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6H2SO4 + P4O10 🔥→ 6SO3 + 4H3PO4

The reaction of sulfuric acid and tetraphosphorus decaoxide yields sulfur trioxide and phosphoric acid. 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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SO4Sulfuric acid6
Lewis base
Oxoacid
P4O10Tetraphosphorus decaoxide1
Lewis acid
Dehydrating acidic oxide

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO3Sulfur trioxide6
Acidic oxide
H3PO4Phosphoric acid4
Lewis conjugate
Oxoacid

Thermodynamic changes

Changes in standard condition (1)

Reaction of sulfuric acid and tetraphosphorus decaoxide
ΔrG118.8 kJ/mol
K0.15 × 10−20
pK20.81
6H2SO4Liquid + P4O10Crystalline solidhexagonal
🔥
6SO3Liquid + 4H3PO4Crystalline 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
105.7118.8−45.5
per 1 mol of
17.6219.80−7.58
105.7118.8−45.5
per 1 mol of
17.6219.80−7.58
per 1 mol of
26.4329.70−11.4

Changes in standard condition (2)

Reaction of sulfuric acid and tetraphosphorus decaoxide
6H2SO4Liquid + P4O10Amorphous solid
🔥
6SO3Liquid + 4H3PO4Crystalline 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
164
per 1 mol of
27.3
164
per 1 mol of
27.3
per 1 mol of
41.0

Changes in aqueous solution (1)

Reaction of sulfuric acid and tetraphosphorus decaoxide
ΔrG349.5 kJ/mol
K0.59 × 10−61
pK61.23
6H2SO4Ionized aqueous solution + P4O10Crystalline solidhexagonal
🔥
6SO3Crystalline solidβ + 4H3PO4Un-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
559.2349.5707.5
per 1 mol of
93.2058.25117.9
559.2349.5707.5
per 1 mol of
93.2058.25117.9
per 1 mol of
139.887.38176.9

Changes in aqueous solution (2)

Reaction of sulfuric acid and tetraphosphorus decaoxide
ΔrG349.5 kJ/mol
K0.59 × 10−61
pK61.23
6H2SO4Ionized aqueous solution + P4O10Crystalline solidhexagonal
🔥
6SO3Crystalline solidβ + 4H3PO4Un-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
559.2349.5707.5
per 1 mol of
93.2058.25117.9
559.2349.5707.5
per 1 mol of
93.2058.25117.9
per 1 mol of
139.887.38176.9

Changes in aqueous solution (3)

Reaction of sulfuric acid and tetraphosphorus decaoxide
ΔrG844.8 kJ/mol
K0.99 × 10−148
pK148.00
6H2SO4Ionized aqueous solution + P4O10Crystalline solidhexagonal
🔥
6SO3Crystalline solidβ + 4H3PO4Ionized 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
603.0844.8−806.5
per 1 mol of
100.5140.8−134.4
603.0844.8−806.5
per 1 mol of
100.5140.8−134.4
per 1 mol of
150.8211.2−201.6

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
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]
P4O10 (cr)
hexagonal
-2984.0[1]-2697.7[1]228.86[1]211.71[1]
P4O10 (am)-3042[1]
* (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution, (am):Amorphous solid

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
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]
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, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (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)