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2FePO4 + 3H2SO4 → Fe2(SO4)3 + 2H3PO4

The reaction of iron(III) phosphate and sulfuric acid yields iron(III) sulfate and phosphoric acid (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FePO4Iron(III) phosphate2
Brønsted base
Salt of weak acid
H2SO4Sulfuric acid3
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe2(SO4)3Iron(III) sulfate1
Conjugate base
Salt of strong acid
H3PO4Phosphoric acid2
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of iron(III) phosphate and sulfuric acid
2FePO4Crystalline solid + 3H2SO4Liquid
Fe2(SO4)3Crystalline solid + 2H3PO4Crystalline solid
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
−102.5
−51.25
per 1 mol of
−34.17
per 1 mol of
−102.5
per 1 mol of
−51.25

Changes in aqueous solution (1)

Reaction of iron(III) phosphate and sulfuric acid
2FePO4Crystalline solid + 3H2SO4Ionized aqueous solution
Fe2(SO4)3Ionized aqueous solution + 2H3PO4Un-ionized aqueous solution
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
−78.9
−39.5
per 1 mol of
−26.3
per 1 mol of
−78.9
per 1 mol of
−39.5

Changes in aqueous solution (2)

Reaction of iron(III) phosphate and sulfuric acid
2FePO4Crystalline solid + 3H2SO4Ionized aqueous solution
Fe2(SO4)3Ionized aqueous solution + 2H3PO4Un-ionized aqueous solution
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
−78.9
−39.5
per 1 mol of
−26.3
per 1 mol of
−78.9
per 1 mol of
−39.5

Changes in aqueous solution (3)

Reaction of iron(III) phosphate and sulfuric acid
2FePO4Crystalline solid + 3H2SO4Ionized aqueous solution
Fe2(SO4)3Ionized aqueous solution + 2H3PO4Ionized aqueous solution
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
−57.0
−28.5
per 1 mol of
−19.0
per 1 mol of
−57.0
per 1 mol of
−28.5

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
FePO4 (cr)-1297.5[1]
FePO4 (cr)
2 hydrate
strengite
-1888.2[1]-1657.5[1]171.25[1]180.54[1]
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
* (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution

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
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[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, (l):Liquid, (ao):Un-ionized aqueous solution

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)