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3CuSO4 + 2H3PO4 🔥→ Cu3(PO4)2 + 3SO3 + 3H2O

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
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Reaction of oxoacid salt and dehydrating acid
Oxoacid saltBrønsted base + Dehydrating acidBrønsted acid
SaltConjugate base + Acidic oxide + H2OConjugate acid

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuSO4Copper(II) sulfate3
Brønsted base
Oxoacid salt
H3PO4Phosphoric acid2
Brønsted acid
Dehydrating acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu3(PO4)2Copper(II) phosphate1
Conjugate base
Salt
SO3Sulfur trioxide3
Acidic oxide
H2OWater3
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of copper(II) sulfate and phosphoric acid
ΔrG339.7 kJ/mol
K0.31 × 10−59
pK59.51
3CuSO4Crystalline solid + 2H3PO4Crystalline solid
🔥
Cu3(PO4)2Crystalline solid + 3SO3Liquid + 3H2OLiquid
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
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
ΔrG476.3 kJ/mol
K0.36 × 10−83
pK83.44
3CuSO4Un-ionized aqueous solution + 2H3PO4Un-ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
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
ΔrG228.6 kJ/mol
K0.89 × 10−40
pK40.05
3CuSO4Un-ionized aqueous solution + 2H3PO4Ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
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
ΔrG476.3 kJ/mol
K0.36 × 10−83
pK83.44
3CuSO4Un-ionized aqueous solution + 2H3PO4Un-ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
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
ΔrG385.2 kJ/mol
K0.33 × 10−67
pK67.48
3CuSO4Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
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
ΔrG137.5 kJ/mol
K0.81 × 10−24
pK24.09
3CuSO4Crystalline solid + 2H3PO4Ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
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
ΔrG385.2 kJ/mol
K0.33 × 10−67
pK67.48
3CuSO4Crystalline solid + 2H3PO4Un-ionized aqueous solution
🔥
Cu3(PO4)2Crystalline solid + 3SO3Crystalline solidβ + 3H2OLiquid
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
385.2
per 1 mol of
128.4
per 1 mol of
128.4

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)