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Na2O + 2H2SO4 → 2NaHSO4 + H2O

The reaction of sodium oxide and sulfuric acid yields sodium hydrogensulfate and water (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

Reaction of basic oxide and acid
Basic oxideBrønsted base + AcidBrønsted acid
SaltConjugate base + H2OConjugate acid

Oxidation state of each atom

Reaction of sodium oxide and sulfuric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide1
Brønsted base
Basic oxide
Strongly basic oxide
H2SO4Sulfuric acid2
Brønsted acid
Acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaHSO4Sodium hydrogensulfate2
Conjugate base
Salt
Salt of strong acid and strong base
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of sodium oxide and sulfuric acid
ΔrG−467.3 kJ/mol
K7.37 × 1081
pK−81.87
Na2OCrystalline solid + 2H2SO4Liquid
2NaHSO4Crystalline solid + H2OLiquid
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
−494.6−467.3−93.0
per 1 mol of
−494.6−467.3−93.0
per 1 mol of
−247.3−233.7−46.5
−247.3−233.7−46.5
per 1 mol of
−494.6−467.3−93.0

Changes in aqueous solution

Reaction of sodium oxide and sulfuric acid
ΔrG−408.21 kJ/mol
K3.28 × 1071
pK−71.52
Na2OCrystalline solid + 2H2SO4Ionized aqueous solution
2NaHSO4Ionized aqueous solution + H2OLiquid
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
−307.99−408.21336.3516
per 1 mol of
−307.99−408.21336.3516
per 1 mol of
−154.00−204.10168.2258
−154.00−204.10168.2258
per 1 mol of
−307.99−408.21336.3516

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
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[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, (g):Gas, (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
NaHSO4 (cr)-1125.5[1]-992.8[1]113.0[1]
NaHSO4 (ai)-1127.46[1]-1017.80[1]190.8[1]-38[1]
NaHSO4 (cr)
1 hydrate
-1421.7[1]-1231.6[1]155[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, (ai):Ionized aqueous solution, (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)