3CuSO4 + 2H3PO4 🔥→ Cu3(PO4)2 + 3SO3 + 3H2O
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The reaction of copper(II) sulfate and phosphoric acid yields copper(II) phosphate, sulfur trioxide, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of copper(II) sulfate and phosphoric acid
General equation
- Oxoacid saltBrønsted base + Dehydrating acidBrønsted acid ⟶ SaltConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of copper(II) sulfate and phosphoric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CuSO4 | Copper(II) sulfate | 3 | Brønsted base | Oxoacid salt |
H3PO4 | Phosphoric acid | 2 | Brønsted acid | Dehydrating acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cu3(PO4)2 | Copper(II) phosphate | 1 | Conjugate base | Salt |
SO3 | Sulfur trioxide | 3 | – | Acidic oxide |
H2O | Water | 3 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 339.7 kJ/mol K 0.31 × 10−59 pK 59.51
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 | – | 339.7 | – | – |
per 1 mol of | – | 113.2 | – | – |
per 1 mol of | – | 169.8 | – | – |
per 1 mol of | – | 339.7 | – | – |
per 1 mol of | – | 113.2 | – | – |
per 1 mol of | – | 113.2 | – | – |
Changes in aqueous solution (1)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 476.3 kJ/mol K 0.36 × 10−83 pK 83.44
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 | – | 476.3 | – | – |
per 1 mol of | – | 158.8 | – | – |
per 1 mol of | – | 238.2 | – | – |
per 1 mol of | – | 476.3 | – | – |
per 1 mol of | – | 158.8 | – | – |
per 1 mol of | – | 158.8 | – | – |
Changes in aqueous solution (2)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 228.6 kJ/mol K 0.89 × 10−40 pK 40.05
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 | – | 228.6 | – | – |
per 1 mol of | – | 76.20 | – | – |
per 1 mol of | – | 114.3 | – | – |
per 1 mol of | – | 228.6 | – | – |
per 1 mol of | – | 76.20 | – | – |
per 1 mol of | – | 76.20 | – | – |
Changes in aqueous solution (3)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 476.3 kJ/mol K 0.36 × 10−83 pK 83.44
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 | – | 476.3 | – | – |
per 1 mol of | – | 158.8 | – | – |
per 1 mol of | – | 238.2 | – | – |
per 1 mol of | – | 476.3 | – | – |
per 1 mol of | – | 158.8 | – | – |
per 1 mol of | – | 158.8 | – | – |
Changes in aqueous solution (4)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 385.2 kJ/mol K 0.33 × 10−67 pK 67.48
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 | – | 385.2 | – | – |
per 1 mol of | – | 128.4 | – | – |
per 1 mol of | – | 192.6 | – | – |
per 1 mol of | – | 385.2 | – | – |
per 1 mol of | – | 128.4 | – | – |
per 1 mol of | – | 128.4 | – | – |
Changes in aqueous solution (5)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 137.5 kJ/mol K 0.81 × 10−24 pK 24.09
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 | – | 137.5 | – | – |
per 1 mol of | – | 45.83 | – | – |
per 1 mol of | – | 68.75 | – | – |
per 1 mol of | – | 137.5 | – | – |
per 1 mol of | – | 45.83 | – | – |
per 1 mol of | – | 45.83 | – | – |
Changes in aqueous solution (6)
- Reaction of copper(II) sulfate and phosphoric acid◆
ΔrG 385.2 kJ/mol K 0.33 × 10−67 pK 67.48
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 | – | 385.2 | – | – |
per 1 mol of | – | 128.4 | – | – |
per 1 mol of | – | 192.6 | – | – |
per 1 mol of | – | 385.2 | – | – |
per 1 mol of | – | 128.4 | – | – |
per 1 mol of | – | 128.4 | – | – |
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 |
---|---|---|---|---|
CuSO4 (cr) | -771.36[1] | -661.8[1] | 109[1] | 100.0[1] |
CuSO4 (ai) | -844.50[1] | -679.04[1] | -79.5[1] | – |
CuSO4 (ao) | – | -692.18[1] | – | – |
CuSO4 (cr) 1 hydrate | -1085.83[1] | -918.11[1] | 146.0[1] | 134[1] |
CuSO4 (cr) 3 hydrate | -1684.31[1] | -1399.96[1] | 221.3[1] | 205[1] |
CuSO4 (cr) 5 hydrate | -2279.65[1] | -1879.745[1] | 300.4[1] | 280[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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 |
---|---|---|---|---|
Cu3(PO4)2 (cr) | – | -2051.3[1] | – | – |
SO3 (cr) β | -454.51[1] | -374.21[1] | 70.7[1] | – |
SO3 (l) | -441.04[1] | -373.75[1] | 113.8[1] | – |
SO3 (g) | -395.72[1] | -371.06[1] | 256.76[1] | 50.67[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, (l):Liquid, (g):Gas
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°, -771.36 kJ · mol−1
- ^ ΔfG°, -661.8 kJ · mol−1
- ^ S°, 109. J · K−1 · mol−1
- ^ Cp°, 100.0 J · K−1 · mol−1
- ^ ΔfH°, -844.50 kJ · mol−1
- ^ ΔfG°, -679.04 kJ · mol−1
- ^ S°, -79.5 J · K−1 · mol−1
- ^ ΔfG°, -692.18 kJ · mol−1
- ^ ΔfH°, -1085.83 kJ · mol−1
- ^ ΔfG°, -918.11 kJ · mol−1
- ^ S°, 146.0 J · K−1 · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, -1684.31 kJ · mol−1
- ^ ΔfG°, -1399.96 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ Cp°, 205. J · K−1 · mol−1
- ^ ΔfH°, -2279.65 kJ · mol−1
- ^ ΔfG°, -1879.745 kJ · mol−1
- ^ S°, 300.4 J · K−1 · mol−1
- ^ Cp°, 280. 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
- ^ ΔfG°, -2051.3 kJ · mol−1
- ^ ΔfH°, -454.51 kJ · mol−1
- ^ ΔfG°, -374.21 kJ · mol−1
- ^ S°, 70.7 J · K−1 · mol−1
- ^ ΔfH°, -441.04 kJ · mol−1
- ^ ΔfG°, -373.75 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -395.72 kJ · mol−1
- ^ ΔfG°, -371.06 kJ · mol−1
- ^ S°, 256.76 J · K−1 · mol−1
- ^ Cp°, 50.67 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