6CuO + P4O10 → 2Cu3(PO4)2
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The reaction of copper(II) oxide and tetraphosphorus decaoxide yields copper(II) phosphate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of copper(II) oxide and tetraphosphorus decaoxide
General equation
- Reaction of basic oxide and acidic oxide
- Basic oxideLewis base + Acidic oxideLewis acid ⟶ Oxoacid saltLewis conjugate
- Reaction of weakly basic oxide and weakly acidic oxide
- Weakly basic oxideLewis base + Weakly acidic oxideLewis acid ⟶ Salt of weak acid and weak baseLewis conjugate
Oxidation state of each atom
- Reaction of copper(II) oxide and tetraphosphorus decaoxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuO | Copper(II) oxide | 6 | Lewis base | Basic oxide Weakly basic oxide |
| P4O10 | Tetraphosphorus decaoxide | 1 | Lewis acid | Acidic oxide Weakly acidic oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu3(PO4)2 | Copper(II) phosphate | 2 | Lewis conjugate | Oxoacid salt Salt of weak acid and weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of copper(II) oxide and tetraphosphorus decaoxide◆
ΔrG −626.7 kJ/mol K 6.21 × 10109 pK −109.79
| 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 | – | −626.7 | – | – |
per 1 mol of | – | −104.5 | – | – |
per 1 mol of | – | −626.7 | – | – |
per 1 mol of | – | −313.4 | – | – |
Changes in standard condition (2)
- Reaction of copper(II) oxide and tetraphosphorus decaoxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution
- Reaction of copper(II) oxide and tetraphosphorus decaoxide◆
ΔrG −626.7 kJ/mol K 6.21 × 10109 pK −109.79
| 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 | – | −626.7 | – | – |
per 1 mol of | – | −104.5 | – | – |
per 1 mol of | – | −626.7 | – | – |
per 1 mol of | – | −313.4 | – | – |
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 |
|---|---|---|---|---|
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[1] |
| P4O10 (cr) hexagonal | -2984.0[1] | -2697.7[1] | 228.86[1] | 211.71[1] |
| P4O10 (am) | -3042[1] | – | – | – |
* (cr):Crystalline solid, (am):Amorphous solid
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 |
|---|---|---|---|---|
| Cu3(PO4)2 (cr) | – | -2051.3[1] | – | – |
* (cr):Crystalline 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)