6Zn + P4O10 + 6H2O → 2Zn3(PO4)2 + 6H2↑
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- Reaction of , tetraphosphorus decaoxide, and water
The reaction of , tetraphosphorus decaoxide, and water yields zinc phosphate and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of , tetraphosphorus decaoxide, and water
General equation
- Reducing agent + Acidic oxide + H2OOxidizing agent ⟶ SaltOxidation product + Reduction product
Oxidation state of each atom
- Reaction of , tetraphosphorus decaoxide, and water
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 6 | Reducing | Active metal | ||
| P4O10 | Tetraphosphorus decaoxide | 1 | – | Acidic oxide |
| H2O | Water | 6 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn3(PO4)2 | Zinc phosphate | 2 | Oxidized | Salt |
| 6 | Reduced | Hydrogen |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of , 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 | −1085.8 | – | – | – |
| −180.97 | – | – | – | |
per 1 mol of | −1085.8 | – | – | – |
per 1 mol of | −180.97 | – | – | – |
per 1 mol of | −542.90 | – | – | – |
| −180.97 | – | – | – |
Changes in standard condition (2)
- Reaction of , 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 | −1028 | – | – | – |
| −171.3 | – | – | – | |
per 1 mol of | −1028 | – | – | – |
per 1 mol of | −171.3 | – | – | – |
per 1 mol of | −514.0 | – | – | – |
| −171.3 | – | – | – |
Changes in aqueous solution (1)
- Reaction of , 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 | −1085.8 | – | – | – |
| −180.97 | – | – | – | |
per 1 mol of | −1085.8 | – | – | – |
per 1 mol of | −180.97 | – | – | – |
per 1 mol of | −542.90 | – | – | – |
| −180.97 | – | – | – |
Changes in aqueous solution (2)
- Reaction of , 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 | −1111.0 | – | – | – |
| −185.17 | – | – | – | |
per 1 mol of | −1111.0 | – | – | – |
per 1 mol of | −185.17 | – | – | – |
per 1 mol of | −555.50 | – | – | – |
| −185.17 | – | – | – |
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] | 41.63[1] | 25.40[1] |
| (g) | 130.729[1] | 95.145[1] | 160.984[1] | 20.786[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, (g):Gas, (am):Amorphous solid, (l):Liquid
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 |
|---|---|---|---|---|
| Zn3(PO4)2 (cr) | -2892.4[1] | – | – | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.63 J · K−1 · mol−1
- ^ Cp°, 25.40 J · K−1 · mol−1
- ^ ΔfH°, 130.729 kJ · mol−1
- ^ ΔfG°, 95.145 kJ · mol−1
- ^ S°, 160.984 J · K−1 · mol−1
- ^ Cp°, 20.786 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
- ^ 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°, -2892.4 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1