
| 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 | 6253.8 | 5942.7 | 1043.1 | – |
per 1 mol of | 1042.3 | 990.45 | 173.85 | – |
per 1 mol of | 1042.3 | 990.45 | 173.85 | – |
| 1042.3 | 990.45 | 173.85 | – | |
per 1 mol of | 2084.6 | 1980.9 | 347.70 | – |
| 1250.8 | 1188.5 | 208.62 | – |
Changes in aqueous solution (2)
- Decomposition of sodium dihydrogenphosphate◆
ΔrG 5997.2 kJ/mol K 0.22 × 10−1050 pK 1050.66
| 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 | 6169.8 | 5997.2 | 578 | – |
per 1 mol of | 1028.3 | 999.53 | 96.3 | – |
per 1 mol of | 1028.3 | 999.53 | 96.3 | – |
| 1028.3 | 999.53 | 96.3 | – | |
per 1 mol of | 2056.6 | 1999.1 | 193 | – |
| 1234.0 | 1199.4 | 116 | – |
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 |
|---|---|---|---|---|
| NaOH (cr) | -425.609[1] | -379.494[1] | 64.455[1] | 59.54[1] |
| NaOH (g) | -207.1[1] | -210.0[1] | 228.43[1] | 48.37[1] |
| NaOH (ai) | -470.114[1] | -419.150[1] | 48.1[1] | -102.1[1] |
| NaOH (cr) 1 hydrate | -734.543[1] | -629.338[1] | 99.50[1] | 90.17[1] |
| NaOH (l) 2 hydrate | -1019.076[1] | -873.091[1] | 195.979[1] | 239.41[1] |
| NaOH (l) 3.5 hydrate | -1459.798[1] | -1236.356[1] | 286.089[1] | 354.43[1] |
| NaOH (l) 4 hydrate | -1605.15[1] | -1356.64[1] | 318.70[1] | – |
| NaOH (l) 5 hydrate | -1894.31[1] | -1596.34[1] | 386.06[1] | – |
| NaOH (l) 7 hydrate | -2469.02[1] | -2073.80[1] | 526.31[1] | – |
| (cr) white | 0[1] | 0[1] | 41.09[1] | 23.84[1] |
| (cr) red, triclinic | -17.6[1] | -12.1[1] | 22.80[1] | 21.21[1] |
| (cr) black | -39.3[1] | – | – | – |
| (am) red | -7.5[1] | – | – | – |
| (g) | 314.64[1] | 278.25[1] | 163.193[1] | 20.786[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] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (am):Amorphous solid, (ao):Un-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°, -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°, -425.609 kJ · mol−1
- ^ ΔfG°, -379.494 kJ · mol−1
- ^ S°, 64.455 J · K−1 · mol−1
- ^ Cp°, 59.54 J · K−1 · mol−1
- ^ ΔfH°, -207.1 kJ · mol−1
- ^ ΔfG°, -210.0 kJ · mol−1
- ^ S°, 228.43 J · K−1 · mol−1
- ^ Cp°, 48.37 J · K−1 · mol−1
- ^ ΔfH°, -470.114 kJ · mol−1
- ^ ΔfG°, -419.150 kJ · mol−1
- ^ S°, 48.1 J · K−1 · mol−1
- ^ Cp°, -102.1 J · K−1 · mol−1
- ^ ΔfH°, -734.543 kJ · mol−1
- ^ ΔfG°, -629.338 kJ · mol−1
- ^ S°, 99.50 J · K−1 · mol−1
- ^ Cp°, 90.17 J · K−1 · mol−1
- ^ ΔfH°, -1019.076 kJ · mol−1
- ^ ΔfG°, -873.091 kJ · mol−1
- ^ S°, 195.979 J · K−1 · mol−1
- ^ Cp°, 239.41 J · K−1 · mol−1
- ^ ΔfH°, -1459.798 kJ · mol−1
- ^ ΔfG°, -1236.356 kJ · mol−1
- ^ S°, 286.089 J · K−1 · mol−1
- ^ Cp°, 354.43 J · K−1 · mol−1
- ^ ΔfH°, -1605.15 kJ · mol−1
- ^ ΔfG°, -1356.64 kJ · mol−1
- ^ S°, 318.70 J · K−1 · mol−1
- ^ ΔfH°, -1894.31 kJ · mol−1
- ^ ΔfG°, -1596.34 kJ · mol−1
- ^ S°, 386.06 J · K−1 · mol−1
- ^ ΔfH°, -2469.02 kJ · mol−1
- ^ ΔfG°, -2073.80 kJ · mol−1
- ^ S°, 526.31 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.09 J · K−1 · mol−1
- ^ Cp°, 23.84 J · K−1 · mol−1
- ^ ΔfH°, -17.6 kJ · mol−1
- ^ ΔfG°, -12.1 kJ · mol−1
- ^ S°, 22.80 J · K−1 · mol−1
- ^ Cp°, 21.21 J · K−1 · mol−1
- ^ ΔfH°, -39.3 kJ · mol−1
- ^ ΔfH°, -7.5 kJ · mol−1
- ^ ΔfH°, 314.64 kJ · mol−1
- ^ ΔfG°, 278.25 kJ · mol−1
- ^ S°, 163.193 J · K−1 · mol−1
- ^ Cp°, 20.786 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
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1